For a first order reaction A $$ \to $$ B the reaction rate a reactant concentration of 0.01 M is found to be 2.0 $$ \times $$ 10^$$-$$5 mol L^$$-$$1 s^$$-$$1. The half-life period of the reaction is

The rate of reaction between two reactions A and B decreases by a factor of 4 if the concentration of reactant B is doubled. The order of this reaction with respect to reactant B is

The rate of a first order reaction is 1.5 $$ \times $$ 10^$$-$$2 mol L^$$-$$1 min^$$-$$1 at 0.5 M concentration of the reactant. The half-life of the reaction is

The temperature dependence of rate constant (k) of a chemical reaction is written in terms of Arrhenius equation, $$k = A \cdot {e^{ - E{}^ * /RT}}$$. Activation energy (E^{$$ * $$}) of the reaction can be calculated by plotting