The reaction whose equation is 2SO2 + O2 = 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 when the temperature increases by 30°C.

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

4. A certain reaction, represented by the equation A + 2 B = AB2, occurs 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 at

a) increase in temperature

b) decrease in pressure

c) increasing the concentration of carbon dioxide.

6. Law of mass action: at constant temperature, the rate of a given 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 is

CO +2H2 → CH3OH, when the pressure in the reacting system decreases by 4 times?

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

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 when the temperature increases by 30°C?

1.Draw up classification schemes for chemical reactions: a) according to the number and composition of starting substances and reaction products; b) by thermal

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

Help please, I need to solve a chemistry test 1) Chemical elements - magnesium, aluminum, sodium - arrange in order of strength

metal properties. For the element with the most pronounced metallic properties, draw a diagram of the atomic structure. Molecular composition. structural electronic formula of its compound.

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

3) Complete the equations of those reactions that proceed to completion 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: carbonic, sulfurous, selenic.

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

Municipal educational institution "Secondary school with. Cherny Yar" Astrakhan region

Teacher I categories

Babakalenko Vera Alexandrovna

2010

Test on the topic “Classification of chemical reactions” Option 1.

1 . It is incorrect to say that producing ammonia from nitrogen is a process:

A) decomposition; b) catalytic; V) reversible; G) homogeneous.

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

A) b) exchange;

V) always reversible; G) catalytic.

3. Of the following processes, a chemical reaction includes:

A) combustion; b) boiling V) sublimation; G) melting

4. The reaction is irreversible:

A) b) obtaining sulfurous acid from sulfur oxide ( IV) and water;

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

A) a solution of potassium hydroxide and hydrochloric acid; b) magnesium and sulfur;

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

Test on the topic “Classification of chemical reactions” Option 2.

1. The reaction is homogeneous:

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

V) oxidation of nitric oxide ( II) oxygen G) reaction between chalk and hydrochloric acid

2. Zn+ 2 HCl = ZnCl 2 + H 2

A) redox; b) exchange;

V) reversible; G) catalytic.

3 . Of the following processes is not considered a chemical reaction:

A) magnesium combustion; b) iron rusting

V) boiling water; G) decomposition of calcium carbonate

4 . The reaction is irreversible:

A) decomposition of carbonic acid; b) producing sulfurous acid from sulfur oxide ( IV) and water

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

5. Ion exchange reactions include the reaction between:

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

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

Test on the topic “Classification of chemical reactions” Option 3.

1. The reactions of the compound include:

A) phosphorus burning V) reaction between copper and nitric acid solution b) reaction between potassium and water G) reaction between chalk and hydrochloric acid

2. It is true that the reaction is: CuO+ 2 HCl = CuCl 2 + H 2 O

A) redox; b) exchange;

V) connections; G) homogeneous.

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

A) absorbed; b) does not change;

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

4 . The reaction is homogeneous:

A ) Zn + 2HCl = ZnCl 2 + H 2; b) 2 NO + O 2 = 2NO 2

V ) S+O 2 =SO 2; G) CaO+H 2 O = Ca(OH) 2.

5. Ion exchange reactions include the reaction between:

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

V) 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:

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

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

2. It is true that the reaction is: C a(OH) 2 + 2 HCl = CaCl 2 + 2 H 2 O

A) redox; b) exchange;

V) connections; G) catalytic.

3 . A reaction that occurs without changing the composition of a substance is:

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

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

4 . The reaction is exothermic:

A ) MgCO 3 = MgO + CO 2; b) 2 H 2 O 2 = O 2 + 2H 2 O

V ) S+O 2 =SO 2; G) 2 H 2 O = O 2 + 2H 2

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

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

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

Test on the topic “Classification of chemical reactions”

Indicate the reaction schemes for the compound:

1) Fe(OH) 3 → Fe 2 O 3 + H 2 O;

2) AgNO 3 → Ag + NO 2 + O 2;

3) SO 2 + O 2 → SO 3;

4) NO 2 + O 2 + H 2 O → HNO 3.

Indicate the reaction schemes for which a catalyst is necessarily used:

1) KOH + H 2 SO 4 → K 2 SO 4 + H 2 O;

2) N 2 + H 2 → NH 3;

3) NH 3 + O 2 → NO + H 2 O;

4) NH 3 + O 2 → N 2 + H 2 O.

Label the equations or diagrams of decomposition reactions:

1) HNO 3 → H 2 O + NO 2 +O 2;

2) Fe + Cu(NO 3) 2 = Fe(NO 3) 2 + Cu;

3) NaOH + HCl = NaCl + H 2 O;

4) H 2 O 2 → H 2 O + O 2 .

Provide equations or schemes for substitution reactions:

1) Zn + 2AgNO 3 = Zn(NO 3) 2 + 2Ag;

2) Fe + H 2 SO 4 = FeSO 4 + H 2;

3) CaCl 2 + Na 2 CO 3 = CaCO 3 + 2NaCl;

4) CuO + H 2 → Cu + H 2 O.

Label the equations or diagrams of exothermic reactions:

1) N 2 + H 2 → NH 3 + Q;

2) SO 2 + O 2 + Q→ SO 3;

3) C + O 2 = CO 2 + 369 kJ;

4) CaCO 3 = CaO + CO 2 + 157 kJ.

Provide equations or schemes for exchange reactions:

1) NaOH + H 2 SO 4 → Na 2 SO 4 + H 2 O;

2) Ba(NO 3) 2 + K 2 SO 4 → BaSO 4 + KNO 3;

3) N 2 O 5 + H 2 O → HNO 3;

4) CuO + 2HNO 3 = Cu(NO 3) 2 + H 2 O.

The number of products is always less than the number of starting substances in the case of reactions:

1) exchange;

2) connections;

3) decomposition;

4) substitutions.

Label the equations or diagrams of redox reactions:

1) Al + Cl 2 → AlCl 3;

2) BaCO 3 = BaO + CO 2;

3) H 2 O 2 → H 2 O + O 2;

4) Cu + AgNO 3 → Cu(NO 3) 2 + Ag.

Provide equations or schemes for irreversible reactions:

1) N 2 + 3H 2 ⇆ 2NH 3;

2) Ba(OH) 2 + H 2 SO 4 → BaSO 4 + H 2 O;

3) NaOH + HCl = NaCl + H 2 O;

4) SO 2 + O 2 ⇆ SO 3.

The number of products is always greater than the number of starting substances in the case of reactions:

1) decomposition;

2) exchange;

3) connections;

4) substitutions.

The redox reaction in inorganic chemistry is always:

1) decomposition;

2) exchange;

3) substitution;

4) connections.

In inorganic chemistry, a substitution reaction occurs:

1) between two simple substances;

2) two complex substances;

3) simple and complex substances;

4) both two simple and two complex substances.

Redox reactions can be:

1) substitution;

2) exchange;

3) decomposition;

4) connections.

Without changing the oxidation state of atoms of elements, the following reactions always occur:

1) exchange;

2) connections;

3) decomposition;

4) substitutions.

The following substances can enter into an exchange reaction with each other:

1) simple and complex;

2) two simple ones;

3) two complex;

4) both two simple and two complex.

As a result of the decomposition reaction, the following can be formed:

1) only simple substances;

2) only complex substances;

3) either only simple or only complex substances;

4) both simple and complex substances.

Substances that can react with each other include:

1) only simple ones;

2) only complex ones;

3) both simple and complex;

4) simple with complex.

Please indicate true statements:

1) as a result of the decomposition reaction, no more than two new substances are formed;

2) in an exchange reaction, the number of products with different compositions is always equal to the number of starting substances with different compositions;

3) in a compound reaction, the number of starting substances of different compositions is always greater than the products;

4) in inorganic substitution reactions, the number of starting substances with different compositions is equal to the number of products with different compositions.

Indicate the diagram or equation of the redox decomposition reaction:

1) CaCO 3 = CaO + CO 2;

2) H 2 O 2 → H 2 O + O 2;

3) Cu + O 2 → CuO;

4) NaHCO 3 → Na 2 CO 3 + H 2 O + CO 2.

Label the equations or diagrams of the redox reactions of the compound:

1) SO 2 + O 2 → SO 3;

2) NO 2 + H 2 O → HNO 3 + NO;

3) NO 2 + O 2 + H 2 O → HNO 3;

4) SO 2 + NaOH = NaHSO 3.

Indicate the schemes or equations of redox substitution reactions:

1) CaCO 3 + SiO 2 = CaSiO 3 + CO 2;

2) Fe(OH) 2 + HCl → FeCl 2 + H 2 O;

3) Zn + H 2 SO 4 = ZnSO 4 + H 2;

4) Fe 2 O 3 + H 2 → Fe + H 2 O.

ReactionNOTcan be simultaneously:

1) metabolism and redox;

2) redox and decomposition;

3) substitution and redox;

4) compounds and redox.

Homogeneous can be:

1) only exchange reactions;

2) compound reactions only;

3) only decomposition reactions;

4) all of the above reactions, as well as substitution reactions.

The same reaction can occur simultaneously:

a) reversible and exothermic;

b) substitution and exchange;

c) exchange and decomposition;

d) compounds and decompositions.

Label the equations or diagrams of homogeneous compound reactions:

1) CaO (tv) + CO 2 (g) = CaCO 3 (tv);

2) CO (g) + O 2 (g) → CO 2 (g);

3) NO 2 (g) + H 2 O (l) + O 2 (g) → HNO 3 (l);

4) SO 3 (l) + H 2 O (l) = H 2 SO 4 (l).

Provide equations or schemes for homogeneous redox decomposition reactions:

1) Cu(NO 3) 2 (solid) → CuO (solid) + NO 2 (g) + O 2 (g);

2) SO 3 (g) → SO 2 (g) + O 2 (g);

3) NH 4 NO 3 (solid) → N 2 O (g) + H 2 O (l);

4) 2NH 3 (g) = N 2 (g) + 3H 2 (g).

Label the equations or diagrams of heterogeneous redox reactions:

1) Na (solid) + H 2 O (l) → NaOH (p-p) + H 2 (g);

2) H 2 (g) + CuO (s) = Cu (s) + H 2 O (g);

3) NO 2 (g) + CO (g) → N 2 (g) + CO 2 (g);

4) H 2 (g) + N 2 O (g) = N 2 (g) + H 2 O (g).

Indicate schemes or equations of homogeneous exothermic exchange reactions:

1) NaOH (p-p) + HCl (p-p) = NaOH (p-p) + H 2 O (l) + Q;

2) Ba(OH) 2 (p-p) + 2HCl (p-p) = BaCl 2 (p-p) + 2H 2 O (l) + Q;

3) N 2 (g) + H 2 (g) → NH 3 (g) + Q;

4) H 2 (g) + I 2 (g) → HI (g) − Q.

Schemes (equations) of reactions for the production of SO are given 2 . Of these, heterogeneous redox reactions will be:

a) FeS 2 (tv) + O 2 (g) → Fe 2 O 3 (tv) + SO 2 (g);

b) NaHSO 3 (p-p) + HCl (p-p) → NaCl (p-p) + H 2 O (l) + SO 2 (g);

c) S (s) + O 2 (g) = SO 2 (g);

d) Fe 2 (SO 4) 3 (tv) → Fe 2 O 3 (tv) + SO 2 (g) + O 2 (g).

The following reactions are given: a) firing of pyrite; b) limestone burning; c) photosynthesis; d) interaction of aqueous solutions of sodium sulfate and barium chloride. Of the following reactions, the redox reactions will be:

The following signs are suitable to describe the neutralization reaction:

1) always homogeneous;

2) exchange;

3) products - usually salt and water;

4) can be homogeneous and heterogeneous.

Given are substances whose formulas are Zn, ZnO, Zn(OH) 2 , ZnCO 3 ,SO 2 . Indicate the number of substances that can react with H 2 SO 4 (divided) by type of exchange reaction:

Given are substances whose formulas are Al 2 O 3 , Al, Al(OH) 3 ,Na 3 , Al(NO 3 ) 3 ,SO 2 , P 2 O 5 . The number of substances with which KOH (solution) can react according to the type of reaction of the compound is equal to:

Give the formula of the substance with which CuSO 4 (solution) reacts according to the type of exchange reaction:

Substances with formulas Fe are given 2 O 3 , NaHS, Fe(OH) 3 , Ba(NO 3 ) 2 , NaHSO 4 ,Na 2 . Number of substances with which H 2 SO 4 (divided) reacts according to the type of exchange reaction, equal to:

The reactions of the compound include the following reactions:

1) between K 2 S (solution) and H 2 S;

2) Al(OH) 3 and NaOH (p-p);

3) K 3 and HCl (p-p);

4) Al 2 O 3 and KOH (solid).

Specify exothermic processes:

1) F 0 (g) + e - → F − (g);

2) H 2 (g) → 2H (g);

3) Mg (g) → Mg 2+ (g) + 2 e - ;

4) Ca 2+ (g) + 2 e - = Ca (g).