Calculate the order of the reaction in $A$ and $B$

$A$        $(mol/l)$	$B$      $(mol/l)$	Rate
$0.05$	$0.05$	$1.2\times 10^{-3}$
$0.10$	$0.05$	$2.4\times 10^{-3}$
$0.05$	$0.10$	$1.2\times 10^{-3}$

$Zn + 2H^+ \to  Zn^{2+} + H_2$

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 reaction, ${N_2}{O_5} \longrightarrow 2NO + \frac{1}{2}\,{O_2}$ is of first order for $N_2O_5$ with rate constant $6.2 \times 10^{-4}\, s^{-1}$. what is the value of rate of reaction when $[N_2O_5] = 1.25\, mol\, L^{-1}$

The rate constant for the reaction, $2{N_2}{O_5} \to 4N{O_2}$ $ + {O_2}$ is $3 \times {10^{ - 5}}{\sec ^{ - 1}}$. If the rate is $2.40 \times {10^{ - 5}}\,mol\,\,litr{e^{{\rm{ - 1}}}}{\sec ^{ - 1}}$. Then the concentration of ${N_2}{O_5}$ (in mol litre $^{-1}$) is

Write differential rate expression of following reaction and give its order of reaction :

$5 B r^{-}+B r O_{3}^-+6 H^{+} \rightarrow 3 B r_{2}+3 H_{2} O$

Reaction : $KCl{O_3} + 6FeS{O_4} + 3{H_2}S{O_4} \to $ $KCl + 3F{e_2}{\left( {S{O_4}} \right)_3} + 3{H_2}O$

Which is True $(T)$ and False $(F) $ in the following sentence ?

The reaction is complex.