Topic: Chemical Kinetics, Test No.: 02, Total MCQs: 15
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Question 1 |
Consider the reaction,
Cl2 (aq) + H2S (aq) → S(s) + 2H+(aq) + 2Cl–(aq)
The rate equation for this reaction is, rate = k [Cl2] [H2S]
Which of these mechanisms is/are consistent with this rate equation? [AIEEE 2010]
(a). Cl2 + H2S → H+ + Cl– + Cl+ + HS– (slow)
Cl+ + HS– → H+ + Cl– + S (fast)
(b). H2S 
H+ + HS–
(fast equilibrium)
Cl2 + HS– → 2Cl– + H+ + S (slow)
(a) only | |
(b) only | |
Both (a) and (b) | |
Neither (a) nor (b) |
Question 2 |
The time for half life period of a certain reaction A → Products is 1 h. When the initial concentration of the reactant 'A' is 2.0 mol L–1, how much time does it take for its concentration to come from 0.50 to 0.25 mol L–1, if it is a zero order reaction? [AIEEE 2010]
0.25 h | |
1 h | |
4 h | |
0.5 h |
Question 3 |
The time taken for 10% completion of a first order reaction is 20 min. Then, for 19% completion, the reaction will take [WB JEE 2009]
40 mins | |
60 mins | |
30 mins | |
50 mins |
Question 4 |
For a chemical reaction A → B, the rate of the reaction is 2 × 10–3 mol dm–3 s–1 when the initial concentration is 0.05 mol dm–3. The rate of the same reaction is 1.6 × 10–2 mol dm–3 s–1 when the initial concentration is 0.1 mol dm–3. The order of the reaction is [Karnataka CET 2009]
0 | |
3 | |
1 | |
2 |
Question 5 |
For the decomposition of a compound AB at 600 K, the following data were obtained [Karnataka CET 2009]
|
[AB] mol dm–3 |
Rate of decomposition of AB in mol dm–3 s–1 |
|
0.20 |
2.75 × 10–8 |
|
0.40 |
11.0 × 10–8 |
|
0.60 |
24.75 × 10–8 |
The order for the decomposition of AB is
0 | |
1 | |
2 | |
1.5 |
Question 6 |
The rate equation for a reaction: A → B is r = K [A]°. If the initial concentration of the reactant is a mol dm–3, the half life period of the reaction is [Karnataka CET 2009]
K/a | |
a/K | |
2a/K | |
a/2K |
Question 7 |
For a first order reaction A → P, the temperature (T) dependent rate constant (k) was found to follow the equation
log k =
–(2000) 
+ 6.0.
The pre–exponential factor A and the activation energy Ea, respectively, are [IIT JEE 2009]
1.0 × 106 s−1 and 9.2 kJmol−1 | |
6.0 s−1 and 16.6 kJmol−1 | |
1.0 × 106 s−1 and 16.6 kJmol−1 | |
1.0 × 106 s−1 and 38.3 kJmol−1 |
Question 8 |
For the reaction A + B → products, it is observed that
(i) On doubling the concentration of A only, the rate of reaction is also doubled.
(ii) On doubling the initial concentration of both A and B, there is change by a factor of 8 in the rate of reaction.
The rate of reaction is given by [CBSE AIPMT 2009]
rate = k [A] [B] | |
rate = k [A]2 [B] | |
rate = k [A] [B]2 | |
rate = k [A]2 [B]2 |
Question 9 |
For the
reaction, N2 + 3H2 →
2NH3, if 
= 2 × 10–4
mol L–1 s–1, the value of –
would be [CBSE
AIPMT 2009]
4 × 10–4 mol L–1 s–1 | |
6 × 10–4 mol L–1 s–1 | |
1 × 10–4 mol L–1 s–1 | |
3 × 10–4 mol L–1 s–1 |
Question 10 |
Half life period of a first order reaction is 1386 seconds. The specific rate constant of the reaction is [CBSE AIPMT 2009]
0.5 × 10–2 s–1 | |
0.5 × 10–3 s–1 | |
5.0 × 10–2 s–1 | |
5.0 × 10–3 s–1 |
Question 11 |
In the reaction
BrO3– (aq) + 5Br– (aq) + 6H+ → 3Br2 (l) + 3H2O(l)
The rate of appearance of bromine (Br2) is related to the rate of disappearance of bromide ions as [CBSE AIPMT 2009]
| |
| |
| |
|
Question 12 |
The half life period of a first order chemical reaction is 6.93 minutes. The time required for the completion of 99% of the chemical reaction will be (log 2 = 0.301) [AIEEE 2009]
230.3 minutes | |
23.03 minutes | |
46.06 minutes | |
460.6 minutes |
Question 13 |
Under the same
reaction conditions, initial concentration of 1.386 mol dm–3 of a
substance becomes half in 40 seconds and 20 seconds through first order and
zero order kinetics respectively. Ratio 
of the rate
constants for first order (k1) and zero order (k0) of
the reaction is [IIT JEE 2008]
0.5 mol–1 dm3 | |
1.0 mol–1 dm–3 | |
1.5 mol dm–3 | |
2.0 mol–1 dm–3 |
Question 14 |
The bromination of acetone that occurs in acid solution is represented by the equation
CH3COCH3(aq) + Br2(aq) → CH3COCH2Br(aq) + H+(aq) + Br–(aq)
These kinetic data were obtained from given reaction concentrations. [CBSE AIPMT 2008]
Initial concentrations, (M)
|
[CH3COCH3] |
[Br2] |
[H+] |
|
0.30 |
0.05 |
0.05 |
|
0.30 |
0.10 |
0.05 |
|
0.30 |
0.10 |
0.10 |
|
0.40 |
0.05 |
0.20 |
Initial Rate, disappearance of Br2, Ms–1
5.7 × 10–5
5.7 × 10–5
1.2 × 10–4
3.1 × 10–4
Based on these data, the rate of reaction is
rate = k [CH3COCH3] [Br2] | |
rate = k [CH3COCH3] [Br2] [H+]2 | |
rate = k[CH3COCH3][Br2] [H+] | |
rate = k[CH3COCH3] [H+] |
Question 15 |
The rate constants k1 and k2 for two different reactions are 1016 × e–2000/T and 1015 × e–1000/T, respectively. The temperature at which k1 = k2 is [CBSE AIPMT 2008]
| |
2000 K | |
| |
1000 K |
