For a given reaction $t_{1/2} = \frac{1}{k \cdot a}$,the order of reaction will be:

For the reaction $A \to xP$,when $[A] = 2.2 \, mM$,the rate was found to be $2.4 \, mM \, s^{-1}$. On reducing the concentration of $A$ to half,the rate changes to $0.6 \, mM \, s^{-1}$. The order of reaction with respect to $A$ is

If in a certain reaction,two different reactants take part,then:

The rate constant for the reaction $A \longrightarrow B$ is $2 \times 10^{-4} \ L \ mol^{-1} \ min^{-1}$. The concentration of $A$ at which the rate of the reaction is $(1 / 12) \times 10^{-5} \ M \ sec^{-1}$ is :-

The conversion of $A \to B$ follows second order kinetics. Doubling the concentration of $A$ will increase the rate of formation of $B$ by a factor of:

The reaction $2N_2O_5 \rightleftharpoons 4NO_2 + O_2$ follows first order kinetics. Hence,the molecularity of the reaction is