11. A reaction proceeds through the formation of an intermediate B in a unimolecular reaction \[A\xrightarrow{{{k_a}}}B\xrightarrow{{{k_b}}}C\]
The integrated rate law for this reaction is
The integrated rate law for this reaction is
12. If ka ≫ kb, then concentration versus time plot for the reaction is
13. In a homogeneous catalytic reaction, 1.0 M of a substrate band 1.0 μM of a catalyst yields 1.0 mM of a product in 10 s. The turnover frequency (TOF) of the reaction (S-1) is
14. For the reaction, P + Q + R → S, experimental data for the measured initial rates is given below:
Expt.
Initial conc. P
(M)
Initial conc. Q
(M)
Initial conc. R
(M)
Initial rate
(m/s)
1
0.2
0.5
0.4
8.0 × 10-5
2
0.4
0.5
0.4
3.2 × 10-4
3
0.4
2.0
0.4
1.28 × 10-3
4
0.1
0.25
1.6
4.0 × 10-5
The order of the reaction with respect to P, Q and R respectively, is
| Expt. | Initial conc. P (M) |
Initial conc. Q (M) |
Initial conc. R (M) |
Initial rate (m/s) |
| 1 | 0.2 | 0.5 | 0.4 | 8.0 × 10-5 |
| 2 | 0.4 | 0.5 | 0.4 | 3.2 × 10-4 |
| 3 | 0.4 | 2.0 | 0.4 | 1.28 × 10-3 |
| 4 | 0.1 | 0.25 | 1.6 | 4.0 × 10-5 |
15. A reaction follows second order rate law, $$\frac{{ - d\left[ A \right]}}{{dt}} = k{\left[ A \right]^2},$$ if
16. The half-life (t1/2) for the hydrolysis of an ester varies with the initial concentration of the reactant ([E]0) as follows:
[E]0/10 mol/L
5.0
4.0
3.0
t1/2/s
240
300
400
The order of the reaction is
| [E]0/10 mol/L | 5.0 | 4.0 | 3.0 |
| t1/2/s | 240 | 300 | 400 |
17. The specific rate constant of decomposition of a compound is represented by $$\ln k = 5.0 - \frac{{12000}}{T}$$
The activation energy of decomposition foe this compound at 300 K is
The activation energy of decomposition foe this compound at 300 K is
18. In a consecutive first order reaction,
(where k1 and k2 are the respective rate constants) species B has transient existence. Therefore,
(where k1 and k2 are the respective rate constants) species B has transient existence. Therefore,