The reaction $2 NO + Br _2 \rightarrow 2 NOBr$

takes places through the mechanism given below :

$NO + Br _2 \Leftrightarrow NOBr _2 \text { (fast) }$

$NOBr _2+ NO \rightarrow 2 NOBr \text { (slow) }$

The overall order of the reaction is $.....$.

The three experimental data for determine the differential rate of reaction $Cl _{2( g )} + 2NO _{( g )} \rightarrow 2 NOCl_{( g )}$ at $310\, K$ temperature.

$(a)$ Derive differential rate of reaction.

$(b)$ Calculate order of reaction.

$(c)$ Calculate value of rate constant.

The rate law of the reaction $2{N_2}{O_5} \to 4N{O_2} + {O_2}$ is

The reaction $CH _{3} COF + H _{2} O \quad \rightleftharpoons CH _{3} COOH + HF$

Condition $I$ $:$ $\left[ H _{2} O \right]_{0}=1.00 \,M$

                           $\left[ CH _{3} COF \right]_{0}=0.01 \,M$

Condition $II$ $:$ $\left[ H _{2} O \right]_{0}=0.02 \,M$

                             $\left[ CH _{3} COF \right]_{0}=0.80 \,M$

Determine the order of reaction and calculate rate constant.

${A_2} + {B_2} \to 2AB;R.O.R = k{[{A_2}]^a}{[{B_2}]^b}$

Order of reaction with respect to $A_2$ and $B_2$ are respectively 

The dimension of rate constant of a second order reaction involves