When the temperature of a reaction increases from 27 ^oC to 37 ^oC, the rate increases by 2.5 times. The activation energy in the temperature range will be:

1. 53.6 kJ                                             

2. 12.61 kJ

3. 7.08 kJ                                             

4. 70.8 kJ

The graph that represents a first-order reaction is:

1.		2.
3.		4.

The rate of a reaction increases 4-fold when concentration of reactant is increased 16 times.

If the rate of reaction is 4 × 10^-6 mol L^-1s^-1 when concentration of the reactant is 4 × 10^-4  mol L^-1, the rate constant of the reaction will be : 

1. 2 × 10^-4 m^1/2 L^-1/2 s^-1                            

2. 1 × 10^-2 s^-1

3. 4 × 10^-4 mol^-1/2 L^-1/2 s^-1                         

4. 25 mol^-1L min^-1                              

If ‘a’ is the initial concentration of a substance which reacts according to zero-order kinetics and k is the rate constant, the time for the reaction to go to completion will be:

The decomposition of a gaseous compound yields the following information:

For a given reaction the concentration of the reactant plotted against time gave a straight line with negative slope.

The order of the reaction will be:

1. 3                                                      

2. 2

3. 1                                                      

4. 0

The relationship between temperature and the variance in reaction rate is:

1.		2.
3.		4.

If a reaction A + B $\to$ C is exothermic to the extent of 30 kJ/mol and the forward reaction has an activation energy of 70 kJ/mol, the activation energy for the reverse reaction will be:

1. 30 kJ/mol                                       

2. 40kJ/mol

3. 70 kJ/mol                                       

4. 100 kJ/mol

A first-order reaction takes 40 min for 30 % decomposition. The t_1/2 for this reaction will be:

The half-life period for a first-order reaction is 20 minutes. The time required to change the concentration of the reactants from 0.08 M to 0.01 M will be: