Consider the reaction :  N_2(g) + 3H_2(g) $$ \to $$ 2NH_3(g)

The equality relationship between $${{d\left[ {N{H_3}} \right]} \over {dt}}$$ and $$ - {{d\left[ {{H_2}} \right]} \over {dt}}$$ is

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