$A$ reaction is first order with respect to a reactant $A$ and second order with respect to reactant $B$. What is the effect on the rate when the concentration of both $A$ and $B$ is doubled?

If $a$ is the initial concentration of the reactant,the half-life period of the reaction of $n^{th}$ order is inversely proportional to

For a reaction,$I^{-} + OCl^{-} \to IO^{-} + Cl^{-}$ in an aqueous medium,the rate of reaction is given by $\frac{d[IO^{-}]}{dt} = k[I^{-}][OCl^{-}]$. The overall order of reaction is

For the reaction $2A + B \rightarrow C$,the rate law is given by $\text{Rate} = k[A][B]$. Which of the following statements is correct for this reaction?

The following data are for the decomposition of ammonium nitrate in aqueous solution. The order of the reaction is:

$N_2$ volume in $cc$ $(V_t)$	$6.25$	$9.50$	$11.42$	$13.65$	$35.05$ $(V_{\infty})$
Time $(t)$ in minutes	$10$	$15$	$20$	$25$	$\infty$

Consider the reaction between chlorine and nitric oxide:
$Cl_{2(g)} + 2NO_{(g)} \rightarrow 2NOCl_{(g)}$
On doubling the concentration of both reactants,the rate of the reaction increases by a factor of $8$. However,if only the concentration of $Cl_2$ is doubled,the rate increases by a factor of $2$. The order of this reaction with respect to $NO$ is :