The reaction, the equation of which is 2SO2 + O2 \u003d 2 SO3 + Q, is classified as a reaction:

a) irreversible, exothermic;

b) reversible, endothermic;

c) irreversible, endothermic;

d) reversible, exothermic

2. The temperature coefficient of the reaction is 2. Determine how many times the reaction rate will increase with an increase in temperature by 30 ° C.

3. Zinc and iron react with sulfuric acid of the same concentration. In which tube will the reaction rate be faster?

4. Some reaction, displayed by the equation A + 2 B \u003d AB2, proceeds in solution. The initial concentration of substance B was 4 mol/L. After 2 minutes, the concentration of substance B was 0.5 mol/L. Calculate the average rate of a chemical reaction.

5. Determine in which direction the equilibrium of the chemical reaction CH4 (g) + H2O (g) → CO2 (g) + H2 (g) - Q will shift when

a) an increase in temperature

b) pressure drop

c) an increase in the concentration of carbon dioxide.

6. The law of mass action: at a constant temperature, the rate of this reaction is proportional to the product ...

7. Systems in which there are no interfaces separating parts of the system from each other are called ...

8. How will the rate of a chemical reaction change, the equation of which

CO + 2H2 → CH3OH, with a 4-fold decrease in pressure in the reacting system?

9. How will the rate of a chemical reaction change, the equation of which

2NH3 + 3CuO = N2 + 3H2O + 3Cu if the ammonia concentration decreases by 3 times.

10. The temperature coefficient is 3. How many times will the rate of a chemical reaction increase with an increase in temperature by 30 ° C.

2. Give examples chemical reactions, in which the qualitative composition of substances remains constant.

metallic properties. For the element with the most pronounced metallic properties, draw a diagram of the structure of the atom. Compose a molecular formula. structural electronic formula of its compound.

2) Carry out the following transformations Fe->Fes->H2S->Na2S. Name all substances. Indicate the type of chemical reaction; for reaction 3, write the full ionic and abbreviated equations.

3) Complete the equations of those reactions that proceed to the end as a result of the formation of gas: a) CaCo3 + HCl ->... b) BaCl2 + AgNO3 ->... c) K2SO3 + HNO3 ->... d) Na2CO3 + KCl->...

4) Write the formulas of acids and their corresponding acid oxides coal, sulfur, selenium.

5) (task) The mass of nitric acid in 350 cm2 of a solution with a mass fraction of acid of 16% and completely 1.09 g / cm3 was poured a solution of lithium hydroxide. Determine the mass and number of molecules of the formed salt. PLEASE HELP I would be very grateful

Test work No. 1

Option 1

Part A Questions .

Part B Questions drawn uplooking for a match , as well as .

each task of part A is estimated at 0.5 points, tasks of part B are graded differently: a completely correct answer - 1 point, out of three answers only 2 are correct - 0.5 points. The task of part C is evaluated differently: from 0.5 to 3 points. After the work is completed, the scores of correctly completed tasks are summed up during the check, thus obtaining the primary score.

8 - 9 5

6 - 7 4

3 - 5 3

0 - 2 2

Part BUT

Hydrochloric acid reacts more rapidly with

1) hg 2) Zn 3) mg 4 )Fe

Reaction does not apply to OVR

1) Al+O 2 → Al 2 O 3

2 ) MnO 2 + H 2 → Mn+H 2 O


3)H 2 O 2 → H 2 + O 2


4) HNO 3 + Fe(OH) 3 → Fe(NO 3 ) 3 + H 2 O

The reducing agent in the reaction scheme

Mn 2 O 7 + NH 3 → MNO 2 + H 2 O + N 2 is

N 2 0 2) N 3- 3) Mn 4+ 4) Mn 7+

When dissolved in water, hydroxide ions form a substance whose formula is

1)Cu(OH) 2 2)Ca(NO 3 ) 2 3) NaOH 4)H 2 SO 4

5. With complete dissociation, 1 mol of copper nitrate (II) in solution is formed

1) 3 mol of copper cations and 1 mol of nitrate ions

2) 2 mol of copper cations and 3 mol of nitrate ions

3) 1 mol of copper cations and 2 mol of nitrate ions

4) 1 mol of copper cations and 3 mol of nitrate ions

6. Choose the correct notation for the right side of the sodium carbonate dissociation equation

1) = Na + + CO 3 2- 2) = Na + + 2CO 3 2-

3) = 2Na + + CO 3 2- 4) = 2Na + + HCO 3 -

Part B

1) S -2 →S 0 BUT . HNO 3 →H 2 O + NO 2 + O 2

2) S +6 →S +4 B . H 2 S+SO 2 → H 2 O+S

3) N +5 → N +4 IN . NH 3 + O 2 → H 2 O + NO

4) N -3 →N 0 G . NH 3 + O 2 → H 2 O+N 2

D . C+H 2 SO 4 → CO 2 + SO 2 +H 2

1) barium hydroxide and hydrochloric acid A.2H + + SO 3 2- → H 2 O + SO 2

2) iron chloride ( III) and silver nitrate B.Fe 3+ +3 Oh - → Fe(Oh) 3

3) iron nitrate ( III) and potassium hydroxide B.Ag + + Cl - → AgCl

4) sodium sulfite and hydrochloric acid D.H + + Oh - → H 2 O

3 SO 2 + O 2 = 2 SO 3 + Q

VI) necessary

raise the temperature

lower the temperature

reduce pressure

4) increase pressure

5) reduce concentrationO 2

6) increase concentrationSO 2

Part C

To 20 g of a solution containing 5% copper sulfate (II), added sodium hydroxide. Calculate the mass of precipitate formed.

Test work No. 1

on the topic “Classification of chemical reactions. Chemical reactions in aqueous solutions»

Option 2

Part A Questions have one correct answer .

Part B Questions drawn uplooking for a match , as well asquestions with multiple answers .

The grading option is: eachthe task of part A is estimated at 0.5 points , taskspart B evaluated differently: completely correct answer - 1 point, out of three answers only 2 are correct - 0.5 points . The taskpart C assessed differentially: 0.5 to 3 points . After completing the work, the scores of correctly completed tasks are summed up during the check, thus obtaining the primary score.

Primary score Score in a five-point system

8 - 9 5

6 - 7 4

3 - 5 3

0 - 2 2

Part A

1. The interaction of water with

1) hg 2) Zn 3) mg 4) N but

2 . Reaction does not apply to OVR

1) KMnO 4 → K 2 MNO 4 +MnO 2 + O 2

2) Cu 2 O+ H 2 → Cu + H 2 O

3) Al(OH)3 + HCl→ AlCl 3 + H 2 O

4) HCl + Fe→ FeCl 2 + H 2

3 .Oxidant in the reaction scheme

CrO 3 + NH 3 → Cr 2 O 3 + H 2 O + N 2 is

Cr +6 2) N 3- 3) Cr +3 4) N 2 0

4. Which substance dissociates to form hydrogen ions?

1) sodium carbonate 2) sodium hydroxide

3) sulphuric acid 4) silicic acid

5. With complete dissociation, 1 mol of aluminum nitrate (III) in solution is formed

1) 3 mol of aluminum cations and 1 mol of nitrate ions

2) 2 mol of aluminum cations and 3 mol of nitrate ions

3) 1 mol of aluminum cations and 2 mol of nitrate ions

4) 1 mol of aluminum cations and 3 mol of nitrate ions

6. Choose the correct notation for the right side of the sodium phosphate dissociation equation

1) = Na + +PO 4 3- 2) = 3 Na + +PO 4 3-

3) = 2Na + +PO 4 3- 4) = Na + + HPO 4 2-

Part B

Establish a correspondence between the redox process, indicated by the electron transfer scheme, and the chemical reaction scheme.

1) S 0 →S 2- BUT . SO 2 + O 2 → SO 3

2) S 4+ →S 6+ B . NH 3 + O 2 →NO + H 2 O

3) N -3 → N +2 IN . S+O 2 →SO 2

4) N +4 →N +5 G . H 2 O + NO 2 + O 2 → HNO 3

D. H 2 + S → H 2 S

2. Set the correspondence between the reagents and the abbreviated ionic reaction equation

Reduced reagents ionic equations reactions

1) copper sulfate ( II) and sodium hydroxide A.CO 3 2- + 2 H + → H 2 O + CO 2

2) Nitric acid and potassium hydroxide B.Cu 2+ + 2 Oh - → Cu(Oh) 2

3) potassium carbonate and hydrochloric acid B.CuO + 2 H + → Cu 2+ + H 2 O

4) copper oxide ( II) and hydrochloric acid D.H + + Oh - → H 2 O

3 . To shift the chemical equilibrium of reaction 2SO 2 + O 2 = 2 SO 3 + Q

towards the formation of sulfur oxide (VI) necessary

1) raise the temperature

2) lower the temperature

3) reduce pressure

4) increase pressure

5) reduce concentrationO 2

6) increase concentrationSO 2

Part C

Determine the amount of heat that will be released during the formation of 120 g of magnesium oxideas a result of the combustion reaction of magnesium, using the thermochemical equation.

2 mg + O 2 = 2 MgO+ 1204 kJ

A small test on the topic " Classification of chemical reactions "for students in grade 11 in 4 versions. . Useful for the current control of knowledge on this topic, as well as for preparing students for the exam, since the tasks are taken from the tests of the exam different years. Having been engaged for many years in preparing students for the One State Exam, came to the conclusion that at first it is necessary to work out thematic tests, and only then give USE test fully. This is one of those tests.

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MOU "Secondary school with. Cherny Yar, Astrakhan region

Babakalenko Vera Alexandrovna

2010

Test on the topic "Classification of chemical reactions" Option 1.

1 . The statement that the production of ammonia from nitrogen is a process is incorrect:

a) expansions; b) catalytic; c) reversible; d) homogeneous.

2. It is true that a neutralization reaction is a reaction:

a) b) exchange;

in) always reversible; G) catalytic.

3. Of the processes listed below, a chemical reaction includes:

a) burning; b) boiling c) sublimation; d) melting

4. The reaction is irreversible:

a) b) production of sulfurous acid from sulfur(IV) oxide and water;

in) decomposition of copper hydroxide (P); G)

but) potassium hydroxide solution and hydrochloric acid; b) magnesium and sulfur;

in) zinc and hydrochloric acid; G) copper (II) chloride solution and iron.

Test on the topic "Classification of chemical reactions" Option 2.

1. The reaction is homogeneous:

but) burning phosphorus b) reaction between phosphorus(V) oxide and water

in) oxidation of nitric oxide (II) with oxygen G)

2. The statement is true that the reaction: Zn + 2 HCl = ZnCl 2 + H 2

but) redox; b) exchange;

c) reversible; G) catalytic.

3 . Of the following processes, a chemical reaction does not apply:

a) combustion of magnesium; b) iron rusting

c) boiling water; G) decomposition of calcium carbonate

4 . The reaction is irreversible:

but) decomposition of carbonic acid; b ) obtaining sulfurous acid from sulfur oxide (IV) and water

in) decomposition of zinc hydroxide; G) obtaining ammonia from simple substances.

5. Ion exchange reactions include the reaction between:

but) sodium and water; b) iron and sulfur;

in) magnesium and hydrochloric acid; G) barium chloride solution and sodium sulfate solution.

Test on the topic "Classification of chemical reactions" Option 3.

1. Compound reactions include:

but) burning phosphorus in) reaction between copper and nitric acid solution b) d) reaction between chalk and hydrochloric acid

2. The statement is true that the reaction: CuO + 2 HCl \u003d CuCl 2 + H 2 O

but) redox; b) exchange;

c) connections; d) homogeneous.

3 . During chemical reactions, the thermal energy of the reaction system:

a) is absorbed b) does not change;

c) stands out; G) may be absorbed or released.

4 . The reaction is homogeneous:

a) Zn + 2HCl \u003d ZnCl 2 + H 2; b) 2 NO + O 2 \u003d 2NO 2

c) S + O 2 \u003d SO 2; d) CaO + H 2 O \u003d Ca (OH) 2.

5. Ion exchange reactions include the reaction between:

but) sodium and chlorine; b) zinc and sulfur;

in) iron and hydrochloric acid; G) barium chloride solution and silver nitrate solution.

Test on the topic "Classification of chemical reactions" Option 4.

1. Substitution reactions include:

but) burning phosphorus b) reaction between lithium hydroxide and hydrochloric acid

in) reaction between potassium and water G) decomposition of aluminum hydroxide when heated

2. The statement is true that the reaction: Ca (OH) 2 + 2 HCl \u003d CaCl 2 + 2 H 2 O

but) redox; b) exchange;

c) connections; G) catalytic.

3 . A reaction that does not change the composition of a substance is:

but) formation of ozone from oxygen; b) combustion of aluminum;

in) decomposition of potassium permanganate; G) complete oxidation glucose.

4 . The reaction is exothermic:

a) MgCO 3 \u003d MgO + CO 2; b) 2 H 2 O 2 \u003d O 2 + 2H 2 O

c) S + O 2 \u003d SO 2; d) 2 H 2 O \u003d O 2 + 2H 2

5. Reactions that take place without changing the oxidation state include the reaction between:

but) sodium and chlorine; b) zinc and sulfur;

in) iron and hydrochloric acid; G) barium chloride solution and silver nitrate solution.

1) The exchange reaction is

a) BaO + HOH →; b) H2SO4 + Zn →; c) HNO3 + Ca(OH)2 →; d) N2 + O2 →

2) The reversible reaction is

a) HCl + KOH → KCl - + H2O; b) N2 + O2 → 2NO;

c) C(s) + O2 → CO2; d) BaCl2 + 2AgNO3 → 2AgCl + Ba(NO3)2

3) Endothermic reactions are:

a) CaCO3 \u003d CaO + CO2 -Q; b) 2H2O2 → 2H3O + O2 + Q

c) N2 + O2 → 2NO -Q; d) 2SO2 + O2 → 2SO3 + Q

4) Catalyst is...

a) a reaction retarder that reacts with the starting materials;

b) a reaction accelerator that reacts with the starting materials;

c) a reaction accelerator that is not consumed and is not included in the products;

5) A homogeneous reaction is:

a) 2H2O2(l) ↔ 2H2O(l) + O2(g); b) CH₄(g) + 2O₂(g) → CO₂(g) + 2H₂O(steam);

c) 2Al(s) + 3Cl2(g) → 2AlCl3(s); d) Ca(tv) + 2HCl(l) → CaCl2(l) + H2(g)

6) Not a redox reaction is

a) 2C + O2 → 2CO; b) N2 + O2 → 2NO

c) BaO + SO2 → BaSO3; d) 2Al + 6HCl → 2AlCl3 + 3H2

7) The decomposition reaction is:

a) 2Mg + O2 → 2MgO; b) (CuOH)2CO3 = 2CuO + CO2 + H2O;

c) 3O2 → 2O3; d) CH₄ + 2O₂ → CO₂ + 2H₂O

8) A reaction that proceeds without changing the composition of substances is

a) N2 + O2 → 2NO; b) P4 ↔ 4P; c) 2C + O2 → 2CO; d) N2 + 3H2 → 2NH3

a) FeCl3 + NaOH →

c) Mg + HNO3 →

10) The displacement of less active metals from their oxides by more active metals is ...

a) oxidation; b) burning; c) metallothermy; d) metal-plastic.

11) Berthollet's rule says:

a) Every pure substance, regardless of the method of its preparation, always has a constant qualitative and quantitative composition.

b) The mass of the substances that entered into the reaction is equal to the mass of the substances formed as a result of it.

c) The volumes of reacting gases are related to each other and to the volumes of gaseous reaction products formed as small integers equal to stoichiometric coefficients.

d) Reactions between electrolyte solutions proceed to completion if a precipitate, a gas, or a low-dissociating substance is formed.

12) Describe the chemical reaction in all respects:

2H2O2(l) ↔ 2Н3O(l) + O2(g) + Q

Test on the topic "Classification of chemical reactions"

1) Exothermic reactions are:

a) Mg + 1/2O2 → MgO +614 kJ; b) H2 + O2 → 2H2O -484 kJ;

c) d) CH₄ + 2O₂ → CO₂ + 2H₂O +891 kJ; d) 2C + 2H2 → C2H4 -55 kJ

2) An inhibitor is...

a) a reagent that slows down or stops a chemical reaction;

b) a reagent that speeds up a chemical reaction;

c) a reagent that monitors the presence of by-products in the reaction system;

d) a means of monitoring the progress of a chemical reaction.

3) The substitution reaction is

a) Na2O + HOH →; b) H2SO4 + Al →; c) AgNO3 + CaCl2 →; d) N2 + H2 →

4) An irreversible reaction is:

a) K2CO3 + HCl → KCl -+ CO2 + H2O; b) N2 + O2 → 2NO;

c) SO2 + 1/2O2 → SO3; d) N2 + 3H2 → 2NH3

5) The redox reaction is:

a) CO2 + Na2O → Na2CO3; b) 2Al + 6HCl → 2AlCl3 + 3H2

c) BaCl2 + K2SO4 → BaSO4 + 2KCl; d) 2HNO3 + CaO → Ca(NO3)2 + H2O

6) A heterogeneous reaction is:

a) 2H2(g) + O2(g) ↔ 2H2O (steam); b) CH₄(g) + 2O₂(g) → CO₂(g) + 2H₂O(steam);

c) Al(s) + 3HCl(l) → AlCl3(l) + 1/2Н2(g) d) 2Al(s) + 3I2(s) → 2AlI3(s)

7) A reaction that proceeds without changing the composition of substances is:

c) 3C2H2 → C6H6; d) S + O2 → SO2

8) The reaction of the connection is:

a) 2CrO + 1/2O2 → Cr2O3; b) (CuOH)2CO3 → 2CuO + CO2 + H2O;

c) P4 → 4P; d) C2H₄ + 3O₂ → 2CO₂ + 2H₂O

9) Add the reaction equations and determine their type (s.r., r.s., r.z., r.o.):

a) Na + HOH →

d) H3PO4 + NaOH→

10) The interaction of strong acids and bases to form salt and water is ...

a) leaching; b) neutralization; c) oxidation; d) acid-base titration.

11) The law of constancy of the composition reads:

a) The volumes of reacting gases are related to each other and to the volumes of gaseous reaction products formed as small integers equal to stoichiometric coefficients.

b) Reactions between electrolyte solutions proceed to completion if a precipitate, a gas, or a low-dissociating substance is formed.

c) Every pure substance, regardless of the method of its preparation, always has a constant qualitative and quantitative composition.

d) The mass of the substances that entered into the reaction is equal to the mass of the substances formed as a result of it.

12) Describe the chemical reaction in all respects:

2SO2(g) + O2(g) ↔ 2SO3(g) + Q