The rate constant of a second-order reaction is
10^–2 mol^–1 litre s^–1 . The rate constant expressed in cc molecule^–1 min^–1 is:

1. 9.96 × 10^–22

2. 9.96 × 10^–23

3. 9.96 × 10^–21

4. 1.004 × 10^–24

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):

1. 23.03 minutes

2. 46.06 minutes

3. 460.6 minutes

4. 230.3 minutes

A drop of solution (volume 0.05 mL) contains 3.0 x10^-6 mole of H⁺. If the rate constant of disappearance of H+ is 1.0x10⁷ mol litre sec?. How long would it take for H⁺ in drop to disappear?

1. 6x10^-8 sec

2. 6x10^-7 sec

3. 6x10^-9 sec

4. 6x10^-10 sec

Identify the correct statement for a zero-order reaction.

1. A reaction in which reactants do not react

2. A reaction in which one reactant is present in large excess

3. A reaction whose rate remains constant with time

4. A reaction whose rate increases with time

For A + B $\to \hspace{0.17em}$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.

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

The rate constant value for a zero-order reaction is 2 x10^-2 mol L^-1 sec^-1. If the concentration of the reactant after 25 sec is 0.5 M, then the initial concentration of reactant is: 

1. 0.5 M

2. 1.25 M

3. 12.5M

4. 1.0 M

The rate constant for a second order reaction is 8x10^-5 M^-1 min^-1 . How long will it take a 1M solution to be reduced to 0.5M?

1. 8.665 x 10³ minute

2. 8 x 10^-5 minute

3. 1.25 x 10⁴ minute

4. 4x10^-5 minute

The activation energy for a reaction is 9.0 kcal/mol. The increase in the rate constant when its temperature is increased from 298K to 308K is:

1. 10%

2. 100%

3. 50%

4. 63%