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

For an elementary chemical reaction, ${A_2} \underset{{{k_{ - 1}}}}{\overset{{{k_1}}}{\longleftrightarrow}} 2A$ the expression for $\frac{{d\left[ A \right]}}{{dt}}$ 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

The rate law for the reaction$RCl + NaOH(aq) \to ROH + NaCl$ is given by Rate $ = {K_1}[RCl]$. The rate of the reaction will be

The instantaneous rate of disappearance of $MnO_4^-$ ion in the following reaction is $4.56\times10^{-3}\,Ms^{-1}$,  $2MnO_4^-+ 10I^-+ 16 H^+ \to  2 Mn^{2+} + 5I_2 + 8H_2O$ The rate of appearance $I_2$ is

Which of the following is correct