For a certain reaction : $(A)(g)  \to  B(g)$ Half life for different initial pressures of $A$  is given below

 $\begin{array}{|l|l|l|} \hline {P_{{A_0}}}(atm) & 0.1 & 0.025 \\ \hline {t_{1/2}}(\sec\,\,) & 100 & 50 \\ \hline \end{array}$

The correct statement about order of reaction is

The reaction of ozone with oxygen atoms in the presence of chlorine atoms can occur by a two step process shown below

${O_3}(g)\, + \,C{l^ * }(g)\, \to \,{O_2}(g) + Cl{O^ * }(g)$ ..... $(i)$               $[{K_i} = 5.2 \times {10^9}\,\,L\,mo{l^{ - 1}}\,{s^{ - 1}}]$

$Cl{O^ * }(g) + {O^ * }(g)\, \to \,{O_2}(g) + \,C{l^ * }(g)$ ..... $(ii)$                $[{K_{ii}} = 2.6 \times {10^{10}}\,\,L\,mo{l^{ - 1}}\,{s^{ - 1}}]$

The closest rate constant for the overall reaction 

${O_3}(g){\mkern 1mu}  + {\mkern 1mu} {O^*}(g){\mkern 1mu}  \to {\mkern 1mu} 2{O_2}(g)$ is  ........... $L\,\,mo{l^{ - 1}}\,{s^{ - 1}}$

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

$(a)$ $2.1 \times 10^{-2}\,mol \,L ^{-1} \,s ^{-1}$

$(b)$ $4.5 \times 10^{-3} \,min ^{-1}$

$Zn + 2H^+ \to  Zn^{2+} + H_2$

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

The data for the reaction $A + B \to C$ isThe rate law corresponds to the above data is

Exp.	$[A]_0$	$[B]_0$	Initial rate
$(1)$	$0.012$	$0.035$	$0.10$
$(2)$	$0.024$	$0.070$	$0.80$
$(3)$	$0.024$	$0.035$	$0.10$
$(4)$	$0.012$	$0.070$	$0.80$

Assertion : The kinetics of the reaction -

$mA + nB + pC \to m' X + n 'Y + p 'Z$

obey the rate expression as $\frac{{dX}}{{dt}} = k{[A]^m}{[B]^n}$.

Reason : The rate of the reaction does not depend upon the concentration of $C$.