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Chemical Kinetics Case Study Questions With Answers
Here, we have provided case-based/passage-based questions for Class 12 Chemistry Chapter 4 Chemical Kinetics
Case Study/Passage-Based Questions
Case Study 1:The half-life of a reaction is the time required for the concentration of reactant to decrease by half,
this means t1/2 is independent of initial concentration. The figure shows a typical variation of concentration of reactant exhibiting first-order kinetics. It may be noted that though the major portion of the first-order kinetics may be over in
a finite time, the reaction will never cease as the concentration of reactant will be zero only at infinite time.
A first-order reaction has a rate constant k = 3.01 × 10–3 /s. How long it will take to decompose half of the reactant?
(a) 2.303 s (b) 23.03 s
(c) 230.3 s (d) 2303 s
Answer: (c) 230.3 s
The rate constant for a first-order reaction is 7.0 × 10–4 s–1. If the initial concentration of reactant is 0.080 M, what is the half-life of the reaction?
(a) 990 s (b) 79.2 s
(c) 12375 s (d) 10.10 × 10–4 s
Answer: (a) 990 s
For the half-life period of a first-order reaction, which one of the following statements is generally false?
(a) It is independent of initial concentration.
(b) It is dependent on the rate of the reaction.
(c) At t1/2, the concentration of the reactant is reduced by half.
(d) None of these
Answer: (b) It is dependent on the rate of the reaction.
The rate of a first-order reaction is 0.04 mol L–1 s–1 at 10 minutes and 0.03 mol L–1 s–1 at 20 minutes after initiation. The half-life of the reaction is
(a) 4.408 min (b) 44.086 min
(c) 24.086 min (d) 2.408 min
Answer: (c) 24.086 min
The plot of t1/2 vs initial concentration [A]0 for a first-order reaction is given by
Answer: (b) B option is right
Case Study/Passage-Based Questions
Case Study 2:For the reaction : 2NO(g) + Cl2(g) → 2NOCl(g) the following data were collected. All the measurements were taken at 263 K.
The molecularity of the reaction is
(a) 1 (b) 2 (c) 3 (d) 4
Answer: (c) 3
The expression for rate law is
(a) r = k[NO]Cl2 (b) r = k[NO]2[Cl2]
(c) r = k[NO][Cl2]2 (d) r = k[NO]2[Cl2]2
Answer:(b) r = k[NO]2[Cl2]
The overall order of the reaction is
(a) 2 (b) 0
(c) 1 (d) 3
Answer:(d) 3
The value of rate constant is
(a) 150.32 M–2 min–1 (b) 200.08 M–1 min–1
(c) 177.77 M–2 min–1 (d) 155.75 M–1 min–1
Answer:(c) 177.77 M–2 min–1
The initial rate of disappearance of Cl2 in experiment 4 is
(a) 1.75 M min–1 (b) 3.23 M min–1
(c) 2.25 M min–1 (d) 2.77 M min–1
Answer:(d) 2.77 M min–1
Case Study 3: The following reaction, A(g)⟶ΔP(g)+Q(g)+R(g) follows first-order kinetics. The half-life period of this reaction is 69.3 s at 500°C. The Gas A is enclosed in a container at 500°C and at a pressure of 0.4 atm
(i) The rat constant for the reaction is
| (a) 0.4 s-1 | (b) 0.02 s-1 | (c) 0.01 s-1 | (d) 0.3 s-1 |
Answer:(c) 0.01 s-1
(ii) The total pressure of the system after 230 s will be
| (a) 2.15 atm | (b) 1.12 atm | (c) 0.4 atm | (d) 3.08 atm |
Answer:(b) 1.12 atm
(iii) The plot of ln[A] vs t will be
| (a) linear with slope = k | (b) linear with intercept = In[A]o |
| (c) linear with slope = In[A]o | (d) linear with intercept = [A]0 |
Answer:(b) linear with intercept = In[A]o
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