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Class 12 NCERT Solutions Chemistry
Class 12 NCERT Solutions Chemistry
Chapter - 3. Chemical kinetics
Chapter - 3. Chemical kinetics
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From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.
From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.
(i) 3NO(g) → N₂O (g) Rate = k [NO]²
(i) 3NO(g) → N₂O (g) Rate = k [NO]²
(ii) H₂O₂ (aq) + 3I⁻ (aq)+ 2H⁺ → 2H₂O (l) +I⁻₃ Rate = k [H₂O₂][I⁻]
(ii) H₂O₂ (aq) + 3I⁻ (aq)+ 2H⁺ → 2H₂O (l) +I⁻₃ Rate = k [H₂O₂][I⁻]
(iii) CH3CHO (g) → CH₄ (g) + CO(g) Rate = k [CH3CHO]³/²
(iii) CH3CHO (g) → CH₄ (g) + CO(g) Rate = k [CH3CHO]³/²
(iv) C₂H₅Cl (g) → C₂H₄ (g) + HCl (g) Rate = k [C₂H₅Cl]
(iv) C₂H₅Cl (g) → C₂H₄ (g) + HCl (g) Rate = k [C₂H₅Cl]
2. For the reaction:
2. For the reaction:
2A + B → A₂B
2A + B → A₂B
the rate = k[A][B]² with k = 2.0 × 10⁻⁶ mol⁻² L² s⁻¹ . Calculate the initial rate of the reaction when [A] = 0.1 mol L⁻¹ , [B] = 0.2 mol L⁻¹ . Calculate the rate of reaction after [A] is reduced to 0.06 mol L⁻¹ .
the rate = k[A][B]² with k = 2.0 × 10⁻⁶ mol⁻² L² s⁻¹ . Calculate the initial rate of the reaction when [A] = 0.1 mol L⁻¹ , [B] = 0.2 mol L⁻¹ . Calculate the rate of reaction after [A] is reduced to 0.06 mol L⁻¹ .
3. The decomposition of NH3 on platinum surface is zero order reaction. What are the rates of production of N₂ and H₂ if k = 2.5 × 10⁻⁴ mol⁻¹ L s ⁻¹?
3. The decomposition of NH3 on platinum surface is zero order reaction. What are the rates of production of N₂ and H₂ if k = 2.5 × 10⁻⁴ mol⁻¹ L s ⁻¹?
4. The decomposition of dimethyl ether leads to the formation of CH₄ , H₂ and CO and the reaction rate is given by
4. The decomposition of dimethyl ether leads to the formation of CH₄ , H₂ and CO and the reaction rate is given by
Rate = k [CH₃OCH₃ ] ³/²
Rate = k [CH₃OCH₃ ] ³/²
The rate of reaction is followed by increase in pressure in a closed vessel, so the rate can also be expressed in terms of the partial pressure of dimethyl ether, i.e.,
The rate of reaction is followed by increase in pressure in a closed vessel, so the rate can also be expressed in terms of the partial pressure of dimethyl ether, i.e.,
k [CH3OCH3]³/²
k [CH3OCH3]³/²
If the pressure is measured in bar and time in minutes, then what are the units of rate and rate constants?
If the pressure is measured in bar and time in minutes, then what are the units of rate and rate constants?
5. Mention the factors that affect the rate of a chemical reaction.
5. Mention the factors that affect the rate of a chemical reaction.
6. A reaction is second order with respect to a reactant. How is the rate of reaction affected if the concentration of the reactant is
6. A reaction is second order with respect to a reactant. How is the rate of reaction affected if the concentration of the reactant is
(i) doubled (ii) reduced to half ?
(i) doubled (ii) reduced to half ?
7. What is the effect of temperature on the rate constant of a reaction? How can this effect of temperature on rate constant be represented quantitatively?
7. What is the effect of temperature on the rate constant of a reaction? How can this effect of temperature on rate constant be represented quantitatively?
8. In a pseudo first order reaction in water, the following results were obtained:
8. In a pseudo first order reaction in water, the following results were obtained:
t/s 0 30 60 90
t/s 0 30 60 90
[A]/mol L⁻¹ 0.55 0.31 0.17 0.085
[A]/mol L⁻¹ 0.55 0.31 0.17 0.085
9. A reaction is first order in A and second order in B.
9. A reaction is first order in A and second order in B.
(i) Write the differential rate equation.
(i) Write the differential rate equation.
(ii) How is the rate affected on increasing the concentration of B three times?
(ii) How is the rate affected on increasing the concentration of B three times?
(iii) How is the rate affected when the concentrations of both A and B are doubled?
(iii) How is the rate affected when the concentrations of both A and B are doubled?
10. In a reaction between A and B, the initial rate of reaction (r₀ ) was measured for different initial concentrations of A and B as given below:
10. In a reaction between A and B, the initial rate of reaction (r₀ ) was measured for different initial concentrations of A and B as given below:
A/mol L⁻¹ 0.20 0.20 0.40
A/mol L⁻¹ 0.20 0.20 0.40
b/mol L⁻¹ 0.30 0.10 0.05
b/mol L⁻¹ 0.30 0.10 0.05
r₀/mol L⁻¹s⁻¹ 5.07 x 10⁻⁵ 5.07 x 10⁻⁵ 1.43 x 10⁻⁴
r₀/mol L⁻¹s⁻¹ 5.07 x 10⁻⁵ 5.07 x 10⁻⁵ 1.43 x 10⁻⁴
11. The following results have been obtained during the kinetic studies of the reaction:
11. The following results have been obtained during the kinetic studies of the reaction:
2A + B → C + D
2A + B → C + D
Experimen A/mol L⁻¹ B/mol L⁻¹ Initial rate of formation of D/mol L⁻¹ min⁻¹
Experimen A/mol L⁻¹ B/mol L⁻¹ Initial rate of formation of D/mol L⁻¹ min⁻¹
I. 0.1 0.1 6.0 x 10⁻³
I. 0.1 0.1 6.0 x 10⁻³
II. 0.3 0.2 7.2 x 10⁻²
II. 0.3 0.2 7.2 x 10⁻²
III. 0.3 0.4 2.88 x 10⁻¹
III. 0.3 0.4 2.88 x 10⁻¹
IV. 0.4 0.1 2.40 x 10⁻²
IV. 0.4 0.1 2.40 x 10⁻²
Determine the rate law and the rate constant for the reaction.
Determine the rate law and the rate constant for the reaction.
12. Th e reaction between A and B is first order with respect to A and zero order with respect to B. Fill in the blanks in the following table:
12. Th e reaction between A and B is first order with respect to A and zero order with respect to B. Fill in the blanks in the following table:
Experimen [A]/ mol L⁻¹ [B]/ mol L⁻¹ Initial rate/mol L⁻¹ min⁻¹
Experimen [A]/ mol L⁻¹ [B]/ mol L⁻¹ Initial rate/mol L⁻¹ min⁻¹
i. 0.1 0.1 2.0 x 10⁻²
i. 0.1 0.1 2.0 x 10⁻²
i - 0.2 4.0 x 10⁻²
i - 0.2 4.0 x 10⁻²
iii. 0.4 0.4 -
iii. 0.4 0.4 -
iv. - 0.2 2.0 x 10⁻²
iv. - 0.2 2.0 x 10⁻²
13. 13. Calculate the half-life of a first order reaction from their rate constants given below:
13. 13. Calculate the half-life of a first order reaction from their rate constants given below:
(i) 200 s⁻¹ (ii) 2 min⁻¹ (iii) 4 year⁻¹
(i) 200 s⁻¹ (ii) 2 min⁻¹ (iii) 4 year⁻¹
14. The half-life for radioactive decay of ¹⁴C is 5730 years. An archaeological artifact containing wood had only 80% of the ¹⁴C found in a living tree. Estimate the age of the sample.
14. The half-life for radioactive decay of ¹⁴C is 5730 years. An archaeological artifact containing wood had only 80% of the ¹⁴C found in a living tree. Estimate the age of the sample.
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