State a condition under which a bimolecular reaction is kinetically first order reaction.
State a condition under which a bimolecular reaction is kinetically first order reaction.
A bimolecular reaction becomes first order reaction when one of the reactant is in excess.
$\underset{\text { Ethyl acetate }}{\mathrm{CH}_{3} \mathrm{COOC}_{2} \mathrm{H}_{5}+}+\mathrm{H}_{2} \mathrm{O} \rightarrow \underset{\text { Ethenoic acid }}{\mathrm{CH}_{3} \mathrm{COOH}}+\underset{\begin{array}{l}\mathrm{CO}_{2} \mathrm{H}_{5} \mathrm{OH} \\ \text { Ethenol }\end{array}}{\mathrm{C}}$
This reaction is bimolecular but its order depends only on conc. of $\mathrm{CH}_{3} \mathrm{COOC}_{2} \mathrm{H}_{5}$ and $\left[\mathrm{H}_{2} \mathrm{O}\right]$ almost remain constant.
Similar Questions
Consider the reaction between chlorine and nitric oxide
$Cl _{2}( g )+2 NO ( g ) \rightarrow 2 NOCl ( g )$
On doubling the concentration of both reactants, the rate of the reaction increases by a factor of $8 .$ However, if only the concentration of $C l_{2}$ is doubled, the rate increases by a factor of $2 .$ The order of this reaction with respect to $NO$ is :
Consider the reaction between chlorine and nitric oxide
$Cl _{2}( g )+2 NO ( g ) \rightarrow 2 NOCl ( g )$
On doubling the concentration of both reactants, the rate of the reaction increases by a factor of $8 .$ However, if only the concentration of $C l_{2}$ is doubled, the rate increases by a factor of $2 .$ The order of this reaction with respect to $NO$ is :
- [NEET 2017]
From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.
$(ii)$ $H _{2} O _{2}( aq )+3 I ^{-}( aq )+2 H ^{+} \rightarrow 2 H _{2} O ( l )+ I _{3}^{-} \quad$ Rate $=k\left[ H _{2} O _{2}\right][ I ]$
From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.
$(ii)$ $H _{2} O _{2}( aq )+3 I ^{-}( aq )+2 H ^{+} \rightarrow 2 H _{2} O ( l )+ I _{3}^{-} \quad$ Rate $=k\left[ H _{2} O _{2}\right][ I ]$
The three experimental data for determine the differential rate of reaction $2 NO _{( g )}+ Cl _{2( g )} \rightarrow 2 NOCl_{( g )}$ at definate temperature. are given below.
$(a)$ Calculate order of reaction.
$(b)$ Calculate value of rate constant.
The three experimental data for determine the differential rate of reaction $2 NO _{( g )}+ Cl _{2( g )} \rightarrow 2 NOCl_{( g )}$ at definate temperature. are given below.
$(a)$ Calculate order of reaction.
$(b)$ Calculate value of rate constant.
Half-life period of a first order reaction is $1386$ seconds. The specific rate constant of the reaction is
Half-life period of a first order reaction is $1386$ seconds. The specific rate constant of the reaction is
- [AIPMT 2009]
What is the order of reaction $r\, = \,k{[A]^{\frac{3}{2}}}\,{[B]^2}$ ?
What is the order of reaction $r\, = \,k{[A]^{\frac{3}{2}}}\,{[B]^2}$ ?