The unit of rate constant for a zero-order reaction is:
1.
2.
3.
4.
The half-life of a certain enzyme catalysed reaction is 138 s, that follow the 1st order kinetics. The time required for the concentration of the substance to fall from 1.28 mg L–1 to 0.04 mg L–1, is:
1. 276 s
2. 414 s
3. 552 s
4. 690 s
The rate of the reaction can be written in three ways:
The relationship between k and k′ and between
k and k′′ are-
1. k′ = k, k′′= k
2. k′= 2k; k′′= k
3. k′= 2k, k′′= k/2
4. k′ = 2k; k′′= 2k
The rate of the reaction
2NO + Cl2 → 2NOCl is given by the rate equation
rate = k[NO]2[Cl2]
The value of the rate constant can be increased by:
1. Increasing the concentration of NO
2. Increasing the concentration of Cl2
3. Increasing the temperature
4. All of the above
Activation energy and rate constant (k1 and k2) of a chemical reaction at two different temperatures (T1 and T2) are related by:
1. | \(\ln \frac{k_2}{k_1}=-\frac{E_a}{R}\left(\frac{1}{T_2}-\frac{1}{T_1}\right)\) |
2. | \(\ln \frac{k_2}{k_1}=-\frac{E_a}{R}\left(\frac{1}{T_2}+\frac{1}{T_1}\right)\) |
3. | \(\ln \frac{k_2}{k_1}=\frac{E_a}{R}\left(\frac{1}{T_2}-\frac{1}{T_1}\right)\) |
4. | \(\ln \frac{k_2}{k_1}=-\frac{E_a}{R}\left(\frac{1}{T_1}-\frac{1}{T_2}\right)\) |
1. | 12 | 2. | 16 |
3. | 32 | 4. | 10 |
1. | 1 | 2. | 2 |
3. | 3 | 4. | 0 |
Consider the reaction
N2(g) + 3H2(g) → 2NH3(g)
The equality relationship between \(
\frac{{d}\left[{{NH}_{3}}\right]}{dt}\) and \(
{-}\frac{{d}\left[{{H}_{2}}\right]}{dt}\) is :
1.
2.
3.
4.
For the reaction, \(2 A+B \rightarrow 3 C+D\)
An incorrect expression for the rate of reaction is:
1. | \(-\frac{d[C]}{3} d t \) | 2. | \(-\frac{d[B]}{d t} \) |
3. | \(\frac{d[D]}{d t} \) | 4. | \(-\frac{d[A]}{2 d t}\) |
If 60% of a first-order reaction was completed in 60 min, 50% of the same reaction would be completed in approximately:
(log 4 = 0.60, log 5 = 0.69)
1. | 50 min | 2. | 45 min |
3. | 60 min | 4. | 40 min |