Define following term / Give definition :

$(1)$ Rate law / Rate equation / Rate expression

$(2)$ Unimolecular reaction

Rate constant of reaction is $1.388 \times 10^{-3}\, mole^{-2}\,lit^{-2}\,sec^{-1}$ order of reaction will be

When the concentration of A in the reaction  $A + B$ $\rightleftharpoons$ $AB$ is doubled, the rate of reaction will be

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

$H _{2} O _{2}+ I ^{-} \rightarrow H _{2} O + IO ^{-}$

$H _{2} O _{2}+ IO ^{-} \rightarrow H _{2} O + I ^{-}+ O _{2}$

The instantaneous rate of disappearance of $MnO_4^-$ ion in the following reaction is $4.56\times10^{-3}\,Ms^{-1}$,  $2MnO_4^-+ 10I^-+ 16 H^+ \to  2 Mn^{2+} + 5I_2 + 8H_2O$ The rate of appearance $I_2$ is

Consider the following reaction,

$2 H _2( g )+2 NO ( g ) \rightarrow N _2( g )+2 H _2 O ( g )$

which following the mechanism given below:

$2 NO ( g ) \underset{ k _{-1}}{\stackrel{ k _1}{\rightleftharpoons}} N _2 O _2( g )$

$N _2 O _2( g )+ H _2( g ) \stackrel{ k _2}{\rightleftharpoons} N _2 O ( g )+ H _2 O ( g )$

$N _2 O ( g )+ H _2( g ) \stackrel{ k _3}{\rightleftharpoons} N _2( g )+ H _2 O ( g )$

(fast equilibrium)

(slow reaction)

(fast reaction)

The order of the reaction is