For the reaction A + B → C + D, the initial rate for different reactions and initial concentration of reactants are given below: S.No Initial concentration Initial rate A mol L - 1 B mol L - 1 mol L - 1 s - 1 1 1 . 0 1 . 0 2 × 10 - 3 2 2 . 0 1 . 0 4 × 10 - 3 3 4 . 0 1 . 0 8 × 10 - 3 4 1 . 0 2 . 0 2 × 10 - 3 5 1 . 0 4 . 0 2 × 10 - 3 What is the overall order of reaction?

For the given reaction, rate = k [ A ] x [ B ] y . After substituting the values of initial rates and initial concentrations, the value of x and y can be calculated. Then ( x + y ) will give the order of the reaction. For experiment ( i ) 2 . 0 × 10 - 3 = [ 1 . 0 ] x [ 1 . 0 ] y For experiment ( ii ) 4 . 0 × 10 - 3 = [ 2 . 0 ] x [ 1 . 0 ] y For experiment ( iii ) 8 . 0 × 10 - 3 = [ 4 . 0 ] x [ 1 . 0 ] y For experiment ( iv ) 2 . 0 × 10 - 3 = [ 1 . 0 ] x [ 2 . 0 ] y For experiment ( v ) 2 . 0 × 10 - 3 = [ 1 . 0 ] x [ 4 . 0 ] y Determination of x . In order to get the value of x , divide equation (2) by (1) 4 . 0 × 10 - 3 2 . 0 × 10 − 3 = [ 2 . 0 ] x [ 1 . 0 ] y [ 1 . 0 ] x [ 1 . 0 ] y 2 1 = 2 x x = 1 Determination of y . In order to get the value of y , divide equation (4) by (1) 2 . 0 × 10 - 3 2 . 0 × 10 - 3 = [ 1 . 0 ] x [ 2 . 0 ] y [ 1 . 0 ] x [ 1 . 0 ] y y = 0 The overall order of reaction = 1 + 0 = 1

For the reaction A + B → C + D, the initial rate for different reactions and initial concentration of reactants are given below: S.No Initial concentration Initial rate A mol L - 1 B mol L - 1 mol L - 1 s - 1 1 1 . 0 1 . 0 2 × 10 - 3 2 2 . 0 1 . 0 4 × 10 - 3 3 4 . 0 1 . 0 8 × 10 - 3 4 1 . 0 2 . 0 2 × 10 - 3 5 1 . 0 4 . 0 2 × 10 - 3 Write the rate law equation.

For the given reaction, rate = k [ A ] x [ B ] y . After substituting the values of initial rates and initial concentrations, the value of x and y can be calculated. Then ( x + y ) will give the order of the reaction. For experiment ( i ) 2 . 0 × 10 - 3 = [ 1 . 0 ] x [ 1 . 0 ] y For experiment ( ii ) 4 . 0 × 10 - 3 = [ 2 . 0 ] x [ 1 . 0 ] y For experiment ( iii ) 8 . 0 × 10 - 3 = [ 4 . 0 ] x [ 1 . 0 ] y For experiment ( iv ) 2 . 0 × 10 - 3 = [ 1 . 0 ] x [ 2 . 0 ] y For experiment ( v ) 2 . 0 × 10 - 3 = [ 1 . 0 ] x [ 4 . 0 ] y Determination of x . In order to get the value of x , divide equation (2) by (1) 4 . 0 × 10 - 3 2 . 0 × 10 − 3 = [ 2 . 0 ] x [ 1 . 0 ] y [ 1 . 0 ] x [ 1 . 0 ] y 2 1 = 2 x x = 1 Determination of y . In order to get the value of y , divide equation (4) by (1) 2 . 0 × 10 - 3 2 . 0 × 10 - 3 = [ 1 . 0 ] x [ 2 . 0 ] y [ 1 . 0 ] x [ 1 . 0 ] y y = 0 The overall order of reaction = 1 + 0 = 1 The rate law (also known as the rate equation) for a chemical reaction is an expression that provides a relationship between the rate of the reaction and the concentrations of the reactants participating in it. Rate law, r α A 1 B 0 r α A 1 r = k A 1

Embibe Experts Solutions for Chapter: Chemical Kinetics, Exercise 1: ICSE-2019

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Embibe Experts Chemistry Solutions for Exercise - Embibe Experts Solutions for Chapter: Chemical Kinetics, Exercise 1: ICSE-2019

Attempt the free practice questions on Chapter 4: Chemical Kinetics, Exercise 1: ICSE-2019 with hints and solutions to strengthen your understanding. EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY solutions are prepared by Experienced Embibe Experts.

Questions from Embibe Experts Solutions for Chapter: Chemical Kinetics, Exercise 1: ICSE-2019 with Hints & Solutions

EASY

12th ICSE

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 4 - Chemical Kinetics>ICSE-2018>Q 3

The rate of reaction becomes four times when the temperature changes from $293 K$ to $313 K$ . Calculate the energy of activation $(E_{a})$ of the reaction assuming that it does not change with temperature. $(R = 8.314 J K^{- 1} {mol}^{- 1})$ .

EASY

12th ICSE

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 4 - Chemical Kinetics>ICSE-2018>Q 4

$40 %$ of a first order reaction is completed in $50$ minutes. How much time will it take for the completion of $80 %$ of this reaction?

EASY

12th ICSE

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 4 - Chemical Kinetics>ICSE-2019>Q 6

A catalyst is a substance which:

EASY

12th ICSE

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 4 - Chemical Kinetics>ICSE-2019>Q 7

For the reaction A + B → C + D, the initial rate for different reactions and initial concentration of reactants are given below:

S.No	Initial concentration		Initial rate
S.No	$[A] mol L^{- 1}$	$[B] mol L^{- 1}$	$mol L^{- 1} s^{- 1}$
$1$	$1.0$	$1.0$	$2 \times 10^{- 3}$
$2$	$2.0$	$1.0$	$4 \times 10^{- 3}$
$3$	$4.0$	$1.0$	$8 \times 10^{- 3}$
4	$1.0$	$2.0$	$2 \times 10^{- 3}$
5	$1.0$	$4.0$	$2 \times 10^{- 3}$

What is the overall order of reaction?

EASY

12th ICSE

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 4 - Chemical Kinetics>ICSE-2019>Q 8

For the reaction A + B → C + D, the initial rate for different reactions and initial concentration of reactants are given below:

S.No	Initial concentration		Initial rate
S.No	$[A] mol L^{- 1}$	$[B] mol L^{- 1}$	$mol L^{- 1} s^{- 1}$
$1$	$1.0$	$1.0$	$2 \times 10^{- 3}$
$2$	$2.0$	$1.0$	$4 \times 10^{- 3}$
$3$	$4.0$	$1.0$	$8 \times 10^{- 3}$
4	$1.0$	$2.0$	$2 \times 10^{- 3}$
5	$1.0$	$4.0$	$2 \times 10^{- 3}$

Write the rate law equation.

EASY

12th ICSE

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 4 - Chemical Kinetics>ICSE-2019>Q 9

25% of a first-order reaction is completed in 30 minutes. Calculate the time taken in minutes for the reaction to go to 90% completion.

EASY

12th ICSE

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 4 - Chemical Kinetics>ICSE-2019>Q 10

Show that for a first order reaction the time required to complete $75 %$ of reaction is about $2$ times more than that required to complete $50 %$ of the reaction.

MEDIUM

12th ICSE

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 4 - Chemical Kinetics>ICSE-2020>Q 11

A first order reaction is $50 %$ completed in $30$ minutes at $300 K$ and in $10$ minutes at $320 K$ . Calculate the activation energy of the reaction.

( $R = 8.314 J K^{- 1} {mol}^{- 1}$ ).

Embibe Experts Solutions for Chapter: Chemical Kinetics, Exercise 1: ICSE-2019

Embibe Experts Chemistry Solutions for Exercise - Embibe Experts Solutions for Chapter: Chemical Kinetics, Exercise 1: ICSE-2019

Questions from Embibe Experts Solutions for Chapter: Chemical Kinetics, Exercise 1: ICSE-2019 with Hints & Solutions

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