Medium
Write the differential rate expression for the following reactions and determine their order of reaction:
$1. CHCl_3 + Cl_2 \rightarrow CCl_4 + HCl$
$2. CH_3COOC_2H_5 + H_2O \rightarrow CH_3COOH + C_2H_5OH$
$1. CHCl_3 + Cl_2 \rightarrow CCl_4 + HCl$
$2. CH_3COOC_2H_5 + H_2O \rightarrow CH_3COOH + C_2H_5OH$
(N/A) For reaction $1$: $CHCl_3 + Cl_2 \rightarrow CCl_4 + HCl$
The experimental rate law is $Rate = k[CHCl_3][Cl_2]^{1/2}$.
The differential rate expression is: $-\frac{d[CHCl_3]}{dt} = -\frac{d[Cl_2]}{dt} = \frac{d[CCl_4]}{dt} = \frac{d[HCl]}{dt} = k[CHCl_3][Cl_2]^{1/2}$.
The order of reaction is $1 + 1/2 = 1.5$.
For reaction $2$: $CH_3COOC_2H_5 + H_2O \rightarrow CH_3COOH + C_2H_5OH$
This is a pseudo-first-order reaction because water is in large excess.
The experimental rate law is $Rate = k'[CH_3COOC_2H_5]$.
The differential rate expression is: $-\frac{d[CH_3COOC_2H_5]}{dt} = k'[CH_3COOC_2H_5]$.
The order of reaction is $1$.
The experimental rate law is $Rate = k[CHCl_3][Cl_2]^{1/2}$.
The differential rate expression is: $-\frac{d[CHCl_3]}{dt} = -\frac{d[Cl_2]}{dt} = \frac{d[CCl_4]}{dt} = \frac{d[HCl]}{dt} = k[CHCl_3][Cl_2]^{1/2}$.
The order of reaction is $1 + 1/2 = 1.5$.
For reaction $2$: $CH_3COOC_2H_5 + H_2O \rightarrow CH_3COOH + C_2H_5OH$
This is a pseudo-first-order reaction because water is in large excess.
The experimental rate law is $Rate = k'[CH_3COOC_2H_5]$.
The differential rate expression is: $-\frac{d[CH_3COOC_2H_5]}{dt} = k'[CH_3COOC_2H_5]$.
The order of reaction is $1$.
Explore More
Similar Questions
What is the molecularity of the following reactions?
$1.$ $NH_4NO_2(s) \rightarrow N_2(g) + 2H_2O(l)$
$2.$ $2HI(g) \rightarrow H_2(g) + I_2(g)$
$3.$ $2NO(g) + O_2(g) \rightarrow 2NO_2(g)$
$1.$ $NH_4NO_2(s) \rightarrow N_2(g) + 2H_2O(l)$
$2.$ $2HI(g) \rightarrow H_2(g) + I_2(g)$
$3.$ $2NO(g) + O_2(g) \rightarrow 2NO_2(g)$
Difficult
View SolutionFor a reaction $A \to B$,the rate of reaction quadrupled when the concentration of $A$ is doubled. The rate expression of the reaction is $r = K[A]^n$. The value of $n$ is
Easy
View SolutionThe rate equation for the reaction $2A + B \longrightarrow \text{products}$ is $\text{rate} = k[A][B]^2$. If $k$ at $T \, K$ is $5.0 \times 10^{-6} \, mol^{-2} \, L^2 \, s^{-1}$,the initial rate of the reaction,when $[A] = 0.05 \, mol \, L^{-1}$ and $[B] = 0.1 \, mol \, L^{-1}$ is:
Write the general reaction,its differential rate equation,and the rate law.
Difficult
View SolutionConsider the following reaction $A + B \rightarrow C$.
The time taken for $A$ to become $1/4$ of its initial concentration is twice the time taken to become $1/2$ of the same. Also,when the change of concentration of $B$ is plotted against time,the resulting graph gives a straight line with a negative slope and a positive intercept on the concentration axis. The overall order of the reaction is . . . . .
The time taken for $A$ to become $1/4$ of its initial concentration is twice the time taken to become $1/2$ of the same. Also,when the change of concentration of $B$ is plotted against time,the resulting graph gives a straight line with a negative slope and a positive intercept on the concentration axis. The overall order of the reaction is . . . . .
Vedclass Products
For Students
Vedclass Test Series
Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.
Start Free TrialFor Teachers
Exam Paper Generator
Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.
Try FreeFor Institutes
Online Exam Module
Live online exams with unlimited students, 360° analytics & white-label branding.
See Demo