The rate constant of a first-order reaction is\(4 \times 10^{-3} \mathrm{sec}^{-1}.\) At a reactant concentration of \(0.02~\mathrm{M},\) the rate of reaction would be:

1.	\(8 \times 10^{-5} \mathrm{M} ~\mathrm{sec}^{-1} \)	2.	\(4 \times 10^{-3} \mathrm{M} ~\mathrm{sec}^{-1} \)
3.	\(2 \times 10^{-1} \mathrm{M}~ \mathrm{sec}^{-1} \)	4.	\(4 \times 10^{-1} \mathrm{M}~ \mathrm{sec}^{-1}\)

For a first-order reaction A $\to$ Products, the rate of reaction at [A] = 0.2 M is 1.0 x 10^-2 mol litre^-1 min^-1. The half-life period for the reaction will be:

The following mechanism has been proposed for the reaction of NO with Br₂ to form NOBr:

NO(g) + Br₂(g) $\rightleftharpoons$ NOBr₂(g)

NOBr₂(g) + NO(g) $\to$2NOBr(g)

If the second step is the rate determining step, the order of the reaction with respect to NO(g) will be:

1. 1

2. 0

3. 3

4. 2

For a given reaction, the presence of a catalyst reduces the energy of activation by 2 kcal at 27 ^oC. The rate of reaction will be increased by:

1. 20 times

2. 14 times

3. 28 times

4. 2 times

A reaction A₂ + B₂ $\to$ 2AB occurs by the following mechanism:

A₂ $\to$ A + A               .....(slow)

A + B₂ $\to$ AB + B       .....(fast)

A + B $\to$ AB               .....(fast)

Its order would be:

1. 3/2

2. 1

3. 0

4. 2

For the elementary reaction M $\to$ N, the rate of disappearance of M increases by a factor of 8 upon doubling the concentration of M. The order of the reaction with respect to M will be:

1. 4

2. 3

3. 2

4. 1

For A + B $\to$C + D, $∆$H = -20 kJ mol^-1 , the activation energy of the forward reaction is 85 kJ mol^-1. The activation energy for the backward reaction is…. kJ mol^-1.

In the Arrhenius equation K = Ae^-E_a/RT, the quantity e^-E_a/kT is referred as:

1. Boltzmann factor.

2. Frequency factor.

3. Activation factor.

4. None of the above.

In the following reaction: xA →  yB

$\log \left(-\frac{d\left[A\right]}{d\mathrm{t }}\right)=$ $\log$ $\left(\frac{d\left[B\right]}{dt}\right)$ $+$ $0.3$ 

where the -ve sign indicates the rate of disappearance of the reactant. Then, x : y equals:

Half-life is independent of the concentration of a reactant. After 10 minutes, the volume of N₂ gas is 10 L and after complete reaction, it is 50 L. Hence, the rate constant is:

1. $\frac{2.303}{10}$log 5 min^-1

2. $\frac{2.303}{10}$ log 1.25 min^-1

3. $\frac{2.303}{10}$ log 2 min^-1

4. $\frac{2.303}{10}$ log 4 min^-1