The time required for a definite fraction of a reaction to complete is inversely proportional to the initial concentration of the reactant. Find the order of the reaction.

The rate law for a reaction between the substances $A$ and $B$ is given by,$rate = k[A]^n[B]^m$. On doubling the concentration of $A$ and halving the concentration of $B$,the ratio of the new rate to the earlier rate of the reaction will be as

Which of the following statements is $NOT$ correct regarding the order of reaction?

For a particular reaction,the rate expression is given as $r = k[A][B]^{0.5}$. If the volume of the vessel is reduced to one-fourth of the initial volume,the rate of reaction would

For any reaction,the rate constant $K = 2.3 \times 10^{-5} \ mol^{-3/2} \ L^{3/2} \ S^{-1}$. The order of the reaction is . . . . . . .

Select the incorrect option :