For a reaction between A and B the order with respect to A is 2 and the order with respect to B is 3. The concentration of both A and B is doubled the rate will increase by a factor of:

1.	12	2.	16
3.	32	4.	10

Activation energy $E_a$ and rate constant (k₁ and k₂) of a chemical reaction at two different temperatures (T₁ and T₂) are related by:

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

The rate of the reaction $2{\mathrm{N}}_2{\mathrm{O}}_5\to 4{\mathrm{NO}}_2+{\mathrm{O}}_2$  can be written in three ways:

$\frac{-d\left[N_2{O}_5\right]}{dt}=k\left[N_2{O}_5\right]$
$\frac{d\left[N{O}_2\right]}{dt}=k\text{'}\left[N_2{O}_5\right]$
$\frac{d\left[O_2\right]}{dt}=k\text{'}\text{'}\left[N_2{O}_5\right]$

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 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 unit of rate constant for a zero-order reaction is:

1. ${\mathrm{s}}^{-1}$

2. $\mathrm{mol}$ ${\mathrm{L}}^{-1}{\mathrm{s}}^{-1}$

3. $\mathrm{L}$ ${\mathrm{mol}}^{-1}{\mathrm{s}}^{-1}$

4. ${\mathrm{L}}^2{\mathrm{mol}}^{-2}{\mathrm{s}}^{-1}$

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. $\frac{d\left[N{H}_3\right]}{dt}=-\frac{1}{3}\frac{d\left[H_2\right]}{dt}$

2. $+\frac{d\left[N{H}_3\right]}{dt}=-\frac{2}{3}\frac{d\left[H_2\right]}{dt}$

3. $+\frac{d\left[N{H}_3\right]}{dt}=-\frac{3}{2}\frac{d\left[H_2\right]}{dt}$

4. $+\frac{d\left[N{H}_3\right]}{dt}=-\frac{d\left[H_2\right]}{dt}$

For the reaction, \(2 A+B \rightarrow 3 C+D\)

An incorrect expression for the rate of reaction is:

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)