Consider the following data for the given reaction  $2 \mathrm{HI}_{(\mathrm{g})} \rightarrow \mathrm{H}_{2(\mathrm{~g})}+\mathrm{I}_{2(\mathrm{~g})}$ .  The order of the reaction is................

	$1$	$2$	$3$
$\mathrm{HI}\left(\mathrm{mol} \mathrm{L}^{-1}\right)$	$0.005$	$0.01$	$0.02$
Rate $\left(\mathrm{mol} \mathrm{L}^{-1} \mathrm{~s}-1\right)$	$7.5 \times 10^{-4}$	$3.0 \times 10^{-3}$	$1.2 \times 10^{-2}$

The conversion of molecules $X$ to $Y$ follows second order kinetics. If concentration of $X$ is increased to three times how will it affect the rate of formation of $Y ?$

The reaction $2{N_2}{O_5}$ $\rightleftharpoons$ $2N{O_2} + {O_2}$ follows first order kinetics. Hence, the molecularity of the reaction is

Which of the following rate laws has an overall order of $0.5$  for reaction involving substances $x$, $y$ and $z$

Reaction rate between two substance $A$ and $B$ is expressed as following $:$ rate $= k[A ]^n[B]^m$ If the concentration of $A$ is doubled and concentration of $B$ is made half of initial concentration, the ratio of the new rate to the earlier rate will be

For the non-stoichiometric reaction $2A + B \to C + D,$ the following kinetic data were  obtained in three separate experiments, all at $298\,K$.

For the reaction the rate of formation of $C$ will be