For a chemical reaction,$ A + 2B \to C + D,$ the rate of reaction increases three times, when concentration of $A$ only is increased nine times. While when concentration of $B$ only is increased $2\,times,$ then rate of reaction also increases $2\,times$. The order of this reaction is

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

Following is the rate constant of reaction what is the overall order of reaction ?

$(a)$ $2.418 \times 10^{-5}\,hr ^{-1}$

$(b)$ $7.1 \times 10^{-4} \,atm \,s ^{-1}$

Consider the reaction, $2A + B \rightarrow$ products. When concentration of $B$ alone was doubled, the half-life did not change. When the concentration of $A$ alone was doubled, the rate increased by two times. The unit of rate constant for this reaction is

For the reaction $C{H_3}COOC{H_3} + {H_2}O\xrightarrow{{{H^ + }}}$ $C{H_3}COOH + C{H_3}OH$ The progress of the process of reaction is followed by

Differential form of the rate equation is

$\frac{{dx}}{{dt}} = k\left[ P \right]{\left[ Q \right]^{0.5}}{\left[ R \right]^{0.5}}$ 

Which statement about the above equation is wrong?