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

For the decomposition of azoisopropane to hexane and nitrogen at $543$ $K ,$ the following data are obtained.

Calculate the rate constant.

For the reaction $A + 2B \to C,$ rate is given by $R$ $ = [A]{[B]^2}$ then the order of the reaction is

The rate of the reaction becomes twice when the concentration of reactant becomes $8$ times then the order of the reaction is

$Zn + 2H^+ \to  Zn^{2+} + H_2$

The half-life period is independent of the concentration of zinc at constant $pH$. For the constant concentration of $Zn$, the rate becomes $100$ times when $pH$ is decreased from $3\, to\, 2$. Identify the correct statements $(pH = -\log [H^{+}])$

$(A)$  $\frac{{dx}}{{dt}}\, = k{[Zn]^0}{[{H^ + }]^2}$

$(B)$  $\frac{{dx}}{{dt}}\, = k{[Zn]}{[{H^ + }]^2}$

$(C)$ Rate is not affected if the concentraton of zinc is made four times and that of $H^+$ ion is halved.

$(D)$ Rate becomes four times if the concentration of $H^+$ ion is doubled at constant $Zn$ concentration

For the reaction $2NO_2 + F_2 \to 2NO_2F$ , following mechanism has been provided

$N{O_2} + {F_2}\xrightarrow{{slow}}N{O_2}F + F$

$N{O_2} + F\xrightarrow{{fast}}N{O_2}F$

Thus rate expression of the above reaction can be written as