The dimension of rate constant of a second order reaction involves

Write unit of rate constant of following reaction :

$1.$ $\frac {1}{2}$ order

$2.$ $\frac {3}{2}$ order

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

Consider a reaction $\mathrm{aG}+\mathrm{bH} \rightarrow$ Products. When concentration of both the reactants $\mathrm{G}$ and $\mathrm{H}$ is doubled, the rate increases by eight times. However, when concentration of $\mathrm{G}$ is doubled keeping the concentration of $\mathrm{H}$ fixed, the rate is doubled. The overall order of the reaction is

Mechanism of a hypothetical reaction

$X_2 + Y_2 \rightarrow 2XY,$ is given below :

$(i)\,\, X_2 \rightarrow X + X\, (fast)$

$(ii)\,\,X + Y_2 \rightleftharpoons XY + Y\, (slow)$

$(iii)\,\,X + Y \rightarrow XY\, (fast)$

The overall order of the reaction will be

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

$2 HI \rightarrow H _{2}+ I _{2}$

$2 NO _{( g )}+ O _{2( g )} \rightarrow 2 NO _{2( g )}$