Transcript

1 OPTION I Instructions for the execution of the work The examination work consists of two parts, including 34 tasks. Part 1 contains 29 tasks with a short answer, part 2 contains 5 tasks with a detailed answer. 3.5 hours (210 minutes) are allocated for the examination work in chemistry. The answer to the tasks of part 1 is a sequence of numbers or a number. Write the answer according to the samples below in the answer field in the text of the work, and then transfer it to the answer form 1. Write down the sequence of numbers in tasks 1 26 without spaces, commas and other additional symbols. Part 1 The answer to tasks 1 26 is a sequence of numbers. Write the answer in the answer field in the text of the work, and then transfer it to the ANSWER FORM 1 to the right of the number of the corresponding task, starting from the first cell. Write the sequence of numbers without spaces, commas and other additional characters. Write each character in a separate box in accordance with the samples given in the form. The numbers in the answers to tasks 5, 10 12, 18, 19 can be repeated. To complete tasks 1 3 use the following row of chemical elements. The answer in tasks 1 3 is a sequence of numbers, under which the chemical elements in this row are indicated. 1) Al 2) O 3) F 4) N 5) S CMM Form 1 Determine the atoms of which two of the indicated elements in the ground state have one unpaired electron at the external energy level. Write down the numbers of the selected elements in the answer field. 3.4. Answers to the tasks include a detailed description of the entire progress of the task. In answer form 2, indicate the problem number and write down its complete solution. All USE forms are filled in with bright black ink. The use of a gel, or capillary, or fountain pen is allowed. When completing assignments, you can use the draft. Draft entries do not count towards grading work. When doing the work, use the Periodic Table of Chemical Elements D.I. Mendeleev, table of solubility of salts, acids and bases in water, electrochemical series of metal voltages. These accompanying materials are attached to the text of the work. Use a non-programmable calculator for calculations. The points received by you for completed tasks are summed up. Try to complete as many tasks as possible and score the most points. We wish you success! 2 3 From the listed chemical elements, select three elements that are in the Periodic Table of Chemical Elements of D.I. Mendeleev are in the same period. Arrange the selected elements in ascending order of their highest oxidation state. Write down the numbers of the selected elements in the required sequence in the answer field. From among the elements indicated in the row, select two elements that exhibit the lowest oxidation state equal to 2. Write down the numbers of the selected elements in the answer field.

2 4 From the proposed list, select two compounds in which only ionic chemical bond... 1) LiH 2) NaCl 3) SO 2 4) CO 5) Na 2 O 2 Write down the numbers of the selected compounds in the answer field. 7 From the list provided, select two oxides that react with sulfuric acid solution, but do not react with sodium hydroxide solution. 1) NO 2) SO 2 3) CuO 4) MgO 5) ZnO 5 Establish a correspondence between the formula of a substance and the class / group to which this substance belongs: for each position marked with an 8 letter, select the corresponding position marked digit. 6 FORMULA OF SUBSTANCE A) CO B) CO 2 C) Cu 2 O CLASS / GROUP 1) acidic oxide 2) basic oxide 3) amphoteric oxide 4) non-salt-forming oxide Select two substances from the list of proposed substances, with each of which copper interacts. 1) calcium chloride (p p) 2) concentrated hydrochloric acid 3) oxygen 4) iron (III) chloride (p-p) 5) diluted sulphuric acid A B C 9 A few drops of a solution of substance Y were added to a test tube with a solution of salt X. As a result of the reaction, a gel-like precipitate formed. From the proposed list, select substances X and Y that can enter into the described reaction. 1) KOH 2) HCl 3) Cu (NO 3) 2 4) K 2SO 3 5) Na 2SiO 3 Write down the numbers of the selected substances in the table under the appropriate letters. The following scheme of transformations of substances is set: NaOH Y AgNO 3 X OH Determine which of the indicated substances are substances X and Y. 1) NH 4 NO 3 2) NH 3 H 2 O 3) AgOH 4) Ag 2 O 5) HNO 3 Write down in the table with the numbers of the selected substances under the corresponding letters.

3 10 Set the correspondence between the reaction equation and the change in the oxidation state of the oxidizing agent. THE EQUATION OF REACTION CHANGE IN THE DEGREE OF OXIDATION OF THE OXIDANT A) 2NH 3 + 2K \u003d 2KNH 2 + H 2 1) 1 0 B) H 2 S + 2K \u003d K 2 S + H 2 2) +2 0 C) 4NH 3 + 6NO \u003d 5N 2 + 6H 2 O 3) +1 0 D) 2H 2 S + 3O 2 \u003d 2SO 2 + 2H 2 O 4) 0 2 5) Establish a correspondence between the name of the substance and the class / group to which this substance belongs: for each position marked with a letter, select the corresponding position marked with a number. NAME OF SUBSTANCE A) ethyl nitrate B) isopropylbenzene C) nitroglycerin CLASS / GROUP 1) aldehydes 2) esters 3) hydrocarbons 4) polyhydric alcohols A B C 11 Establish a correspondence between the formula of the substance and the reagents with each of which this substance can interact: for each position marked with a letter, select the corresponding position marked with a number. FORMULA OF THE SUBSTANCE REAGENTS A) Sodium oxide 1) CO 2, H 2 S, H 2 O B) Silicon (IV) oxide 2) HF, CaCO 3, KOH C) Iron (II) oxide 3) NaOH, FeO, H 2 D ) Carbon monoxide (II) 4) HNO 3, O 2, CO 5) H 2 O, K 2 CO 3, Cl From the proposed list, select two substances that are structural isomers of propanol-1. 1) isopropanol 2) methylethyl ether 3) propyl acetate 4) propyl formate 5) dipropyl ether From the list provided, select two substances that interact with a cold neutral solution of potassium permanganate. 1) ethylene glycol 2) ethanol 3) ethyne 4) ethene 5) ethanic acid

4 15 16 From the proposed list, select two substances with which sodium hydroxide solution reacts 1) ethyl acetate 2) methanol 3) phenol 4) potassium acetate 5) aniline From the proposed list, select two substances with which aminoacetic acid reacts. 18 Establish a correspondence between the name of the substance and the product that is predominantly formed when this substance interacts with water: for each position marked with a letter, select the corresponding position marked with a number. NAME OF SUBSTANCE INTERACTION PRODUCT A) butene-1 1) butanol-1 B) butene-2 \u200b\u200b2) butanol-2 C) butyne-1 3) dibutyl ether D) butyne-2 4) butanal 5) butanone 6) butanediol-1, 2 1) ethylene 2) calcium hydroxide 3) hydrogen 4) aminopropionic acid 5) silicon oxide 17 The following transformation scheme is set: CH 3 CH 2 CH 2 Cl A CH 3 CH 2 COH Determine which of the indicated substances are substances X and Y 1) NaOH (alcohol) 2) NaOH (aq) 3) Cu (OH) 2 4) CuO 5) HCl Write down the numbers of the selected substances in the table under the appropriate letters. 19 Establish a correspondence between the reactants and the carbon-containing product, which is formed by the interaction of these substances: for each position marked with a letter, select the corresponding position marked with a number. REACTANTS A) ethanol and sodium B) methanal and ammonia solution silver oxide B) methanol and acetic acid D) metanoic acid and sodium oxide PRODUCT OF INTERACTION 1) formaldehyde 2) formyl acetate 3) sodium formate 4) methyl acetate 5) ammonium formate 6) sodium ethylate

5 20 From the proposed list of reactions select two reactions proceeding by the ionic mechanism. 1) CH 4 + O 2 2) C 3 H 8 + Br 2 3) C 6 H 6 + Br 2 H 2O 2 4) CH 3 CH \u003d CH 2 + Br 2 5) CH 3 CH \u003d CH 2 + Br 2 (rr) Write down the numbers of the selected types of reactions in the answer field. 23 Establish a correspondence between the salt formula and the ratio of this salt to hydrolysis: for each position marked with a letter, select the corresponding position marked with a number. SALT FORMULA A) Ba (ClO 4) 2 B) NaHCO 3 C) K 2 Se D) HgF 2 RELATIONSHIP TO HYDROLYSIS 1) hydrolyzes according to cation 2) hydrolyzes according to anion 3) does not undergo hydrolysis 4) hydrolyzes according to cation and anion 21 Of the proposed list of external influences, select two influences that lead to an increase in the rate of reaction of carbon monoxide (ii) with oxygen. 1) Increasing oxygen concentration 2) Increasing concentration of carbon monoxide (iv) 3) Increasing temperature 4) decreasing concentration of carbon monoxide (iv) Match the equation chemical reaction and the direction of the displacement of the chemical equilibrium with increasing pressure in the system: for each position indicated by a letter, select the corresponding position indicated by a number. REACTION EQUATION DIRECTION OF DISPLACEMENT OF CHEMICAL EQUILIBRIUM A) 2SO 2 (g) + O 2 (g) 2SO 3 (d) 5) decrease in the concentration of carbon monoxide (ii) B) C 2 H 4 (d) + H 2 (d) C 2 H 6 (g) 1) shifts towards the direct reaction B) H2 (g) + Br 2 (g) 2HBr (g) 2) shifts towards the reverse reaction Write down the numbers of the selected external influences in the answer field. D) 4HCl (g) + O 2 (g) 2Cl 2 (g) + 2H 2 O (g) 3) there is no displacement of equilibrium 22 Establish a correspondence between the salt formula and the electrolysis products of an aqueous solution of this salt, which were released at the anode: For each position marked with a letter, select the corresponding position marked with a number. SALT FORMULA A) Sn (NO 3) 2 B) KI C) CaBr 2 ELECTROLYSIS PRODUCTS 1) hydrogen 2) oxygen 3) metal D) ZnSO 4 4) halogen 5) sulfur oxide (IV) Establish a correspondence between the names of two substances and the reagent , with which you can distinguish between these substances: for each position marked with a letter, select the corresponding position indicated by the number NAMES OF SUBSTANCES REAGENT A) propanol-2 and glycerin 1) K 2 SO 4 (solution) B) propyne and butyne-2 2) OH (solution) B) phenol and acetone 3) Cu (OH) 2 (freshly precipitated) D) ethyl acetate and ethanol 4) KOH (solution) 5) K

6 26 Establish a correspondence between the substance and its area of \u200b\u200bapplication: for each position indicated by a letter, select the corresponding position indicated by a number. SUBSTANCE FIELD OF APPLICATION A) terephthalic acid 1) production of fertilizers B) nitrobenzene 2) as fuel C) synthesis gas 3) production of aluminum D) vinyl chloride 4) production of polymers 5) production of dyes Part 2 Use ANSWER FORM 2 to record answers to tasks Write down first the task number (30, 31, etc.), and then its detailed solution. Write down the answers clearly and legibly. Write the reaction equation using the electronic balance method for calculating the coefficients: Cr 2 O 3 + KBrO 3 + CO Determine the oxidizing agent and reducing agent. Sulfur was fused with iron. The reaction product was dissolved in hydroiodic acid. The evolved gas was burned in an excess of oxygen. The combustion product was absorbed in an aqueous solution of ferrous sulfate (iii). Write the equations for the four reactions described. 32 Write the reaction equations with which you can carry out the following transformations: The answer to the tasks is a number. Write this number in the answer field in the text of the work, while observing the specified degree of accuracy. Then transfer this number to ANSWER FORM 1 to the right of the number of the corresponding task, starting with the first cell. Write each character in a separate box in accordance with the samples given in the form. It is not necessary to write the units of measurement of physical quantities. In 100 g of water at 20 ° C, 31.6 g of potassium nitrate can dissolve. Calculate the mass fraction of salt in a saturated solution at a given temperature. % (Write down the number to the nearest whole.) Calculate the volume of air (n.o.) required to burn 10 liters of methane (n.o.). l. (Write down the number to the nearest whole.) Calculate the mass of oxygen (in grams) required to calcine 9.7 g of zinc sulfide. d. (Write down the number to the nearest tenths.) Do not forget to transfer all answers to answer form 1 in accordance with the instructions for performing work C t, cat. huts H 2, cat. O 2, t, cat. NH 3 CH 4 X 1 vinyl acetylene X 2 ethanic acid X 3 When writing the reaction equations, use the structural formulas of organic substances. When silver was dissolved in 100 g of a 31.5% solution of nitric acid, the mass fraction of the acid decreased to 6.3%. Determine the mass of dissolved silver. In the answer, write down the reaction equations that are indicated in the condition of the problem, and provide all the necessary calculations (indicate the units of measurement of the desired physical quantities). When burning a sample of some organic compound weighing 1.32 g, 1.232 liters of carbon dioxide (n.o. ) 0.45 ml of water and 0.69 g of potassium carbonate. When passing an excess of carbon dioxide through a solution of this substance, turbidity is observed Based on the given conditions of the task: 1) make the calculations necessary to establish the molecular formula organic matter (indicate the units of measurement of the sought physical quantities); 2) write down the molecular formula of the original organic matter; 3) make up the structural formula of this substance, which uniquely reflects the order of bonds of atoms in its molecule. 4) write the equation for the reaction of this substance with an excess of carbon dioxide in this solution, using the structural formula of the substance ..

7 Part 1 KIM OPTION II Instructions for the execution of the work The examination work consists of two parts, including 34 tasks. Part 1 contains 29 tasks with a short answer, part 2 contains 5 tasks with a detailed answer. 3.5 hours (210 minutes) are allocated for the examination work in chemistry. The answer to the tasks of part 1 is a sequence of numbers or a number. Write the answer according to the samples below in the answer field in the text of the work, and then transfer it to the answer form 1. Write down the sequence of numbers in tasks 1 26 without spaces, commas and other additional characters Form 1 The answer to tasks 1 26 is a sequence of numbers. Write down the answer in the answer field in the text of the work, and then transfer it to the ANSWER FORM 1 to the right of the number of the corresponding task, starting from the first cell. Write the sequence of numbers without spaces, commas and other additional characters. Write each character in a separate box in accordance with the samples given in the form. The numbers in the answers to tasks 5, 10 12, 18, 19 can be repeated. To complete tasks 1 3 use the following row of chemical elements. The answer in tasks 1 3 is a sequence of numbers, under which the chemical elements in this row are indicated. 1) Al 2) O 3) F 4) N 5) S Determine which atoms of which two of the elements indicated in the series have electrons in the ground state at three energy levels. Write down the numbers of the selected elements in the answer field. 3.4. Answers to the tasks include a detailed description of the entire progress of the task. In answer form 2, indicate the task number and write down its complete solution. All USE forms are filled in with bright black ink. The use of a gel, or capillary, or fountain pen is allowed. When completing assignments, you can use the draft. Draft entries do not count towards grading work. When performing work, use the Periodic Table of Chemical Elements D.I. Mendeleev, table of solubility of salts, acids and bases in water, electrochemical series of metal voltages. These accompanying materials are attached to the text of the work. Use a non-programmable calculator for calculations. The points received by you for completed tasks are summed up. Try to complete as many tasks as possible and score the most points. We wish you success! 2 3 From the listed chemical elements, select three elements that are in the Periodic Table of Chemical Elements of D.I. Mendeleev are in the same period. Arrange the selected elements in ascending order of their valence in the volatile hydrogen compound. Write down the numbers of the selected elements in the required sequence in the answer field. From among the items listed in the row, select two items that are electronic counterparts. Write down the numbers of the selected elements in the answer field.

8 4 From the proposed list, select two compounds in which only a covalent polar chemical bond is present. 1) LiH 2) NH 4 Cl 3) SO 2 4) CO 5) Na 2 O 2 Write down the numbers of the selected compounds in the answer field. 7 From the list provided, select two oxides that react with sulfuric acid solution, but do not react with sodium hydroxide solution. 1) CO 2) P 2 O 5 3) FeO 4) Al 2 O 3 5) CuO 5 Establish a correspondence between the formula of a substance and the class / group to which this substance belongs: to each position designated by the 8 letter, select the appropriate position indicated by the number. 6 FORMULA OF SUBSTANCE A) Na 2 ZnO 2 B) NH 4 MgPO 4 C) (CuOH) 2 CO 3 CLASS / GROUP 1) medium salt 2) acidic salt 3) double salt 4) basic salt From the proposed list of substances, select two substances, with which zinc does not react. 1) potassium hydroxide (p p) 2) aluminum chloride (p p) 3) calcium chloride (p-p) 4) lithium sulfate (p-p) 5) hydrochloric acid A B C 9 Several were added to the test tube with a solution of salt X drops of a solution of substance Y. As a result of the reaction, the evolution of a colorless gas with a pungent odor was observed. From the proposed list, select substances X and Y that can enter into the described reaction. 1) KOH 2) HCl 3) Cu (NO 3) 2 4) K 2SO 3 5) Na 2SiO 3 Write down the numbers of the selected substances in the table under the appropriate letters. The following scheme of transformations of substances is set: KOH (solution) XY Fe (OH) 3 Determine which of the indicated substances are substances X and Y. 1) FeCl 3 2) FeSO 4 3) Fe (OH) 2 4) FeO 5) Fe 2 O 3 Write down the numbers of the selected substances in the table under the appropriate letters.

9 10 Establish a correspondence between the scheme of transformations and the formulas of the substances in the interaction of which they occur: for each position indicated by a letter, select the corresponding position indicated by a number. SCHEME OF TRANSFORMATIONS A) Fe +2 Fe 0 B) Fe +2 Fe +3 C) Fe 0 Fe +2 D) Fe 0 Fe +3 SUBSTANCES 1) FeO and H 2 2) Fe and H 2 SO 4 (pp) 3 ) Fe and Cl 2 4) Fe (OH) 2 and H 2 O 2 12 Establish a correspondence between the name of the substance and the class / group to which this substance belongs: for each position marked with a letter, select the corresponding position marked digit. NAME OF SUBSTANCE A) trimethylamine B) nitroethane C) nitroglycerin CLASS / GROUP 1) primary amines 2) tertiary amines 3) esters 4) nitro compounds 5) Fe 2 O 3 and H 2 SO 4 A B C 11 Set the correspondence between the formula of the substance and reagents, with each of which this substance can interact: for each position indicated by a letter, select the corresponding position indicated by a number. FORMULA OF THE SUBSTANCE REAGENTS A) Al 1) MgCl 2, HNO 3 (conc.), HBr B) Fe 2) CuCl 2, HNO 3 (dil.), H 2 SO 4 (dil.) C) S 3) CuO, Si , H 2 D) C 4) H 2 SO 4 (conc.), NaOH, H 2 5) NaOH (solution), HCl (solution), Al (NO 3) From the list, select two pairs of substances, which are homologues. 1) ethyl acetate and methyl acetate 2) benzene and phenol 3) methylamine and phenylamine 4) methylpropane and 2-methylpentane 5) acetylene and vinyl acetylene From the list proposed, select two substances that cannot be isolated from a mixture of 1-propanol and concentrated sulfuric acid. 1) propanol-2 2) propanone 3) propylene 4) dipropyl ether 5) propyne

10 15 16 From the proposed list, select two substances with which glycerin reacts. 1) benzene 2) copper (II) hydroxide 3) sodium 4) hydrogen 5) dimethyl ketone From the proposed list, select two substances with which methylamine reacts. 18 Establish a correspondence between the name of the substance and the product that is predominantly formed by the interaction of this substance with hydrogen bromide under normal conditions: for each position marked with a letter, select the corresponding position marked with a number. NAME OF SUBSTANCE INTERACTION PRODUCT А) butene-1 1) 2-bromobutane B) butene-2 \u200b\u200b2) 1-bromobutane C) butadiene-1,3 3) 1-bromobutene-2 \u200b\u200bD) butyne-1 4) 2-bromobutene-1 5) 1,2-dibromobutene 6) 1,1-dibromobutane 1) acetic acid 2) ethane 3) benzene 4) chloromethane 5) sodium hydroxide 17 The following conversion scheme is set: NaOH, spl substances are substances X and Y. 1) Na 2 CO 3 2) CO 2 3) CH 4 4) C 2 H 2 5) H 2 O Write down the numbers of the selected substances in the table under the appropriate letters. 19 Establish a correspondence between the reactants and the carbon-containing product, which is formed by the interaction of these substances: for each position marked with a letter, select the corresponding position marked with a number. REACTING SUBSTANCES A) ethyl acetate and potassium hydroxide B) potassium acetate and sulfuric acid C) propanal and copper hydroxide (ii) D) propanol-2 and acidified solution of potassium permanganate INTERACTION PRODUCT 1) ethanic acid 2) potassium acetate 3) propanol-1 4 ) propanone 5) propanoic acid 6) potassium propionate

11 20 From the proposed list of reactions select two reactions proceeding by the radical mechanism. 1) CH 4 + HNO 3 2) C 3 H 8 + Br 2 3) C 2 H 4 + H 2 O 4) CH 3 CH \u003d CH 2 + Br 2 (solution) 5) C 6 H 6 + HNO 3 Write down the numbers of the selected reaction types in the answer field. 21 From the proposed list of external influences, select two influences that lead to a decrease in the rate of reaction of ethylene with hydrogen. 1) lowering the temperature 2) increasing the concentration of ethylene 3) using a catalyst 4) decreasing the concentration of hydrogen 5) increasing the pressure in the system Write down the numbers of the selected external influences in the answer field. 22 Establish a correspondence between the salt formula and the products of electrolysis of an aqueous solution of this salt, which precipitated on inert electrodes: for each position marked with a letter, select the corresponding position marked with a number. SALT FORMULA ELECTROLYSIS PRODUCTS A) AlCl 3 1) H 2, O 2 B) NaCl 2) H 2, Cl 2 C) CuCl 2 3) Cu, O 2 D) CuSO 4 4) Cu, Cl 2 5) Al, Cl 2 23 Establish a correspondence between the salt formula and the ratio of this salt to hydrolysis: for each position marked with a letter, select the corresponding position marked with a number. 24 SALT FORMULA A) KCl B) Cr (NO 3) 3 C) Sr (CH 3 COO) 2 D) CH 3 COONH 4 RELATIONSHIP TO HYDROLYSIS 1) hydrolyzed by cation 2) hydrolyzed by anion 3) does not undergo hydrolysis 4) hydrolyzes by cation and anion Set the correspondence between the external effect on the equilibrium system Na 2 CO 3 + H 2 O NaOH + NaHCO 3 and the direction of the shift of the chemical equilibrium: to each position marked with a letter, select the corresponding position indicated by a number. EQUATION OF REACTION A) increasing the temperature B) diluting the solution with water C) adding hydrochloric acid D) adding sodium hydroxide DIRECTION OF THE CHEMICAL EQUILIBRIUM DISPLACEMENT 1) shifts towards the forward reaction 2) shifts towards the reverse reaction 3) there is no displacement of equilibrium 25 Match the formulas substances and a reagent with which you can distinguish between their aqueous solutions: for each position indicated by a letter, select the corresponding position indicated by a number. FORMULAS OF SUBSTANCES REAGENT A) Al (NO 3) 3 and Ca (NO 3) 2 1) AlCl 3 (solution) B) Na 3 PO 4 and Na 2 SO 4 2) Br 2 C) HCl and K 2 SO 4 3) HCl D) KI and NaNO 3 4) KOH (solution) 5) BaCl 2 (solution)

12 26 Establish a correspondence between the substance and its area of \u200b\u200bapplication: for each position indicated by a letter, select the corresponding position indicated by a number. SUBSTANCE FIELD OF APPLICATION A) phosphorite 1) production of fertilizers B) phenol 2) as fuel C) methane 3) production of polymers D) chloroprene 4) as a solvent 5) in blast furnace production Part 2 Use ANSWER FORM 2 to record answers to tasks. First, write down the task number (30, 31, etc.), and then its detailed solution. Write down the answers clearly and legibly. Make a reaction equation using the electronic balance method for setting the coefficients: CrCl 2 + K 2 Cr 2 O 7 + CrCl H 2 O Determine the oxidizing agent and reducing agent. Aluminum oxide was fused with potassium hydroxide. The reaction product was introduced into the ammonium chloride solution. The evolved gas was passed through a sulfuric acid solution. The resulting middle salt was calcined. Write the equations for the four reactions described. 32 Write the reaction equations, with the help of which you can carry out the following transformations: 27 The answer to the tasks is a number. Write this number in the answer field in the text of the work, while observing the specified degree of accuracy. Then transfer this number to ANSWER FORM 1 to the right of the number of the corresponding task, starting with the first cell. Write each character in a separate box in accordance with the samples given in the form. It is not necessary to write the units of measurement of physical quantities. Calculate the volume of a sulfuric acid solution with a mass fraction of 8% and a density of 1.05 g / ml required to prepare 200 g of a 2% sulfuric acid solution. ml (Write down the number to the nearest tenth.) 33 KOH alcohol. Cl 2, 500 C NaOH, sol. KMnO 4, H 2O, 0 C HNO 3 (conc.), H 2SO 4 (conc.) X 1 propene X 2 X 3 X 4 X 5 When writing reaction equations, use the structural formulas of organic substances. Bertoleth's salt weighing 45 g was calcined in the presence of a catalyst. In the released gas, 7.2 g of carbon were burned. The resulting gas mixture was passed through an excess of calcium hydroxide solution. Dropped 40 g of sediment. How much salt decomposed without gas evolution? In the answer, write down the reaction equations that are indicated in the condition of the problem, and provide all the necessary calculations (indicate the units of measurement of the sought physical quantities) Volume of oxygen (n.u.) remaining after combustion of 20 liters of ammonia (n.u.) in 20 liters of oxygen (Well.). l (Write down the number to the nearest whole.) Calculate the mass of chlorine (in grams) required to react with 28 g of iron. d. (Write down the number to the nearest hundredth.) Do not forget to transfer all answers to answer form 1 in accordance with the instructions for the work. 34 When a 5.6 g sample of some organic compound was burned, 17.6 g of carbon dioxide and 7.2 ml of water were obtained. The vapor density of this substance at normal level is 2.5 g / l. It is known that when this substance interacts with hydrogen on a platinum catalyst, two isomeric reaction products are formed. Based on the given conditions of the assignment: 1) make the calculations necessary to establish the molecular formula of organic matter (indicate the units of measurement of the sought physical quantities); 2) write down the molecular formula of the original organic matter; 3) make up the structural formula of this substance, which uniquely reflects the order of bonds of atoms in its molecule. 4) Write the equation for the hydrogenation reaction of this substance with the formation of a reaction product with a branched carbon skeleton, using the structural formula of the substance.

13 Part 1 KIM OPTION III Instructions for performing the work The examination work consists of two parts, including 34 tasks. Part 1 contains 29 tasks with a short answer, part 2 contains 5 tasks with a detailed answer. 3.5 hours (210 minutes) are allocated for the examination work in chemistry. The answer to the tasks of part 1 is a sequence of numbers or a number. Write the answer according to the samples below in the answer field in the text of the work, and then transfer it to the answer form 1. Write down the sequence of numbers in tasks 1 26 without spaces, commas and other additional characters Form 1 The answer to tasks 1 26 is a sequence of numbers. Write the answer in the answer field in the text of the work, and then transfer it to the ANSWER FORM 1 to the right of the number of the corresponding task, starting from the first cell. Write down the sequence of numbers without spaces, commas and other additional characters. Write each character in a separate box in accordance with the samples given in the form. The numbers in the answers to tasks 5, 10 12, 18, 19 can be repeated. To complete tasks 1 3 use the following row of chemical elements. The answer in tasks 1 3 is a sequence of numbers, under which the chemical elements in this row are indicated. 1) Al 2) O 3) F 4) N 5) S Determine which atoms of which two of the elements indicated in the series have six electrons in the ground state at the external energy level. Write down the numbers of the selected elements in the answer field. 3.4. Answers to the tasks include a detailed description of the entire progress of the task. In answer form 2, indicate the task number and write down its complete solution. All USE forms are filled in with bright black ink. The use of a gel, or capillary, or fountain pen is allowed. When completing assignments, you can use the draft. Draft entries do not count towards grading work. When doing the work, use the Periodic Table of Chemical Elements of D.I. Mendeleev, table of solubility of salts, acids and bases in water, electrochemical series of metal voltages. These accompanying materials are attached to the text of the work. Use a non-programmable calculator for calculations. The points received by you for completed tasks are summed up. Try to complete as many tasks as possible and score the most points. We wish you success! 2 3 From the listed chemical elements, select three elements that are in the Periodic Table of Chemical Elements of D.I. Mendeleev are in the same period. Arrange the selected elements in ascending order of their electronegativity. Write down the numbers of the selected elements in the required sequence in the answer field. From among the elements listed in the row, select two elements that cannot exhibit the highest oxidation state equal to the group number. Write down the numbers of the selected elements in the answer field.

14 4 From the proposed list, select two compounds in which there is a chemical bond formed by the donor-acceptor mechanism. 1) LiH 2) NH 4 Cl 3) SO 2 4) CO 5) Na 2 O 2 Write down the numbers of the selected compounds in the answer field. 7 From the list provided, select two oxides that react with sulfuric acid solution, but do not react with sodium hydroxide solution. 1) MgO 2) N 2 O 3) CaO 4) SO 3 5) BeO 5 Establish a correspondence between the formula of a substance and the class / group to which this substance belongs: for each position marked with an 8 letter, select the corresponding position indicated by a number. 6 FORMULA OF SUBSTANCE A) Na 2 HPO 4 B) CaCl (OСl) C) Ca (ClO) 2 CLASS / GROUP 1) medium salt 2) acidic salt 3) double salt 4) mixed salt From the proposed list of substances select two substances, with each of which iron reacts under normal conditions. 1) potassium hydroxide (p p) 2) iron (III) chloride (p p) 3) concentrated sulfuric acid 4) concentrated nitric acid 5) diluted hydrochloric acid A B C 9 A few drops of a solution of substance Y were added to a test tube with a solution of salt X As a result of the reaction, the precipitation of a blue flocculent precipitate was observed. From the proposed list, select substances X and Y that can enter into the described reaction. 1) KOH 2) HCl 3) Cu (NO 3) 2 4) K 2SO 3 5) Na 2SiO 3 Write down the numbers of the selected substances in the table under the appropriate letters. The following scheme of substances transformations is set: XYK 2 CO 3 CaCO 3 CO 2 Determine which of the indicated substances are substances X and Y. 1) KOH 2) CaCl 2 3) CaSO 4 4) HCl 5) H 2 O Write down the numbers of the selected substances under the appropriate letters.

15 10 Establish a correspondence between the reaction equation and the property of the element nitrogen, which it manifests in this reaction: for each position marked with a letter, select the corresponding position marked with a number. REACTION EQUATION A) NH 4HCO 3 \u003d NH 3 + H 2O + CO 2 B) 3CuO + 2NH 3 \u003d N 2 + 3Cu + 3H 2O C) 4NH 3 + 5O 2 \u003d 4NO + 6H 2O D) 6Li + N 2 \u003d 2Li 3N PROPERTIES OF NITROGEN 1) is an oxidizing agent 2) is a reducing agent 3) is both an oxidizing agent and a reducing agent 4) does not exhibit redox properties 12 Set a correspondence between the name of the substance and its formula: for each position indicated by a letter, select the corresponding position indicated by a number. NAME OF SUBSTANCE A) aniline B) phenylamine C) aminobenzene FORMULA 1) C 6 H 5 CH 2 OH 2) C 6 H 5 NH 2 3) C 6 H 5 NO 2 4) C 6 H 5 COONH 2 A B C 11 Set correspondence between the formula of a substance and the reagents, during the interaction of which it is formed: for each position indicated by a letter, select the corresponding position indicated by a number. FORMULA OF SUBSTANCE A) Fe (OH) 3 B) FeCl 2 C) FeCl 3 D) Fe REAGENTS 1) Fe and Cl 2 2) Fe (OH) 2 and H 2 O 2 3) FeO and H 2 4) Fe and HCl 5) Fe 2 O 3 and NaOH From the proposed list, select two substances, all carbon atoms in which are in the state of sp 2 -hybridization 1) toluene 2) benzene 3) divinyl 4) acetaldehyde 5) isoprene From the proposed list, select two substances that interact with hydrogen chloride. 1) butene-2 \u200b\u200b2) cyclopentane 3) toluene 4) methylcyclopropane 5) benzene

16 15 16 From the proposed list, select two substances with which formaldehyde does not interact. 1) phenol 2) ethanol 3) diethyl ether 4) hydrogen 5) nitrogen From the list provided, select two substances with which aniline reacts. 18 Establish a correspondence between the name of the substance and the product, which is predominantly formed by the interaction of this substance with oxygen under appropriate conditions: for each position marked with a letter, select the corresponding position marked with a number. NAME OF SUBSTANCE INTERACTION PRODUCT A) cumene 1) phenol B) ethylene (Ag) 2) ethanol C) ethylene (CuCl 2 / PdCl 2) 3) ethanal D) methane 4) propanol 5) ethylene oxide 6) methanol 1) ammonia 2) bromine 3) oxygen 4) water 5) carbon dioxide 17 The following transformation scheme is set: 19 Establish a correspondence between the reactants HC C CH 3 A CH 3 CHOH CH 3 carbon-containing product that is formed by the interaction of these substances: to each position marked with a letter, select Determine which of the specified substances are substances X and Y. the corresponding position indicated by a number. 1) H 2 O 2) CuO 3) CO 2 4) HCl g. 5) Cl 2 Write down the numbers of the selected substances in the table under the appropriate letters. REACTING SUBSTANCES A) isopropanol and hydrogen iodide B) sodium propionate and hydrogen iodide C) isopropyl acetate and sodium hydroxide D) dipropyl ether and hydrogen iodide INTERACTION PRODUCT 1) 1-iodopropane 2) 2-iodopropane 3) propanoic acid 2 5) propane ) sodium propionate

17 20 From the proposed list of reaction types, select two types of reaction, which include the interaction of nitrogen and hydrogen. 1) catalytic 2) endothermic 3) irreversible 4) redox 5) neutralization reaction Write down the numbers of the selected types of reactions in the answer field. 21 From the proposed list of external influences, select two influences that lead to a decrease in the rate of interaction of sulfur (iv) oxide and oxygen. 1) increase in pressure 2) increase in temperature 3) no addition a large number nitric oxide (II) 4) decrease in temperature 5) decrease in oxygen concentration Write down the numbers of the selected external influences in the answer field. 22 Establish a correspondence between the formula of the salt and the electrolysis products of an aqueous solution of this salt, which precipitated on the anode: for each position marked with a letter, select the corresponding position marked with a number. SALT FORMULA A) CH 3 CH 2 COONa ELECTROLYSIS PRODUCTS 1) O 2 B) Na 2 CO 3 2) CO 2, C 4 H 10 C) Cu (NO 3) 3 3) NO 2 D) FeSO 4 4) SO 2 5) CO 2 23 Set the correspondence between the salt formula and the medium of an aqueous solution of this salt: for each position marked with a letter, select the corresponding position marked with a number. 24 SALT FORMULA A) NaClO 4 B) AlCl 3 C) K 2 SiO 3 D) K 2 CO 3 SOLUTION MEDIUM 1) acidic 2) alkaline 3) neutral Set the correspondence between the external effect on the equilibrium system Na 3 PO 4 + H 2 O NaOH + Na 2 HPO 4 and the direction of the displacement of the chemical equilibrium: for each position marked with a letter, select the corresponding position marked with a number. EQUATION OF REACTION A) increasing the temperature B) diluting the solution with water C) adding hydrochloric acid D) adding sodium hydroxide substances and a reagent with which you can distinguish between these substances: for each position indicated by a letter, select the corresponding position indicated by a number. SUBSTANCES REAGENT A) benzene and hexene 1) bromic water B) butyne-1 and butyne-2 2) phenolphthalein C) cyclohexane and cyclohexene 3) hydrochloric acid D) propionic acid and 4) sodium carbonate solution propanol 5) ammonia solution of silver oxide

18 26 Establish a correspondence between the substance and its area of \u200b\u200bapplication: for each position indicated by a letter, select the corresponding position indicated by a number. SUBSTANCE FIELD OF APPLICATION A) cryolite 1) production of fertilizers B) ammonia 2) in blast furnace process C) aminocaproic acid 3) production of aluminum D) coke 4) production of polymers 5) as a solvent Part 2 Use ANSWER FORM 2 to record answers to tasks. Write down the task number first (30, 31, etc.), and then its detailed solution. Write down the answers clearly and legibly. Make a reaction equation using the electronic balance method for setting the coefficients: P 2 O 3 + H 2 Cr 2 O 7 + H 3 PO 4 + CrPO 4 Determine the oxidizing agent and reducing agent. A mixture of aluminum and iron oxide was set on fire. The resulting mixture was added after cooling to an excess of potassium hydroxide solution. The resulting reaction mixture was filtered. The filtrate was treated with an ammonium chloride solution. The solid remaining on the filter was burned in chlorine. Write the equations for the four reactions described. The answer to the tasks is a number. Write this number in the answer field in the text of the work, while observing the specified degree of accuracy. Then transfer this number to ANSWER FORM 1 to the right of the number of the corresponding task, starting with the first cell. Write each character in a separate box in accordance with the samples given in the form. It is not necessary to write the units of measurement of physical quantities. Determine the mass of potassium chloride that should be dissolved in 100 g of a solution with a mass fraction of 5% to obtain a solution with a mass fraction of 15% g. (Write the number down to tenths.) Calculate the volume of air (n.o.) combustion of 1 liter of propane (n.o.). l. (Write down the number to the nearest tenths.) Calculate the mass of sulfur (IV) oxide (in grams) formed by the reaction of 16 g of copper with concentrated sulfuric acid. d. (Write down the number to the nearest whole.) Do not forget to transfer all answers to answer form 1 in accordance with the instructions for performing the work. Write the reaction equations with which you can carry out the following transformations: HCl KMnO 4, H +, t NaOH, water. X 1 Ag C C CH 3 X 1 X 2 X 3 CH 4 When writing the reaction equations, use the structural formulas of organic substances. By dissolving 5.85 g of sodium peroxide in hot water, a 4% alkali solution was obtained. Calculate the amount of water used. What is the maximum volume of carbon dioxide that can be absorbed by this alkali solution? In the answer, write down the reaction equations that are indicated in the condition of the problem, and provide all the necessary calculations (indicate the units of measurement of the desired physical quantities). Some organic compound contains 69.6% oxygen by weight. The molar mass of this compound is 1.586 times greater molar mass air. The compound enters into an esterification reaction with propanol-2 Based on the given conditions of the task: 1) make the calculations necessary to establish the molecular formula of organic matter (indicate the units of measurement of the desired physical quantities); 2) write down the molecular formula of the original organic matter; 3) make up the structural formula of this substance, which uniquely reflects the order of bonds of atoms in its molecule. 4) write the equation for the reaction of this substance with propanol-2, using the structural formula of the substance.

19 Part 1 KIM OPTION IV Instructions for the execution of the work The examination work consists of two parts, including 34 tasks. Part 1 contains 29 tasks with a short answer, part 2 contains 5 tasks with a detailed answer. 3.5 hours (210 minutes) are allocated for the examination work in chemistry. The answer to the tasks of part 1 is a sequence of numbers or a number. Write the answer according to the samples below in the answer field in the text of the work, and then transfer it to the answer form 1. Write down the sequence of numbers in tasks 1 26 without spaces, commas and other additional characters Form 1 The answer to tasks 1 26 is a sequence of numbers. Write down the answer in the answer field in the text of the work, and then transfer it to the ANSWER FORM 1 to the right of the number of the corresponding task, starting from the first cell. Write the sequence of numbers without spaces, commas and other additional characters. Write each character in a separate box in accordance with the samples given in the form. The numbers in the answers to tasks 5, 10 12, 18, 19 can be repeated. To complete tasks 1 3 use the following row of chemical elements. The answer in tasks 1 3 is a sequence of numbers, under which the chemical elements in this row are indicated. 1) Al 2) O 3) F 4) N 5) S Determine which atoms of which two of the elements indicated in the series in the ground state have the same number of electrons on four sublevels. Write down the numbers of the selected elements in the answer field. 3.4. Answers to the tasks include a detailed description of the entire progress of the task. In answer form 2, indicate the task number and write down its complete solution. All USE forms are filled in with bright black ink. The use of a gel, or capillary, or fountain pen is allowed. When completing assignments, you can use the draft. Draft entries do not count towards grading work. When performing work, use the Periodic Table of Chemical Elements D.I. Mendeleev, table of solubility of salts, acids and bases in water, electrochemical series of metal voltages. These accompanying materials are attached to the text of the work. Use a non-programmable calculator for calculations. The points received by you for completed tasks are summed up. Try to complete as many tasks as possible and score the most points. We wish you success! 2 3 From the listed chemical elements, select three elements that are in the Periodic Table of Chemical Elements of D.I. Mendeleev are in the same period. Arrange the selected elements in ascending order of the radii of their atoms. Write down the numbers of the selected elements in the required sequence in the answer field. From among the elements indicated in the row, select two elements whose hydrogen compounds form an aqueous solution with ph< 7. Запишите в поле ответа номера выбранных элементов.

20 4 From the list, select two compounds in which a π-bond is present. 1) LiH 2) NH 4 Cl 3) SO 2 4) CO 5) Na 2 O 2 Write down the numbers of the selected compounds in the answer field. 7 From the list provided, select two oxides that react with sulfuric acid solution, but do not react with sodium hydroxide solution. 1) CO 2 2) NO 3) SrO 4) ZnO 5) MgO 5 6 Establish a correspondence between the formula of a substance and the class / group to which this substance belongs: for each position marked with a letter, select the corresponding position marked digit. FORMULA OF THE SUBSTANCE A) H 3 PO 4 B) NO C) BaO 2 CLASS / GROUP 1) salt 2) oxide 3) peroxide 4) hydroxide A B C From the proposed list of substances select two substances with each of which chromium reacts under normal conditions ... 8 A few drops of a solution of substance Y were added to a test tube with a solution of salt X. As a result of the reaction, a brown precipitate formed. From the proposed list, select substances X and Y that can enter into the described reaction. 1) NaOH 2) HCl 3) AgNO 3 4) K 2 SO 4 5) CuCl 2 Write down the numbers of the selected substances in the table under the appropriate letters. 1) potassium hydroxide (p p) 2) diluted hydrochloric acid 3) concentrated sulfuric acid 4) concentrated nitric acid 5) diluted sulfuric acid 9 The following transformation scheme is set: YH 2 S Al (OH) 3 X Al (OH) 3 Determine which of these substances are substances X and Y. 1) NaOH 2) Al 2 O 3 3) Al 2 S 3 4) Na 5) NaAlO 2 Write down the numbers of the selected substances in the table under the corresponding letters.

21 10 Establish a correspondence between the reaction scheme and the oxidizing substance participating in this reaction: for each position marked with a letter, select the corresponding position marked with a number. REACTION DIAGRAM A) Mg + HCl MgCl 2 + H 2 B) CaH 2 + HCl CaCl 2 + H 2 C) Mg + SiO 2 MgO + Si D) CH 3 Cl + Cl 2 CH 2 Cl 2 + HCl OXIDANT 1) Mg 2) HCl 3) SiO 2 4) CaH 2 5) Cl 2 12 Establish a correspondence between the name of the substance and its formula: for each position indicated by a letter, select the corresponding position indicated by a number. NAME OF SUBSTANCE A) alanine B) aniline C) phenylamine FORMULA 1) CH 3 CH (NH 2) COOH 2) C 6 H 5 CH 2 CH (NH 2) COOH 3) C 6 H 5 NH 2 4) C 6 H 5 CH (NH 2) COOH A B C 11 Establish a correspondence between the formula of a substance and the reagents with each of which this substance can interact: for each position marked with a letter, select the corresponding position indicated by a number. FORMULA OF THE SUBSTANCE REAGENTS A) H 2 SO 4 (solution) 1) HNO 3, I 2, NaOH B) HNO 3 (solution) 2) SO 2, Ca (OH) 2, Cr 2 O 3 C) H 2 S 3) Cu, H 2 O, Ba (NO 3) 2 D) HBr 4) Ba (NO 3) 2, Zn, BaCO 3 5) FeS, F 2, AgNO From the proposed list, select two substances in whose molecules there are two π-bonds. 1) vinyl acetylene 2) propadiene 3) propyne 4) methylpropene 5) methanal From the list, select two substances that interact with water under appropriate conditions. 1) cyclopropane 2) propene 3) toluene 4) methylpropane 5) butyne-2

22 15 From the proposed list, select two substances with which glycerin 18 reacts. 16 1) iron 2) iron (III) chloride 3) copper (II) hydroxide 4) nitric acid 5) water From the list provided, select two substances with which aminobutane does not interact. 1) hydrogen chloride 2) ammonia 3) chloroethane 4) ethylene 5) water Establish a correspondence between the name of the substance and the product that is predominantly formed by the interaction of this substance with chlorine during irradiation: for each position indicated by a letter, select the corresponding position indicated by a number. NAME OF SUBSTANCE INTERACTION PRODUCT A) isobutane 1) hexachlorocyclohexane B) benzene 2) chlorocyclohexane C) ethylbenzene 3) 1-ethyl-2-chlorobenzene D) cyclohexane 4) 2-methyl-2-chloropropane 5) 2-1-chlorobutane 6) -1-chloroethane 17 The following transformation scheme is set: t, AlCl 3 CH 3Cl, Na 19 Set the correspondence between the reactants and benzene XY carbon-containing product that is formed during the interaction of these substances: for each position marked with a letter, select Determine which of of these substances are substances X and Y. corresponding position indicated by a number. 1) chlorobenzene 2) hexachlorocyclohexane 3) toluene 4) 1-methyl-3-chlorobenzene 5) ethylbenzene Write down the numbers of the selected substances in the table under the appropriate letters. REACTANTS A) ethylene glycol and hydrogen chloride B) ethanic acid and copper hydroxide (ii) C) ethanal and copper hydroxide (ii) D) methanic acid and copper hydroxide (ii) INTERACTION PRODUCT 1) copper acetate (ii) 2) ethanic acid 3 ) carbon dioxide 4) 1,2-dichloroethane 5) 1,1-dichloroethane 6) ethanol

23 20 From the proposed list of reaction types, select two types of reaction, which include the interaction of sodium hydroxide and nitric acid solutions 1) catalytic 2) homogeneous 3) irreversible 4) redox 5) endothermic Write down the numbers of the selected types of reactions in the response field. 21 From the suggested list of external influences, select two influences that lead to a decrease in the rate of reaction of propylene with hydrogen. 1) lowering the temperature 2) increasing the concentration of ethylene 3) using a catalyst 4) decreasing the concentration of hydrogen 5) increasing the pressure in the system Write down the numbers of the selected external influences in the answer field. 22 Establish a correspondence between the formula of the salt and the electrolysis products of an aqueous solution of this salt, which precipitated on the cathode: for each position marked with a letter, select the corresponding position marked with a number. SALT FORMULA A) AgF ELECTROLYSIS PRODUCTS 1) F 2 B) AlF 3 2) H 2 C) ZnSO 4 3) metal D) AgNO 3 4) metal and hydrogen 5) NO 2 23 Establish a correspondence between the salt formula and the medium of an aqueous solution of this salt: for each position marked with a letter, select the corresponding position marked with a number. SALT FORMULA A) ZnSO 4 B) NH 4 Cl C) AgNO 3 D) Na 2 S SOLUTION MEDIUM 1) acidic 2) alkaline 3) neutral 24 Establish a correspondence between the chemical reaction equation and the direction of displacement of chemical equilibrium with decreasing pressure in the system: For each position marked with a letter, select the corresponding position marked with a number. 25 Establish a correspondence between the formulas of substances and the reagent with which you can distinguish between these substances: for each position marked with a letter, select the corresponding position marked with a number. FORMULAS OF SUBSTANCES REAGENT A) BaSO 3 and BaSO 4 1) HCl (solution) B) CO 2 and O 2 2) H 2 O C) MgCl 2 and AlCl 3 3) KBr (solution) D) SiO 2 and MgO 4) Ca (OH) 2 (solution) 5) NaNO 3 (solution) EQUATION OF REACTION DIRECTION OF DISPLACEMENT OF CHEMICAL EQUILIBRIUM А) C 3 H 8 (g) C 3 H 6 (g) + H 2 (g) 1) shifts towards the direct reaction B) Fe 2 O 3 (s) + CO (g) 2FeO (s) + CO 2 (g) 2) shifts towards the reverse reaction C) CO (g) + Cl 2 (g) COCl 2 (g) 3) no displacement of equilibrium occurs Г) N 2 (g) + 3H 2 (g) 2NH 3 (g)

24 26 Establish a correspondence between the substance and its area of \u200b\u200bapplication: for each position indicated by a letter, select the corresponding position indicated by a number. SUBSTANCE FIELD OF APPLICATION A) carbon tetrachloride 1) as a catalyst B) vanadium (V) oxide 2) in the production of aluminum C) propylene 3) the production of fertilizers D) benzene 4) as a solvent 5) production of polymers Part 2 Use ANSWER FORM 2. Write down first the task number (30, 31, etc.), and then its detailed solution. Write down the answers clearly and legibly. Make a reaction equation using the electronic balance method for calculating the coefficients: K 2 Cr 2 O H 2 SO 4 K 2 SO H 2 O Determine the oxidizing agent and reducing agent. Barium carbonate was calcined at high temperature. The resulting powder was left in air until completely cooled. Then it was brought into the water and carbon dioxide was passed. The resulting suspension was filtered. A solution of sodium iodide acidified with sulfuric acid was added to the filtrate, and the evolution of iodine was observed. Write the equations for the four reactions described. The answer to the tasks is a number. Write this number in the answer field in the text of the work, while observing the specified degree of accuracy. Then transfer this number to ANSWER FORM 1 to the right of the number of the corresponding task, starting with the first cell. Write each character in a separate box in accordance with the samples given in the form. It is not necessary to write the units of measurement of physical quantities. Calculate the mass of water to be added to 100 ml of vinegar essence (mass fraction acetic acid 70%, density 1.07 g / ml) to obtain a 6% solution of acetic acid. (Write the number down to tenths.) The thermal effect of the decomposition reaction of 1 mol Na 2 SO 4 10H 2 O is Q \u003d 520 kJ. Calculate the amount of heat that must be spent to obtain 54 g of water during the dehydration of sodium sulfate decahydrate J. (Write down the number to the nearest whole.) Calculate the mass of bromine (in grams) that can be isolated from the reaction mixture formed by the interaction of 8.7 g manganese (IV) oxide with an excess of hydrobromic acid. d. (Write down the number to the nearest whole.) Do not forget to transfer all the answers to answer form 1 in accordance with the instructions for the work. Write the reaction equations with which you can carry out the following transformations: t, cat. Br 2.40 C. KOH, sol. KMnO 4, H 2SO 4 C 4 H 10 X 1 X 2 1,4-dibromobutane X 3 X 4 When writing the reaction equations, use the structural formulas of organic substances. After keeping a copper plate weighing 14.72 g in a silver nitrate solution, the plate mass was 19.28 g. Determine the volume of a 96% sulfuric acid solution (ρ \u003d 1.86 g / ml), which is necessary to dissolve the resulting plate. Write down the answer the reaction equations, which are indicated in the condition of the problem, and provide all the necessary calculations (indicate the units of measurement of the desired physical quantities). The mass fraction of oxygen in the monobasic organic amino acid is 42.67%. Based on the given conditions of the assignment: 1) make the calculations necessary to establish the molecular formula of organic matter (indicate the units of measurement of the sought physical quantities); 2) write down the molecular formula of the original organic matter; 3) write the structural formula of this substance, which uniquely reflects the order of the bonds of atoms in its molecule 4) write the equation for the reaction of this substance with sulfuric acid to form an acid salt using the structural formula of the substance.

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The final test in chemistry for grade 10 of the 2017-2018 academic year Option 1. Part A. When completing the tasks of this part (A1-A15), from the four proposed options, choose one correct one. In the form

decomposition (19.85-x) g CaCOQ releases-

B \u003d \u003d 0.44 (19.85-x).

By the condition of the problem, a + b \u003d 6.6, 0.22x + (19.85-x) 0.44 \u003d 6.6. Whence x \u003d 9.68 g BaCO3.

Which is 100% \u003d 48.77%.

The mass of CaCO3 is 10.17 g, i.e. (19.85-9.68).

Which is 100% \u003d 51.23%.

Answer. The mass fraction of barium carbonate in the mixture is 48.77%, and calcium carbonate is 51.23%.

Example 2. During the interaction of a mixture of iron and zinc weighing 4.66 g with sulfuric acid, hydrogen was released with a volume of 1.792 liters (NU). Determine the mass fraction of iron and zinc in the original mixture.

m (Fe + Zn) \u003d 4.66 g, V (H2) \u003d 1.792 liters. Find:% (Fe),% Zn. Decision.

1. We denote by xr the mass of iron in the mixture, then the mass of zinc is (4.66 - x) g.

2. Let us calculate the volume of hydrogen released by the action of iron with a mass of x g and zinc with a mass (4.66-x) g on sulfuric acid using the reaction equations:

a) Fe + H2SO4 -\u003e FeS04 + H2t.

In the interaction of x g Fe, al H2 is released. When 56 g of Fe interacts, 22.4 liters of H2 are released.

From where \u003d -; l,

(4.66-x) g b l

b) Zn + H2S04 ZnS04 + H2t

In the interaction of (4.66-x) g Zn, b l H2 will be released.

When 6.5 g of Zn interacts, 22.4 liters of H2 will be released.

65 4.66-x (4.66-x) -22.4

Where from \u003d; b \u003d

3. Equating the sum of volumes (a + b) of hydrogen,

released by the action of two metals on

acid, to the volume of hydrogen given in the condition,

we get the equation:

a + b \u003d 1.79 g,

22.4 x (4.66's) -22.4

4- - - = 1,792.

Having solved this equation with one unknown, we find x \u003d 3.36 g, so m (Fe) \u003d 3.36 g, then m (Zn) \u003d 4.66 g - 3.36 g \u003d 1.3 g.

4. Find the mass fraction of the component in the mixture

o (Fe) \u003d 100% \u003d 72%,

co (Zn) 100% \u003d 28%.

Answer. Mass fraction of iron in the initial mixture is 72%, and zinc is 28%.

Example 3. A mixture of sodium and potassium carbonates weighing 7 g was dissolved in an excess of sulfuric acid, thus forming a gas with a volume of 1.344 liters. Calculate the mass fraction of carbonates in the mixture.

m (Na2C03 + K2C03) - 7 g, V (C02) \u003d 1.344 l. To find:

% Na2C03,% K2C03. Decision.

Na2C03 + H2S04 -\u003e Na2S04 + C02t + H20 1mol

k2co3 + H2S04 -\u003e K2S04 + C02t + H20

Let us denote through x the amount of Na2C03 substance, and through y - the amount of K2CO3 substance: x - v Na2C03, y - v K2CO3.

The amount of carbon dioxide will be: 1.344 l

v (C09) \u003d * \u003d 0.06 mol, (from the formula

L 22.4 L / mol

From the equation of reactions, the amount of the substance that has reacted with sodium carbonate is equal to the amount of the substance CO2:

v (Na2C03) \u003d ((CO2), i.e. x \u003d x.

The amount of the substance that has reacted with K2CO3 is equal to the amount of the substance CO2, i.e.: v (K2C03) \u003d v (C03), y \u003d y.

Mr (Na2C03) \u003d 23-2 + 12 + 16-3 \u003d 106, M (Na2C03) \u003d 106 g / mol, Mr (K2C03) \u003d 39-2 + 12 + 16-3 \u003d 138, M (K2C03) \u003d 138 g / mol.

The mass of Na2C03 in the mixture will be m (Na2C03) \u003d - M v \u003d 106 x.

The mass of K2C03 in the mixture will be m (K2C03) \u003d M v \u003d \u003d 138 y.

Let's compose an algebraic equation: 106 x + 138 y \u003d 7, x + y \u003d 0.06,

x \u003d 0.04 mol, y \u003d 0.02 mol; m (Na2CO3) 4.24 g; m (K2C03) \u003d 2.76 g.

© (NaXOJ \u003d - 100% \u003d 60.6%,

Method II.

x is the mass of Na2C03 in the mixture. 7th - the mass of K2CO3 in the mixture.

0.06 mol, because

v (Na2C03) \u003d v (C02);

from the reaction equation:

0.06; x \u003d 4.24 (g) - Na2C03

7-4.24 \u003d 2.76 -K2C03

Answer, the mass fraction of Na2C03 in the mixture is 60.6%, K2CO3 - 39.4%.

Example 4. 81.95 g of a mixture of potassium chloride, nitrate and berthollet's salt was calcined to constant weight. At the same time, gas evolution took place. After the interaction of this gas with hydrogen, 14.4 g of water were obtained. The calcination product was dissolved in water and the solution was treated with silver nitrate. Dropped out 100.45 g of precipitate. Determine the composition of the mixture (in percent).

m (KCl + KNO3 + KClO3) \u003d 81.95 g,

t (H20) \u003d 14.4 g,

t (sediment) \u003d 100.45 g.

When ignited, potassium chloride does not decompose

is, and nitrate and berthollet salt decompose with the release of oxygen:

2KN03 -\u003e 2KN02 + 02Т,

2KSYu3 -\u003e 2KS1 + 302f.

Determine the amount of oxygen released. Oxygen, combining with hydrogen, gives water: x mol 14.4 g 02 + 2H2 -\u003e 2H20 1 mol 36 g Mg (H20) \u003d 1-2 + 16 \u003d 18 M (H20) -18 g / mol

\u003d; y \u003d \u003d 0.4 mol 0Q,

or 8.96 l (V \u003d Vm-v).

Since the interaction of oxygen liberated during the calcination with hydrogen formed 14.4 g of water (0.8 mol), then, consequently, 0.4 mol O2 entered into this reaction.

After calcining the mixture of initial salts and separation

FeCl 3 + 3NaOH \u003d Fe (OH) 3 ↓ + 3NaCl

2FeCl 3 + 3Na 2 S \u003d 2FeS + S + 6NaCl

2FeCl 3 + Fe \u003d 3FeCl 2

2FeCl 3 + 2KI \u003d 2FeCl 2 + I 2 + 2KCl

2FeCl 3 + H 2 S \u003d 2FeCl 2 + S + 2HCl

2FeCl 3 + H 2 \u003d 2FeCl 2 + 2HCl

FeCl 3 + 3CH 3 COOAg \u003d (CH 3 COO) 3 Fe + 3AgCl ↓

4FeCl 3 + 6H 2 O 2Fe + 3H 2 + 2Fe (OH) 3 + 6Cl 2

2Fe (NO 3) 3 + 3Zn \u003d 2Fe + 3Zn (NO 2) 2

2Fe (NO 3) 3 + 4H 2 SO 4 (conc.) \u003d Fe 2 (SO 4) 3 + SO 2 + 4HNO 3 + 2H 2 O

Fe (NO 3) 2 + Na 2 S \u003d FeS ↓ + 2NaNO 3

Fe 2 (SO 4) 3 + 2KI \u003d I 2 + 2FeSO 4 + K 2 SO 4

Fe 2 (SO 4) 3 + 3BaI 2 \u003d 2FeI 2 + 3BaSO 4 ↓ + I 2 ↓

Fe 2 (SO 4) 3 + 3BaCl 2 \u003d 3BaSO 4 ↓ + 2FeCl 3

2K 2 FeO 4 + 16HCl \u003d 4KCl + 2FeCl 3 + 3Cl 2 + 8H 2 O

4Fe (NO 3) 3 2Fe 2 O 3 + 12NO 2 + 3O 2

When the solutions are mixed, hydrolysis occurs both by the cation of the weak base and by the anion weak acid:

2FeCl 3 + 3Na 2 SO 3 + 3H 2 O \u003d 2Fe (OH) 3 ↓ + 3SO 2 + 6NaCl

2Fe (NO 3) 3 + 3Na 2 CO 3 + H 2 O \u003d 2Fe (OH) 3 ↓ + 3CO 2 + 6NaNO 3

Fe 2 (SO 4) 3 + 3Na 2 CO 3 + 3H 2 O \u003d 2Fe (OH) 3 ↓ + 3CO 2 + 3Na 2 SO 4

Fe 2 (SO 4) 3 + Na 2 SO 3 + H 2 O \u003d Na 2 SO 4 + 2FeSO 4 + H 2 SO 4

Iron. Iron compounds.

1. The salt obtained by dissolving iron in concentrated sulfuric acid was treated with an excess of sodium hydroxide solution. The resulting brown precipitate was filtered off and calcined. The resulting substance was fused with iron. Write the equations for the described reactions.

2. The precipitate obtained by the interaction of iron (III) chloride and silver nitrate was filtered off. The filtrate was treated with a potassium hydroxide solution. The resulting brown precipitate was separated and calcined. The resulting substance, when heated, reacts with aluminum with the release of heat and light. Write the equations for the described reactions.

3. Gas released during the interaction of hydrogen chloride with potassium permanganate reacts with iron. The reaction product was dissolved in water, and sodium sulfide was added thereto. The lighter of the formed insoluble substances was separated and reacted with hot concentrated nitric acid. Write the equations for the described reactions.

(4) The offensive liquid formed by the interaction of hydrogen bromide with potassium permanganate was separated and heated with iron shavings. The reaction product was dissolved in water, and a cesium hydroxide solution was added thereto. The formed precipitate was filtered off and heated. Write the equations for the described reactions.

5. The substance obtained at the cathode in the electrolysis of an iron (II) chloride solution was fused with sulfur, and the product of this reaction was fired. The resulting gas was passed through a barium hydroxide solution. Write the equations for the described reactions.

6. The iron (III) chloride solution was electrolyzed with graphite electrodes. The brown precipitate formed as a by-product of electrolysis was filtered off and calcined. The substance formed at the cathode was dissolved in concentrated nitric acid with heating. The product released at the anode was passed through a cold potassium hydroxide solution. Write the equations for the described reactions.

7. The solution of ferric chloride was treated with a solution of sodium hydroxide, the precipitate that formed was separated and heated. The solid reaction product was mixed with soda ash and calcined. Sodium nitrate and sodium hydroxide were added to the remaining substance and heated for a long time at a high temperature. Write the equations for the described reactions.

8. Ferrous oxide was heated with dilute nitric acid. The solution was carefully evaporated, the solid residue was dissolved in water, iron powder was added to the resulting solution and after a while it was filtered. A potassium hydroxide solution was added to the filtrate, the precipitate that formed was separated and left in the air, while the color of the substance changed. Write the equations for the described reactions.

9. The ferric chloride was treated while heating with concentrated nitric acid and the solution was carefully evaporated. The solid product was dissolved in water, potash was added to the resulting solution, and the precipitate formed was separated and calcined. Hydrogen gas was passed over the obtained substance while heating. Write the equations for the described reactions.

10. Soda ash was added to the ferric chloride solution and the precipitate formed was separated and calcined. Carbon monoxide was passed over the obtained substance while heating and the solid product of the last reaction was introduced into interaction with bromine. Write the equations for the described reactions.

11. Iron scale was dissolved in concentrated nitric acid with heating. The solution was carefully evaporated and the reaction product was dissolved in water. Iron powder was added to the resulting solution, after a while the solution was filtered, and the filtrate was treated with a potassium hydroxide solution; as a result, a light-green precipitate was formed, which quickly darkens in air. Write the equations for the described reactions.

12. Iron powder was added to the ferric chloride solution and after a while the solution was filtered. Sodium hydroxide was added to the filtrate, the separated precipitate was separated and treated with hydrogen peroxide. To the resulting substance was added an excess of potassium hydroxide and bromine; as a result of the reaction, the color of bromine disappeared. Write the equations for the described reactions.

13. The insoluble substance formed by adding sodium hydroxide to the ferric chloride solution was separated and dissolved in dilute sulfuric acid. Zinc dust was added to the resulting solution, the separated precipitate was filtered off and dissolved in concentrated hydrochloric acid. Write the equations for the described reactions.

14. Iron powder was dissolved in a large amount of diluted sulfuric acid and air was passed through the resulting solution, and then a gas with an odor rotten eggs... The formed insoluble salt was separated and dissolved in a hot solution of concentrated nitric acid. Write the equations for the described reactions.

15. Unknown substance A dissolves in concentrated hydrochloric acid, the dissolution process is accompanied by the release of gas with the smell of rotten eggs; after neutralization of the solution with alkali, a voluminous white (light green) precipitate is formed. When substance A is fired, two oxides are formed. One of them is a gas that has a characteristic pungent odor and decolorizes bromine water with the formation of two strong acids in solution. Write the equations for the described reactions.

16. A silvery-gray metal, which is attracted by a magnet, was added to hot concentrated sulfuric acid and heated. The solution was cooled and sodium hydroxide was added until the formation of an amorphous brown precipitate ceased. The precipitate was separated, calcined, and dissolved in concentrated hydrochloric acid while heating. Write the equations for the described reactions.

17. The substance obtained by heating the iron scale in a hydrogen atmosphere was introduced into a hot concentrated acid and heated. The resulting solution was evaporated, the residue was dissolved in water and treated with a solution of barium chloride. The solution was filtered and a copper plate was introduced into the filtrate, which dissolved after a while. Write the equations for the described reactions.

18. The iron (III) chloride solution was electrolyzed. The brown precipitate formed during electrolysis was filtered off and dissolved in a sodium hydroxide solution, after which such an amount of sulfuric acid was added, which was necessary to form a clear solution. The product released at the anode was passed through a hot potassium hydroxide solution. Write the equations for the described reactions.

19. Iron was burned in chlorine. The reaction product was dissolved in water and iron filings were added to the solution. After a while, the solution was filtered and sodium sulfide was added to the filtrate. The separated precipitate was separated and treated with 20% sulfuric acid, obtaining an almost colorless solution. Write the equations for the described reactions.

20. A mixture of iron powder and a solid product obtained by the interaction of sulfur dioxide and hydrogen sulfide was heated without access to air. The resulting product was fired in air. The resulting solid reacts with aluminum to generate a lot of heat. Write the equations for the described reactions.

21. Iron (III) oxide was fused with soda. The resulting product was taken into water. The resulting precipitate was dissolved in hydroiodic acid. The released halogen was bound with sodium thiosulfate. Write the equations for the described reactions.

22. Chlorine has reacted with hot potassium hydroxide solution. When the solution was cooled, crystals of Berthollet's salt precipitated. The crystals obtained were introduced into a hydrochloric acid solution. the resulting simple substance reacted with metallic iron. The reaction product was heated with a new weight of iron. Write the equations for the described reactions.

23. Pyrite was subjected to roasting, the resulting gas with a pungent odor was passed through hydrosulfuric acid. The formed yellowish precipitate was filtered off, dried, mixed with concentrated nitric acid and heated. The resulting solution gives a precipitate with barium nitrate. Write the equations for the described reactions.

24. Iron filings were dissolved in dilute sulfuric acid, the resulting solution was treated with an excess of sodium hydroxide solution. The formed precipitate was filtered and left in air until it turned brown. The brown matter was calcined to constant weight. Write the equations for the described reactions.

25. Conducted electrolysis of sodium chloride solution. Iron (III) chloride was added to the resulting solution. The precipitate that formed was filtered off and calcined. The solid residue was dissolved in hydroiodic acid. Write the equations for the described reactions.

26. Potassium chlorate was heated in the presence of a catalyst and a colorless gas evolved. By burning iron in an atmosphere of this gas, iron scale was obtained. It was dissolved in dilute hydrochloric acid. To the resulting solution was added a solution containing sodium dichromate and hydrochloric acid. Write the equations for the described reactions.

27. Iron was burned in chlorine. The resulting salt was added to a sodium carbonate solution, and a brown precipitate formed. This precipitate was filtered off and calcined. The resulting substance was dissolved in hydroiodic acid. Write the equations for the described reactions.

28. Sulfur was fused with iron. The reaction product was treated with hydrochloric acid. The gas released during this was burned in an excess of oxygen. The combustion products were absorbed in an aqueous solution of iron (III) sulfate. Write the equations for the described reactions.

29. As a result of incomplete combustion of coal, a gas was obtained, in a stream of which iron oxide (III) was heated. The resulting material was dissolved in hot concentrated sulfuric acid. The resulting salt solution was treated with an excess of potassium sulfide solution. Write the equations for the described reactions.

30. Iron was burned in a chlorine atmosphere. The resulting material was treated with an excess of sodium hydroxide solution. The resulting brown precipitate, which was filtered off and calcined. The residue after calcination was dissolved in hydroiodic acid. Write the equations for the described reactions.

31. Iron was dissolved in dilute nitric acid. An excess of sodium carbonate solution was added to the resulting solution. The separated precipitate was filtered off and calcined. The resulting substance was ground into a fine powder together with aluminum and the mixture was set on fire. It burned out with the release of a large amount of heat. Write the equations for the described reactions.

32. Iron powder was heated with sulfur powder. The reaction product was dissolved in hydrochloric acid, and an excess of alkali was added to the solution. The resulting precipitate was calcined in a nitrogen atmosphere. Write the equations for the described reactions.

33. Iron was burned in a chlorine atmosphere. The resulting salt was dissolved in water and a solution of potassium iodide was added thereto. The precipitate of a simple substance was separated and divided into two parts. The first was treated with dilute nitric acid, and the second was heated in a hydrogen atmosphere. Write the equations for the described reactions.

34. Iron was dissolved in hydrochloric acid, and sodium hydroxide was added to the resulting solution until the precipitation stopped. Oxygen was first passed into the resulting reaction mixture, and then hydroiodic acid was added until the precipitation stopped. Write the equations for the described reactions.

35. The precipitate obtained by the interaction of solutions of iron sulfate () and barium nitrate was filtered off. The filtrate was treated with excess sodium hydroxide. The formed precipitate was separated and calcined. The resulting material was treated with an excess of hydrochloric acid solution. Write the equations for the described reactions.

Iron. Iron compounds.

1.2Fe + 6H 2 SO 4 (conc.) Fe 2 (SO 4) 3 + 3SO 2 + 6H 2 O

Fe 2 (SO 4) 3 + 6NaOH \u003d 2Fe (OH) 3 + 3Na 2 SO 4

2Fe (OH) 3 Fe 2 O 3 + 3H 2 O

Fe 2 O 3 + Fe 3FeO

2. FeCl 3 + 3AgNO 3 \u003d 3AgCl ↓ + Fe (NO 3) 3

Fe (NO 3) 3 + 3KOH \u003d Fe (OH) 3 ↓ + 3KNO 3

2Fe (OH) 3 Fe 2 O 3 + 3H 2 O

Fe 2 O 3 + 2Al 2Fe + Al 2 O 3

3.2KMnO 4 + 16HCl \u003d 2MnCl 2 + 2KCl + 5Cl 2 + 8H 2 O

2Fe + 3Cl 2 \u003d 2FeCl 3

2FeCl 3 + 3Na 2 S \u003d S ↓ + 2FeS ↓ + 6NaCl

S + 6HNO 3 (conc. Hot.) \u003d H 2 SO 4 + 6NO 2 + 2H 2 O

4.2KMnO 4 + 16HBr \u003d 2MnCl 2 + 2KCl + 5Br 2 + 8H 2 O

FeBr 3 + 3CsOH \u003d Fe (OH) 3 ↓ + 3CsBr

2Fe (OH) 3 Fe 2 O 3 + 3H 2 O

5.2FeCl 2 + 2H 2 O Fe + H 2 + Fe (OH) 2 + 2Cl 2

4FeS + 7О 2 2Fe 2 O 3 + 4SO 2

Ba (OH) 2 + SO 2 \u003d BaSO 3 + H 2 O

6.4FeCl 3 + 6H 2 O 2Fe + 3H 2 + 2Fe (OH) 3 + 6Cl 2

2Fe (OH) 3 Fe 2 O 3 + 3H 2 O

Fe + 6HNO 3 (conc.) Fe (NO 3) 3 + 3NO 2 + 3H 2 O

Сl 2 + 2KOH (cold) \u003d KClO + KCl + H 2 O

7. FeCl 3 + 3KOH \u003d Fe (OH) 3 ↓ + 3KCl

2Fe (OH) 3 Fe 2 O 3 + 3H 2 O

Fe 2 O 3 + Na 2 CO 3 2NaFeO 2 + CO 2

2NaFeO 2 + 3NaNO 3 + 2NaOH 2Na 2 FeO 4 + 3NaNO 2 + H 2 O

8.3FeO + 10HNO 3 (dil.) 3Fe (NO 3) 3 + NO + 5H 2 O

9. FeCl 2 + 4HNO 3 (cc.) \u003d Fe (NO 3) 3 + NO 2 + 2HCl + H 2 O

2Fe (NO 3) 3 + 3K 2 CO 3 + 3H 2 O \u003d 2Fe (OH) 3 ↓ + 3CO 2 + 6KNO 3

2Fe (OH) 3 Fe 2 O 3 + 3H 2 O

Fe 2 O 3 + 3H 2 2Fe + 3H 2 O

10.2FeCl 3 + 3Na 2 CO 3 + 3H 2 O \u003d 2Fe (OH) 3 ↓ + 3CO 2 + 6NaCl

2Fe (OH) 3 Fe 2 O 3 + 3H 2 O

Fe 2 O 3 + 3CO 2Fe + 3CO 2

11. Fe 3 O 4 + 10HNO 3 (conc.) \u003d 3Fe (NO 3) 3 + NO 2 + 5H 2 O

2Fe (NO 3) 3 + Fe \u003d 3Fe (NO 3) 2

Fe (NO 3) 2 + 2KOH \u003d Fe (OH) 2 + 2KNO 3

4Fe (OH) 2 + O 2 + 2H 2 O \u003d 4Fe (OH) 3

12.2FeCl 3 + Fe \u003d 3FeCl 2

2Fe (OH) 2 + H 2 O 2 \u003d 2Fe (OH) 3 ↓

2Fe (OH) 3 + 3Br 2 + 10KOH \u003d 2K 2 FeO 4 + 6KBr + 8H 2 O

13. FeCl 2 + 2NaOH \u003d Fe (OH) 2 ↓ + 2NaCl

Fe (OH) 2 + H 2 SO 4 \u003d FeSO 4 + 2H 2 O

FeSO 4 + Zn \u003d ZnSO 4 + Fe

Fe + 2HCl \u003d FeCl 2 + H 2

14. Fe + H 2 SO 4 (dil.) \u003d FeSO 4 + H 2

4FeSO 4 + O 2 + 2H 2 SO 4 \u003d 2Fe 2 (SO 4) 3 + 2H 2 O

Fe 2 (SO 4) 3 + 2H 2 S \u003d FeSO 4 + 2S + FeS + 2H 2 SO 4

FeS + 12HNO 3 (conc.) \u003d Fe (NO 3) 3 + 9NO 2 + H 2 SO 4 + 5H 2 O

15. FeS + 2HCl \u003d FeCl 2 + H 2 S

FeCl 2 + 2NaOH \u003d Fe (OH) 2 ↓ + 2NaCl

4FeS + 7O 2 \u003d 2Fe 2 O 3 + 4SO 2

SO 2 + Br 2 + 2H 2 O \u003d H 2 SO 4 + 2HBr

16. 2Fe + 6H 2 SO 4 (conc.) Fe 2 (SO 4) 3 + 3SO 2 + 6H 2 O

Fe 2 (SO 4) 3 + 6NaOH \u003d 2Fe (OH) 3 ↓ + 3Na 2 SO 4

2Fe (OH) 3 Fe 2 O 3 + 3H 2 O

Fe 2 O 3 + 6HCl 2FeCl 3 + 3H 2 O

17. Fe 3 O 4 + 4H 2 3Fe + 4H 2 O

2Fe + 6H 2 SO 4 (conc.) Fe 2 (SO 4) 3 + 3SO 2 + 6H 2 O

Fe 2 (SO 4) 3 + BaCl 2 \u003d FeCl 3 + BaSO 4 ↓

2FeCl 3 + Cu \u003d 2FeCl 2 + CuCl 2

18.4FeCl 3 + 6H 2 O 2Fe + 3H 2 + 2Fe (OH) 3 + 6Cl 2

Fe (OH) 3 + 3NaOH \u003d Na 3

2Na 3 + 6H 2 SO 4 \u003d Fe 2 (SO 4) 3 + 3Na 2 SO 4 + 12H 2 O

3Cl 2 + 6KOH (hot) \u003d KClO 3 + 5KCl + 3H 2 O

19.2Fe + 3Cl 2 \u003d 2FeCl 3

2FeCl 3 + Fe \u003d 3FeCl 2

FeCl 2 + Na 2 S \u003d FeS ↓ + 2NaCl

FeS + H 2 SO 4 \u003d FeSO 4 + H 2 S

20.SO 2 + 2H 2 S \u003d 3S ↓ + 2H 2 O

4FeS + 7O 2 2Fe 2 O 3 + 4SO 2

Fe 2 O 3 + 2Al 2Fe + Al 2 O 3

21. Fe 2 O 3 + Na 2 CO 3 2NaFeO 2 + CO 2

NaFeO 2 + 2H 2 O \u003d Fe (OH) 3 + NaOH

2Fe (OH) 3 + 6HI \u003d 2FeI 2 + I 2 + 6H 2 O

I 2 + 2Na 2 S 2 O 3 \u003d 2NaI + Na 2 S 4 O 6

22.3Cl 2 + 6KOH (hot) \u003d 5KCl + KClO 3 + 3H 2 O

KClO 3 + 6 HCl \u003d KCl + 3Cl 2 + 3H 2 O

2Fe + 3Cl 2 \u003d 2FeCl 3

2FeCl 3 + Fe \u003d 3FeCl 2

23.4FeS 2 + 11O 2 \u003d 2Fe 2 O 3 + 8SO 2

SO 2 + 2H 2 S \u003d 3S + 2H 2 O

S + 6HNO 3 \u003d H 2 SO 4 + 6NO 2 + 2H 2 O

H 2 SO 4 + Ba (NO 3) 2 \u003d BaSO 4 ↓ + 2HNO 3

24. Fe + H 2 SO 4 \u003d FeSO 4 + H 2

FeSO 4 + 2NaOH \u003d Fe (OH) 2 ↓ + Na 2 SO 4

4Fe (OH) 2 + 2H 2 O + O 2 \u003d 4Fe (OH) 3 ↓

2Fe (OH) 3 Fe 2 O 3 + 3H 2 O

25.2NaCl + 2H 2 O H 2 + 2NaOH + Cl 2

FeCl 3 + 3NaOH \u003d Fe (OH) 3 + 3NaCl

2Fe (OH) 3 Fe 2 O 3 + 3H 2 O

Fe 2 O 3 + 6HI (conc.) \u003d 2FeI 2 + I 2 + 3H 2 O

26.2KClO 3 2KCl + 3O 2

3Fe + 2O 2 \u003d Fe 3 O 4

Fe 3 O 4 + 8HCl \u003d FeCl 2 + 2FeCl 3 + 4H 2 O

6FeCl 2 + Na 2 Cr 2 O 7 + 14HCl \u003d 6FeCl 3 + 2CrCl 3 + 2NaCl + 7H 2 O

27.2Fe + 3Cl 2 \u003d 2FeCl 3

2FeCl 3 + 3Na 2 CO 3 + 3H 2 O \u003d 2Fe (OH) 3 ↓ + 3CO 2 + 6NaCl

2Fe (OH) 3 Fe 2 O 3 + 3H 2 O

Fe 2 O 3 + 6HI \u003d 2FeI 2 + I 2 + 3H 2 O

FeS + 2HCl \u003d FeCl 2 + H 2 S

2H 2 S + 3O 2 \u003d 2SO 2 + 2H 2 O

Fe 2 (SO 4) 3 + SO 2 + 2H 2 O \u003d 2FeSO 4 + 2H 2 SO 4

29. C + O 2 2CO

Fe 2 O 3 + 3CO 2Fe + 3CO 2

2Fe + 6H 2 SO 4 Fe 2 (SO 4) 3 + 3SO 2 + 6H 2 O

https://pandia.ru/text/80/267/images/image012_34.gif "width \u003d" 39 "height \u003d" 12 "\u003e 14. Cu Cu (NO3) 2 CuO CuSO 4 Cu CuCl2

https://pandia.ru/text/80/267/images/image045_7.gif "width \u003d" 39 "height \u003d" 12 "\u003e 15. K KNO 3 O 2 MgO MgCO 3 Mg (HCO 3) 2

https://pandia.ru/text/80/267/images/image024_20.gif "width \u003d" 39 "height \u003d" 12 "\u003e 16. FeSO 4 Fe 2 (SO 4) 3 Fe 2O 3 Fe FeCl 2 FeCl 3

Add the right side of the equations:

Halogens

Potassium + bromine \u003d

Iron + chlorine \u003d

Chlorine + water \u003d

Chlorine + potassium hydroxide \u003d

Chlorine + sodium hydroxide \u003d

Sodium chloride + water \u003d

Hydrogen sulfide + bromine \u003d

Potassium iodide + chlorine \u003d

Hydrogen bromide + sulfur oxide (4) \u003d

Hydrogen chloride + manganese oxide (4) \u003d

Silver chloride (temp.) \u003d

Hydrogen chloride + Berthollet's salt \u003d

Iron + chlorine \u003d

Phosphorus + chlorine (excess \u003d)

Ferric chloride (2) + sulfuric acid (k) \u003d

Potassium chloride + sulfuric acid (k) \u003d

Oxygen and sulfur.

Carbon + oxygen (lack) \u003d

Lithium + oxygen \u003d

Nitrogen and phosphorus

Lithium + nitrogen \u003d

Magnesium + nitrogen \u003d

Ammonia + oxygen (temperature) \u003d \u003d

Ammonia + oxygen (cat.) \u003d

Potassium nitride + water \u003d

Aluminum Chloride + Sodium Hydroxide \u003d

Nitric oxide (4) + water \u003d

Nitric oxide (4) + water + oxygen \u003d

Nitric oxide (4) + potassium hydroxide \u003d

Aluminum nitrite \u003d

Potassium nitrate (temp.) \u003d

Zinc nitrate (temp.) \u003d

Silver nitrate (temp.) \u003d

Nitric oxide (3) + water \u003d

Nitric oxide (5) + water \u003d

Potassium + nitric acid (och. Dil.) \u003d

Potassium + nitric acid (k) \u003d

Calcium Phosphate + Carbon + Quartz \u003d

Phosphorus oxide (5) + potassium hydroxide \u003d

Phosphorus oxide (5) + water (1 molecule) \u003d

Phosphorus oxide (5) + water (2 molecules) \u003d

Phosphorus oxide (5) + water (3 molecules) \u003d

Phosphorus + nitric acid (k) \u003d

Carbon and silicon

Sulfur + carbon \u003d

Carbon + water (steam) \u003d

Carbon + Quartz \u003d

Carbon + sulfuric acid (k) \u003d

Carbon + nitric acid (k) \u003d

Iron oxide (s) + carbon monoxide \u003d

Sodium carbonate + water \u003d

Magnesium silicide + hydrochloric acid \u003d

Potassium silicide + water \u003d

Silicon oxide + carbon \u003d

Quartz + sodium carbonate \u003d

Sodium silicate + carbonic acid \u003d

Silicon oxide + potassium oxide \u003d

Metals of the main subgroups

Lithium + oxygen \u003d

Sodium + oxygen \u003d

Potassium oxide + water \u003d

Magnesium + water \u003d

Sodium hydride + water \u003d

Potassium hydrogen carbonate \u003d

Calcium + Hydrogen \u003d

Barium + Chlorine \u003d

Potassium peroxide + potassium \u003d

Calcium oxide + carbon \u003d

Aluminum + sulfuric acid (k) \u003d

Aluminum + nitric acid (k) \u003d

Aluminum + sodium hydroxide + water \u003d

Aluminum oxide + potassium hydroxide + water \u003d

Aluminum hydroxide + sodium hydroxide \u003d

Aluminum hydroxide + potassium hydroxide (temperature) \u003d

Aluminum + iron oxide (3) \u003d

Aluminum + sodium hydroxide (temperature) \u003d

Side metals

Iron + chlorine \u003d

Iron sulfide + sulfuric acid \u003d

Iron nitrate (temperature) \u003d

Iron + sulfuric acid \u003d

Iron + copper sulfate \u003d

Iron + sulfuric acid (k) \u003d

Iron + nitric acid \u003d

Iron + nitric acid (k)

Iron oxide (3) + carbon monoxide (2) \u003d

Copper + chlorine \u003d

Copper + sulfuric acid (k) \u003d

Copper + nitric acid \u003d

Copper + nitric acid (k) \u003d

Zinc + hydrochloric acid \u003d

Zinc sulfide + oxygen \u003d

Zinc + sodium hydroxide + water \u003d

Zinc + sodium hydroxide (temperature) \u003d

Zinc hydroxide + potassium hydroxide \u003d

Zinc hydroxide (temp.) \u003d

Computational tasks in inorganic chemistry.

Problem solving will help to complete task 39 on the exam .

Subgroup of halogens.

1. A mixture of H2S and HI with a volume of 1.792 liters. passed through an excess of AgNO3 solution. This formed a precipitate 19.19, Determine the ppm and volume fractions of gases in the original mixture.

2. After the thermal decomposition of 197 g of a mixture of KCL and berthollet salt in the presence of MnO2, 149 g of residue was obtained, the melt of which was subjected to electrolysis. How much silicon can react with the gas evolved during electrolysis? Determine the composition of the initial mixture of salts.

3. In what volume of H2O it is necessary to dissolve the hydrogen chloride formed by weak heating of 234 g of NaCL with conc. solution of H2SO4 to obtain a 20% solution of hydrochloric acid?

4. To 100 g of a solution containing the same amount of chloride and fluoride of the same metal, an excess of AgNO3 solution was poured, the precipitate that separated was filtered off, its weight was 14.35 g. The starting salts color the flame yellow. Determine the qualitative and quantitative composition of the salts in the solution in percent.

5. An unknown yellow-green gas with a pungent odor was passed into the NaOH solution. At the same time, a solution of 2 salts is formed, which is used for bleaching fabrics and paper. 11.7 g of one of the salts obtained upon interaction with AgNO3 solution gives 28.7 g of a white curdled precipitate. Calculate the volume of the 10% AgNO3 solution consumed at this p-tition (p \u003d 1.1). What are the salts formed?

6. There is a mixture of KCl, KNO3 and Berthollet's salt. Determine its quantitative composition if, when heated, 8.49 g of this mixture releases 1.12 liters. gas, and when HCl acts on the same amount of the mixture, 1.344 liters are released. gas.

7. When the mixture of KOH and KHCO3 was treated with an excess of HCl, 22.35 g was formed. KCl and released 4.48 liters. gas. Calculate the% composition of the original mixture.

8. A mixture of two gases, one of which was obtained by treating 50 g of CaCO3 with hydrochloric acid, and the second by the interaction of 43.5 g of MnO2 with concentrated hydrochloric acid, was passed through 3018.2 ml. 10% solution of potassium iodide (p \u003d 1.1), Determine the volumetric composition of the gases taken after the end of the reaction. Disregard the solubility of gases.

9. Under the action of HCl on 22.4 g of the unknown metal, metal chloride (2) is formed and 8.96 liters are released. gas. Identify the unknown metal.

10. To 50 g of an aqueous solution containing KCl and NaCl, an excess of pa-a AgNO3 was added. The separated precipitate was filtered off, washed, dried and weighed. Its mass turned out to be 57.4 g. Calculate the concentration of salts in the original solution containing 26.6 g of KCl and NaCl.

11. The salts formed during the interaction of 18 g of a mixture of Fe and Cu with chlorine were treated with an excess of alkali solution. The precipitate was separated and calcined and received 12 g of black powder. Determine the% composition of the initial mixture.

12. After electrolysis of sodium chloride solution, a solution containing 20 g of sodium hydroxide was obtained. The gas evolved at the anode was passed through a 10% solution of potassium iodide (p \u003d 1.1). Calculate the volume of consumed potassium iodide pa-a.

13. In the interaction of 52.2 g of manganese oxide (4) and 336 ml. A 36.5% hydrochloric acid solution (p \u003d 1.19) released gas, which was collected in a flask. When 48.8 g of powder of substance A is introduced into a flask with the resulting gas, a "fire rain" is observed, the substance burns out with the formation of a metal salt, the oxidation state of which in this salt is 3. Determine substance A.

14. When calcining 8.49 g of a mixture of potassium chlorate, potassium nitrate, potassium chloride, 1.12 liters were released. Strip. When the same mass of the mixture interacted with concentrated hydrochloric acid, 1.344 liters were released. gas. Determine the percentage of the original mixture (n.o.).

15. Through a tube with a powdery mixture of chloride and sodium iodide weighing 3 g, passed 1.3 liters. chlorine at 42 degrees C and a pressure of 101.3 kPa. The substance obtained in the tube was calcined at 3000 C. 2 g of substance was released. Determine the mass fraction of salts in the original mixture.

16. A mixture of chlorate, nitrate and potassium chloride weighing 81.9 was calcined, while a gas was evolved, which, upon interaction with hydrogen, formed 14.4 g of water. The residue after calcination was dissolved in water and mixed with a solution of silver nitrate, whereby 100.45 g of precipitate was separated. Determine the% composition of the initial mixture.

Chalcogen subgroup.

What mass of solution with a mass fraction of H2SO4 70% can be obtained from pyrite weighing 200 kg. containing 10% impurities, and the yield of sulfuric acid is 80%. When the gas obtained by firing 8.8 g of FeS and 12 g of FeS2 interacted with solution of NaOH, an average salt was formed. Calculate the volume of consumed 25% NaOH solution (p \u003d 1.28). During the interaction of an average salt of an unknown metal, coloring the flame yellow with an excess of hydrochloric acid, 4.48 g of sulfur oxide, containing 50% sulfur, were released. Determine the formula and amount of the original salt. The gas obtained by burning H2S in an excess of O2 reacted with 250 ml. 25% NaOH solution (p \u003d 1.28) with the formation of an acidic salt. Calculate the amount of consumed hydrogen sulfide. Upon complete combustion of 6.8 g of the substance, 12.8 g of sulfur oxide (2) and 3.6 g of water were obtained. Define the formula starting material... The resulting sulfur oxide (4) was passed through 50 ml. 25% sodium hydroxide solution (p \u003d 1.28) what is the composition of the formed salt and what is its concentration in the solution? When the gas obtained by the action of an excess of sulfuric acid on sodium sulfite with the gas formed as a result of the reaction of excess hydrochloric acid with iron sulfide (2), 9.6 g of a solid were obtained. Calculate the masses of sodium sulfite and iron sulfide. To 200 g of sulfuric acid solution was added 1040 g of 10% barium chloride solution. The precipitate was filtered off. It took 250 ml to completely neutralize the remaining filtrate. 25% sodium hydroxide solution (p \u003d 1.28). Calculate the concentration (in%) of sulfuric acid in the original solution. When processing 11.14 g of a mixture of potassium and zinc chlorides with sulfuric acid and evaporation to dryness, 13.14 g of a mixture of potassium sulfate and zinc sulfate were formed. Determine the quantitative composition of chlorides and sulfates.

1) Copper nitrate was calcined, the resulting solid precipitate was dissolved in sulfuric acid. Hydrogen sulfide was passed through the solution, the resulting black precipitate was fired, and the solid residue was dissolved by heating in concentrated nitric acid.

2) Calcium phosphate was fused with coal and sand, then the resulting simple substance was burned in an excess of oxygen, the combustion product was dissolved in an excess of caustic soda. A barium chloride solution was added to the resulting solution. The resulting precipitate was treated with an excess of phosphoric acid.

Show
Ca 3 (PO 4) 2 → P → P 2 O 5 → Na 3 PO 4 → Ba 3 (PO 4) 2 → BaHPO 4 or Ba (H 2 PO 4) 2 Ca 3 (PO 4) 2 + 5C + 3SiO 2 → 3CaSiO 3 + 2P + 5CO 4P + 5O 2 → 2P 2 O 5 P 2 O 5 + 6NaOH → 2Na 3 PO 4 + 3H 2 O 2Na 3 PO 4 + 3BaCl 2 → Ba 3 (PO 4) 2 + 6NaCl Ba 3 (PO 4) 2 + 4H 3 PO 4 → 3Ba (H 2 PO 4) 2

3) Copper was dissolved in concentrated nitric acid, the resulting gas was mixed with oxygen and dissolved in water. Zinc oxide was dissolved in the resulting solution, then a large excess of sodium hydroxide solution was added to the solution.

4) Dry sodium chloride was acted upon with concentrated sulfuric acid under weak heating, the resulting gas was passed into a barium hydroxide solution. Potassium sulfate solution was added to the resulting solution. The resulting precipitate was fused with coal. The resulting material was treated with hydrochloric acid.

5) A sample of aluminum sulfide was treated with hydrochloric acid. In this case, gas was released and a colorless solution was formed. An ammonia solution was added to the resulting solution, and the gas was passed through a lead nitrate solution. The resulting precipitate was treated with a hydrogen peroxide solution.

Show
Al (OH) 3 ← AlCl 3 ← Al 2 S 3 → H 2 S → PbS → PbSO 4 Al 2 S 3 + 6HCl → 3H 2 S + 2AlCl 3 AlCl 3 + 3NH 3 + 3H 2 O → Al (OH) 3 + 3NH 4 Cl H 2 S + Pb (NO 3) 2 → PbS + 2HNO 3 PbS + 4H 2 O 2 → PbSO 4 + 4H 2 O

6) Aluminum powder was mixed with sulfur powder, the mixture was heated, the resulting substance was treated with water, while gas was released and a precipitate was formed, to which an excess of potassium hydroxide solution was added until complete dissolution. This solution was evaporated and calcined. An excess of hydrochloric acid solution was added to the resulting solid.

7) The potassium iodide solution was treated with a chlorine solution. The resulting precipitate was treated with sodium sulfite solution. A solution of barium chloride was added to the resulting solution, and after separation of the precipitate, a solution of silver nitrate was added.

8) Gray-green powder of chromium (III) oxide was fused with an excess of alkali, the resulting substance was dissolved in water, and a dark green solution was obtained. Hydrogen peroxide was added to the resulting alkaline solution. The result is a yellow solution, which becomes orange when added with sulfuric acid. When passing hydrogen sulfide through the resulting acidified orange solution, it becomes cloudy and turns green again.

Show
Cr 2 O 3 → KCrO 2 → K → K 2 CrO 4 → K 2 Cr 2 O 7 → Cr 2 (SO 4) 3 Cr 2 O 3 + 2KOH → 2KCrO 2 + H 2 O 2KCrO 2 + 3H 2 O 2 + 2KOH → 2K 2 CrO 4 + 4H 2 O 2K 2 CrO 4 + H 2 SO 4 → K 2 Cr 2 O 7 + K 2 SO 4 + H 2 O K 2 Cr 2 O 7 + 3H 2 S + 4H 2 SO 4 → 3S + Cr 2 (SO 4) 3 + K 2 SO 4 + 7H 2 O

9) Aluminum was dissolved in a concentrated potassium hydroxide solution. Carbon dioxide was passed through the resulting solution until the precipitation ceased. The precipitate was filtered off and calcined. The resulting solid residue was fused with sodium carbonate.

10) Silicon was dissolved in a concentrated solution of potassium hydroxide. An excess of hydrochloric acid was added to the resulting solution. The cloudy solution was heated. The separated precipitate was filtered off and calcined with calcium carbonate. Write the equations for the described reactions.

11) Copper (II) oxide was heated in a stream of carbon monoxide. The resulting substance was burned in a chlorine atmosphere. The reaction product was dissolved in water. The resulting solution was divided into two parts. Potassium iodide solution was added to one part, and silver nitrate solution to the second. In both cases, the formation of a precipitate was observed. Write the equations for the four reactions described.

12) Copper nitrate was calcined, the resulting solid was dissolved in dilute sulfuric acid. The resulting salt solution was subjected to electrolysis. The substance released at the cathode was dissolved in concentrated nitric acid. Dissolution proceeded with the evolution of brown gas. Write the equations for the four reactions described.

13) Iron was burned in a chlorine atmosphere. The resulting material was treated with an excess of sodium hydroxide solution. A brown precipitate formed, which was filtered off and calcined. The residue after calcination was dissolved in hydroiodic acid. Write the equations for the four reactions described.
14) Powder of metallic aluminum was mixed with solid iodine and a few drops of water were added. Sodium hydroxide solution was added to the resulting salt until a precipitate formed. The resulting precipitate was dissolved in hydrochloric acid. On subsequent addition of the sodium carbonate solution, precipitation was again observed. Write the equations for the four reactions described.

15) As a result of incomplete combustion of coal, a gas was obtained, in which iron (III) oxide was heated. The resulting material was dissolved in hot concentrated sulfuric acid. The resulting salt solution was subjected to electrolysis. Write the equations for the four reactions described.

16) Some zinc sulfide was divided into two parts. One of them was treated with nitric acid, and the other was fired in air. The interaction of the evolved gases formed a simple substance. This substance was heated with concentrated nitric acid, and a brown gas was evolved. Write the equations for the four reactions described.

17) Potassium chlorate was heated in the presence of a catalyst, while a colorless gas was evolved. By burning iron in an atmosphere of this gas, iron scale was obtained. It was dissolved in an excess of hydrochloric acid. To the resulting solution was added a solution containing sodium dichromate and hydrochloric acid.

Show

1) 2КClО 3 → 2КСl + 3О 2 2) ЗFe + 2O 2 → Fe 3 O 4 3) Fe 3 O 4 + 8HCI → FeCl 2 + 2FeCl 3 + 4H 2 O 4) 6 FeCl 2 + Na 2 Cr 2 O 7 + 14 НСІ → 6 FeCl 3 + 2 CrCl 3 + 2NaCl + 7Н 2 О 18) Iron was burned in chlorine. The resulting salt was added to a sodium carbonate solution, and a brown precipitate formed. This precipitate was filtered off and calcined. The resulting substance was dissolved in hydroiodic acid. Write the equations for the four reactions described. 1) 2Fe + 3Cl 2 → 2FeCl 3 2) 2FeCl 3 + 3Na 2 CO 3 → 2Fe (OH) 3 + 6NaCl + 3CO 2 3) 2Fe (OH) 3 Fe 2 O 3 + 3H 2 O 4) Fe 2 O 3 + 6HI → 2FeI 2 + I 2 + 3H 2 O

19) A solution of potassium iodide was treated with an excess of chlorine water, while the formation of a precipitate was observed first, and then its complete dissolution. The resulting iodine-containing acid was isolated from the solution, dried and heated gently. The resulting oxide reacted with carbon monoxide. Write down the equations of the described reactions.

20) Powder of chromium (III) sulfide was dissolved in sulfuric acid. In this case, gas was released and a colored solution was formed. An excess of ammonia solution was added to the resulting solution, and the gas was passed through lead nitrate. The resulting black precipitate turned white after treatment with hydrogen peroxide. Write down the equations of the described reactions.

21) Aluminum powder was heated with sulfur powder, the resulting substance was treated with water. The precipitate that formed was treated with an excess of concentrated potassium hydroxide solution until it was completely dissolved. An aluminum chloride solution was added to the resulting solution and the formation of a white precipitate was observed again. Write down the equations of the described reactions.

22) Potassium nitrate was heated with powdered lead until the reaction was terminated. The product mixture was treated with water, and then the resulting solution was filtered. The filtrate was acidified with sulfuric acid and treated with potassium iodide. The separated simple substance was heated with concentrated nitric acid. In the atmosphere of the resulting brown gas, red phosphorus was burned. Write down the equations of the described reactions.

23) Copper was dissolved in dilute nitric acid. An excess of ammonia solution was added to the resulting solution, observing first the formation of a precipitate, and then its complete dissolution with the formation of a dark blue solution. The resulting solution was treated with sulfuric acid until the characteristic blue color of copper salts appeared. Write down the equations of the described reactions.

Show
1) 3Cu + 8HNO 3 → 3Cu (NO 3) 2 + 2NO + 4H 2 O 2) Cu (NO 3) 2 + 2NH 3 H 2 O → Cu (OH) 2 + 2NH 4 NO 3 3) Cu (OH) 2 + 4NH 3 H 2 O → (OH) 2 + 4H 2 O 4) (OH) 2 + 3H 2 SO 4 → CuSO 4 +2 (NH 4) 2 SO 4 + 2H 2 O

24) Magnesium was dissolved in dilute nitric acid, and no gas evolution was observed. The resulting solution was treated with an excess of potassium hydroxide solution with heating. The gas released during this process was burned in oxygen. Write down the equations of the described reactions.
25) A mixture of potassium nitrite and ammonium chloride powders was dissolved in water and the solution was gently heated. The released gas reacted with magnesium. The reaction product was added to an excess of hydrochloric acid solution, and no gas evolution was observed. The obtained magnesium salt in solution was treated with sodium carbonate. Write down the equations of the described reactions.

26) Aluminum oxide was fused with sodium hydroxide. The reaction product was introduced into the ammonium chloride solution. The released gas with a pungent smell is absorbed by sulfuric acid. The resulting middle salt was calcined. Write down the equations of the described reactions.

27) Chlorine has reacted with hot potassium hydroxide solution. When the solution was cooled, crystals of Berthollet's salt precipitated. The crystals obtained were introduced into a hydrochloric acid solution. The resulting simple substance reacted with metallic iron. The reaction product was heated with a new weight of iron. Write down the equations of the described reactions.
28) Copper was dissolved in concentrated nitric acid. An excess of ammonia solution was added to the resulting solution, observing first the formation of a precipitate and then its complete dissolution. The resulting solution was treated with an excess of hydrochloric acid. Write down the equations of the described reactions.

29) Iron was dissolved in hot concentrated sulfuric acid. The resulting salt was treated with an excess of sodium hydroxide solution. The resulting brown precipitate was filtered off and calcined. The resulting substance was fused with iron. Write the equations for the four reactions described.

30) As a result of incomplete combustion of coal, a gas was obtained, in the current of which iron oxide (III) was heated. The resulting material was dissolved in hot concentrated sulfuric acid. The resulting salt solution was treated with an excess of potassium sulfide solution.

31) Some zinc sulfide was divided into two parts. One of them was treated with hydrochloric acid, and the other was fired in air. The interaction of the evolved gases formed a simple substance. This substance was heated with concentrated nitric acid, and a brown gas was released.

32) Sulfur was fused with iron. The reaction product was treated with hydrochloric acid. The gas released during this was burned in an excess of oxygen. The combustion products were absorbed in an aqueous solution of iron sulfate (III).