If $R = K{[NO]^2}[{O_2}],$ rate constant may be increased by

The rate of the reaction :

$2N_2O_5 \rightarrow 4NO_2 + O_2$ can be written in three ways.

$\frac{-d[N_2O_5 ]}{dt} = k[N_2O_5]$

$\frac{d[NO_2 ]}{dt} = k'[N_2O_5]\,;$   $\frac{d[O_2 ]}{dt} = k"[N_2O_5]$

The relationship between $k$ and $k'$ and betweenk and $k''$ are

units of rate constant of first and zero order reactions in terms of molarity $M$ unit are respectively

In a chemical reaction $A$ is converted into $B$ . The rates of reaction, starting with initial concentrations of $A$ as $2 \times {10^{ - 3}}\,M$ and $1 \times {10^{ - 3}}\,M$ , are equal to $2.40 \times {10^{ - 4}}\,M{s^{ - 1}}$ and $0.60 \times {10^{ - 4}}\,M{s^{ - 1}}$ respectively. The order of reaction with respect to reactant $A$ will be

For reaction

$Cl_2(aq) + H_2S(aq) \to S(s) + 2H^+(aq) + 2Cl^-(aq)$ rate law is $r = K[Cl_2][H_2S]$
then which of these mechanism is/are consistent with this rate law

$(A)\, H_2S \rightleftharpoons  H^+ + HS^-$ (fast)

         $Cl_2 + HS^-\to 2Cl^-+ H^+ + S$ (slow)

$(B)\, Cl_2 + H_2S \to H^+ + Cl^-+ Cl^+ + HS^-$ (slow)

          $Cl^+ + HS^-\to H^+ + Cl^-+ S$ (fast)

The half-life of $2 $ sample are $0.1 $ and $ 0.4 $ seconds. Their respective concentration are $200 $ and  $ 50 $ respectively. What is the order of the reaction