Reaction : $2Br^{-} + H_2O_2 + 2H^{+} \to  Br_2 + 2H_2O$

take place in two steps :

$(a)$ $Br^{-} + H^{+} + H_2O_2 \xrightarrow{{slow}} HOBr + H_2O$

$(b)$ $HOBr + Br^{-} + H^{+} \xrightarrow{{fast}} H_2O + Br_2$

The order of the reaction is 

For which order reaction a straight line is obtained along with $x\,-$ axis by plotting a graph between half life $({t_{1/2}})$ and initial concentration $ 'a'$

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

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

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

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

For a reaction between $A$ and $B$ the order with respect to $A$ is $2$ and the other with respect to $B$ is $3.$ The concentrations of both $A$ and $B$ are doubled, the rate will increase by a factor of

Catalyst decomposition of hydrogen peroxide is a ........ order reaction