(C) The rate law is given by $Rate = k[A]^x[B]^y$.From observation $1$ and $2$,$[B]$ is constant. When $[A]$ doubles,the rate increases from $2 \times

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(C) The rate law is given by $Rate = k[A]^x[B]^y$.From observation $1$ and $2$,$[B]$ is constant. When $[A]$ doubles,the rate increases from $2 \times 10^{-3}$ to $4 \times 10^{-3}$ (doubles). Thus,$2^x = 2$,which means $x = 1$.From observation $1$ and $3$,$[A]$ is constant. When $[B]$ doubles,the rate increases from $2 \times 10^{-3}$ to $8 \times 10^{-3}$ (quadruples). Thus,$2^y = 4$,which means $y = 2$.The overall order of reaction is $x + y = 1 + 2 = 3$.

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

Medium

What is the order of reaction for $A + B \to C$?

$Observation$ $[A] \ (mol \ L^{-1})$ $[B] \ (mol \ L^{-1})$ $Rate \ (mol \ L^{-1} \ sec^{-1})$

$1$ $0.1$ $0.1$ $2 \times 10^{-3}$

$2$ $0.2$ $0.1$ $4 \times 10^{-3}$

$3$ $0.1$ $0.2$ $8 \times 10^{-3}$

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

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Class 12 Questions

Class 12

Chemistry Questions

Chapter

Chemical Kinetics

Subtopic

Rate law , Rate constant , Order of Reaction and Molecularity

For a reaction scheme $A$ $\xrightarrow{k_1} B$ $\xrightarrow{k_2} C$,if the rate of formation of $B$ is set to be zero,then the concentration of $B$ is given by:

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For a reaction $X + Y \to Z$,the rate is given by $\text{rate} \propto [X]$. What are $(i)$ the molecularity and $(ii)$ the order of the reaction?

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........ of a reaction cannot be determined experimentally.

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For the reaction $A + B \rightarrow \text{Product}$,the rate law is given by $\text{Rate} = K[A]^1[B]^2$. Which of the following statements is incorrect?

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The data for the reaction $A + B \to C$ is given below:

$Exp$ $[A]_0$ $[B]_0$ Initial Rate

$1$ $0.012$ $0.035$ $0.10$

$2$ $0.024$ $0.035$ $0.80$

$3$ $0.012$ $0.070$ $0.10$

$4$ $0.024$ $0.070$ $0.80$

Determine the rate law for the reaction.

$Exp$	$[A]_0$	$[B]_0$	Initial Rate
$1$	$0.012$	$0.035$	$0.10$
$2$	$0.024$	$0.035$	$0.80$
$3$	$0.012$	$0.070$	$0.10$
$4$	$0.024$	$0.070$	$0.80$

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$Observation$	$[A] \ (mol \ L^{-1})$	$[B] \ (mol \ L^{-1})$	$Rate \ (mol \ L^{-1} \ sec^{-1})$
$1$	$0.1$	$0.1$	$2 \times 10^{-3}$
$2$	$0.2$	$0.1$	$4 \times 10^{-3}$
$3$	$0.1$	$0.2$	$8 \times 10^{-3}$

What is the order of reaction for $A + B \to C$? $Observation$ $[A] \ (mol \ L^{-1})$ $[B] \ (mol \ L^{-1})$ $Rate \ (mol \ L^{-1} \ sec^{-1})$ $1$ $0.1$ $0.1$ $2 \times 10^{-3}$ $2$ $0.2$ $0.1$ $4 \times 10^{-3}$ $3$ $0.1$ $0.2$ $8 \times 10^{-3}$

Similar Questions

For a reaction scheme $A$ $\xrightarrow{k_1} B$ $\xrightarrow{k_2} C$,if the rate of formation of $B$ is set to be zero,then the concentration of $B$ is given by:

For a reaction $X + Y \to Z$,the rate is given by $\text{rate} \propto [X]$. What are $(i)$ the molecularity and $(ii)$ the order of the reaction?

........ of a reaction cannot be determined experimentally.

For the reaction $A + B \rightarrow \text{Product}$,the rate law is given by $\text{Rate} = K[A]^1[B]^2$. Which of the following statements is incorrect?

The data for the reaction $A + B \to C$ is given below: $Exp$ $[A]_0$ $[B]_0$ Initial Rate $1$ $0.012$ $0.035$ $0.10$ $2$ $0.024$ $0.035$ $0.80$ $3$ $0.012$ $0.070$ $0.10$ $4$ $0.024$ $0.070$ $0.80$ Determine the rate law for the reaction.

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What is the order of reaction for $A + B \to C$?

$Observation$ $[A] \ (mol \ L^{-1})$ $[B] \ (mol \ L^{-1})$ $Rate \ (mol \ L^{-1} \ sec^{-1})$

$1$ $0.1$ $0.1$ $2 \times 10^{-3}$

$2$ $0.2$ $0.1$ $4 \times 10^{-3}$

$3$ $0.1$ $0.2$ $8 \times 10^{-3}$

The data for the reaction $A + B \to C$ is given below:

$Exp$ $[A]_0$ $[B]_0$ Initial Rate

$1$ $0.012$ $0.035$ $0.10$

$2$ $0.024$ $0.035$ $0.80$

$3$ $0.012$ $0.070$ $0.10$

$4$ $0.024$ $0.070$ $0.80$

Determine the rate law for the reaction.