(C) Let the rate law be $Rate = k[P_{NO}]^x [P_{H_2}]^y$.Comparing experiments $1$ and $2$ where $[P_{H_2}]$ is constant:$\frac{Rate_1}{Rate_2} = (\fr

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

(C) Let the rate law be $Rate = k[P_{NO}]^x [P_{H_2}]^y$.Comparing experiments $1$ and $2$ where $[P_{H_2}]$ is constant:$\frac{Rate_1}{Rate_2} = (\frac{P_{NO,1}}{P_{NO,2}})^x$$\frac{0.135}{0.033} \approx 4.09 \approx 4$$(\frac{40.0}{20.1})^x \approx 2^x$$4 = 2^x \implies x = 2$.Thus,the order of the reaction with respect to $NO$ is $2$.

Class 12 Chemistry Chemical Kinetics Rate law , Rate constant , Order of Reaction and Molecularity

Medium

$2 \ NO + 2 \ H_2 \rightarrow N_2 + 2 \ H_2O$
The above reaction has been studied at $800^{\circ} C$. The related data are given in the table below.

Reaction serial number Initial pressure of $H_2$ / $kPa$ Initial Pressure of $NO$ / $kPa$ Initial rate $(-\frac{dp}{dt}) / (kPa \ s^{-1})$

$1$ $65.6$ $40.0$ $0.135$

$2$ $65.6$ $20.1$ $0.033$

$3$ $38.6$ $65.6$ $0.214$

$4$ $19.2$ $65.6$ $0.106$

The order of the reaction with respect to $NO$ is $...........$

JEE MAIN 2022 All JEE MAIN

A
$1$
B
$0$
C
$2$
D
$3$

Explore More

Browse All

Question Bank

All Subjects

Class 12 Questions

Class 12

Chemistry Questions

Chapter

Chemical Kinetics

Subtopic

Rate law , Rate constant , Order of Reaction and Molecularity

Previous Year

JEE MAIN 2022 Paper All JEE MAIN years →

$A$ study of chemical kinetics of the reaction $A + B \to$ Products,gave the following data at $25 \ ^oC$.

$Exp. \ No.$ $[A]$ $[B]$ $Rate$

$1.$ $1.0$ $0.15$ $4.2 \times 10^{-6}$

$2.$ $2.0$ $0.15$ $8.4 \times 10^{-6}$

$3.$ $1.0$ $0.20$ $5.6 \times 10^{-6}$

Find out the rate law.

Medium

View Solution

For the following rate law,determine the unit of the rate constant: Rate $= -\frac{d[R]}{dt} = k[A]^{\frac{1}{2}}[B]^{2}$

Difficult

View Solution

Which of the following for a chemical reaction can never be a fraction?

Easy

View Solution

For the gaseous reaction,$N_2O_5 \rightarrow 2NO_2 + \frac{1}{2}O_2$,the rate can be expressed as:
$-\frac{d[N_2O_5]}{dt} = K_1[N_2O_5]$
$+\frac{d[NO_2]}{dt} = K_2[N_2O_5]$
$+\frac{d[O_2]}{dt} = K_3[N_2O_5]$
The correct relation between $K_1, K_2$ and $K_3$ is:

MediumTS EAMCET 2024

View Solution

In the given reaction sequence,if $K_3 > K_2 > K_1$,then the rate-determining step is:

Easy

View Solution

Vedclass Products

For Students

Vedclass Test Series

Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.

Start Free Trial

For Teachers

Exam Paper Generator

Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.

Try Free

For Institutes

Online Exam Module

Live online exams with unlimited students, 360° analytics & white-label branding.

See Demo

Reaction serial number	Initial pressure of $H_2$ / $kPa$	Initial Pressure of $NO$ / $kPa$	Initial rate $(-\frac{dp}{dt}) / (kPa \ s^{-1})$
$1$	$65.6$	$40.0$	$0.135$
$2$	$65.6$	$20.1$	$0.033$
$3$	$38.6$	$65.6$	$0.214$
$4$	$19.2$	$65.6$	$0.106$

$Exp. \ No.$	$[A]$	$[B]$	$Rate$
$1.$	$1.0$	$0.15$	$4.2 \times 10^{-6}$
$2.$	$2.0$	$0.15$	$8.4 \times 10^{-6}$
$3.$	$1.0$	$0.20$	$5.6 \times 10^{-6}$

Similar Questions

$A$ study of chemical kinetics of the reaction $A + B \to$ Products,gave the following data at $25 \ ^oC$. $Exp. \ No.$ $[A]$ $[B]$ $Rate$ $1.$ $1.0$ $0.15$ $4.2 \times 10^{-6}$ $2.$ $2.0$ $0.15$ $8.4 \times 10^{-6}$ $3.$ $1.0$ $0.20$ $5.6 \times 10^{-6}$ Find out the rate law.

For the following rate law,determine the unit of the rate constant: Rate $= -\frac{d[R]}{dt} = k[A]^{\frac{1}{2}}[B]^{2}$

Which of the following for a chemical reaction can never be a fraction?

For the gaseous reaction,$N_2O_5 \rightarrow 2NO_2 + \frac{1}{2}O_2$,the rate can be expressed as:$-\frac{d[N_2O_5]}{dt} = K_1[N_2O_5]$$+\frac{d[NO_2]}{dt} = K_2[N_2O_5]$$+\frac{d[O_2]}{dt} = K_3[N_2O_5]$The correct relation between $K_1, K_2$ and $K_3$ is:

In the given reaction sequence,if $K_3 > K_2 > K_1$,then the rate-determining step is:

Vedclass Test Series

Exam Paper Generator

Online Exam Module

$A$ study of chemical kinetics of the reaction $A + B \to$ Products,gave the following data at $25 \ ^oC$.

$Exp. \ No.$ $[A]$ $[B]$ $Rate$

$1.$ $1.0$ $0.15$ $4.2 \times 10^{-6}$

$2.$ $2.0$ $0.15$ $8.4 \times 10^{-6}$

$3.$ $1.0$ $0.20$ $5.6 \times 10^{-6}$

Find out the rate law.

For the gaseous reaction,$N_2O_5 \rightarrow 2NO_2 + \frac{1}{2}O_2$,the rate can be expressed as:
$-\frac{d[N_2O_5]}{dt} = K_1[N_2O_5]$
$+\frac{d[NO_2]}{dt} = K_2[N_2O_5]$
$+\frac{d[O_2]}{dt} = K_3[N_2O_5]$
The correct relation between $K_1, K_2$ and $K_3$ is: