(C) Let the rate law be $Rate = k[A]^x[B]^y$. From experiments $2$ and $3$ (where $[B]$ is constant): $\frac{10}{1} = \frac{k(10)^x(1)^y}{k(1)^x(1)^y}

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First order with respect to $A$ and second order with respect to $B$

(C) Let the rate law be $Rate = k[A]^x[B]^y$. From experiments $2$ and $3$ (where $[B]$ is constant): $\frac{10}{1} = \frac{k(10)^x(1)^y}{k(1)^x(1)^y}$ $\Rightarrow 10 = 10^x$ $\Rightarrow x = 1$. From experiments $1$ and $2$ (where $[A]$ is constant): $\frac{100}{1} = \frac{k(1)^x(10)^y}{k(1)^x(1)^y}$ $\Rightarrow 100 = 10^y$ $\Rightarrow 10^2 = 10^y$ $\Rightarrow y = 2$. Thus,the order with respect to $A$ is $1$ and with respect to $B$ is $2$.

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

Easy

For the reaction $A + B \rightarrow C$,we have the following data:
Initial concentration of $A$ $(M)$ Initial concentration of $B$ $(M)$ Initial Rate $(M \cdot s^{-1})$
$1$ $10$ $100$
$1$ $1$ $1$
$10$ $1$ $10$

The order of the reaction with respect to $A$ and $B$ are:

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A
Not possible to tell with the given data
B
First order with respect to both $A$ and $B$
C
First order with respect to $A$ and second order with respect to $B$
D
Second order with respect to $A$ and first order with respect to $B$

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Class 12

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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Determine the order of reaction on the basis of following data for the reaction $A + B \to C$.
Exp. $[A]$ $[B]$ Rate of reaction $(mol \ L^{-1} \ s^{-1})$
$1$ $0.1$ $0.1$ $2 \times 10^{-3}$
$2$ $0.4$ $0.1$ $0.8 \times 10^{-2}$
$3$ $0.1$ $0.2$ $1.6 \times 10^{-2}$
(in $.5$)

Exp.	$[A]$	$[B]$	Rate of reaction $(mol \ L^{-1} \ s^{-1})$
$1$	$0.1$	$0.1$	$2 \times 10^{-3}$
$2$	$0.4$	$0.1$	$0.8 \times 10^{-2}$
$3$	$0.1$	$0.2$	$1.6 \times 10^{-2}$

Medium

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If the rate expression for a chemical reaction is given by $\text{Rate} = k[A]^m[B]^n$,what is the order of the reaction?

Medium

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For a reaction $A \rightarrow 2 B + C$ the half-lives are $100 \ s$ and $50 \ s$ when the concentration of reactant $A$ is $0.5 \ mol \ L^{-1}$ and $1.0 \ mol \ L^{-1}$ respectively. The order of the reaction is (Nearest Integer).

MediumJEE MAIN 2022

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$A$ chemical reaction proceeds through the following steps:
Step-$I$: $2A \rightleftharpoons X$ (fast)
Step-$II$: $X + B \rightarrow Y$ (slow)
Step-$III$: $Y + B \rightarrow \text{Product}$ (fast)
The rate law for the overall reaction is:

Medium

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Write the formula for the rate of reaction $R \to P$ for zero-order and first-order reactions.

Easy

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Initial concentration of $A$ $(M)$	Initial concentration of $B$ $(M)$	Initial Rate $(M \cdot s^{-1})$
$1$	$10$	$100$
$1$	$1$	$1$
$10$	$1$	$10$

For the reaction $A + B \rightarrow C$,we have the following data: Initial concentration of $A$ $(M)$Initial concentration of $B$ $(M)$Initial Rate $(M \cdot s^{-1})$$1$$10$$100$$1$$1$$1$$10$$1$$10$The order of the reaction with respect to $A$ and $B$ are:

Similar Questions

Determine the order of reaction on the basis of following data for the reaction $A + B \to C$.Exp.$[A]$$[B]$Rate of reaction $(mol \ L^{-1} \ s^{-1})$$1$$0.1$$0.1$$2 \times 10^{-3}$$2$$0.4$$0.1$$0.8 \times 10^{-2}$$3$$0.1$$0.2$$1.6 \times 10^{-2}$ (in $.5$)

If the rate expression for a chemical reaction is given by $\text{Rate} = k[A]^m[B]^n$,what is the order of the reaction?

For a reaction $A \rightarrow 2 B + C$ the half-lives are $100 \ s$ and $50 \ s$ when the concentration of reactant $A$ is $0.5 \ mol \ L^{-1}$ and $1.0 \ mol \ L^{-1}$ respectively. The order of the reaction is (Nearest Integer).

$A$ chemical reaction proceeds through the following steps:Step-$I$: $2A \rightleftharpoons X$ (fast)Step-$II$: $X + B \rightarrow Y$ (slow)Step-$III$: $Y + B \rightarrow \text{Product}$ (fast)The rate law for the overall reaction is:

Write the formula for the rate of reaction $R \to P$ for zero-order and first-order reactions.

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For the reaction $A + B \rightarrow C$,we have the following data:
Initial concentration of $A$ $(M)$ Initial concentration of $B$ $(M)$ Initial Rate $(M \cdot s^{-1})$
$1$ $10$ $100$
$1$ $1$ $1$
$10$ $1$ $10$

The order of the reaction with respect to $A$ and $B$ are:

Determine the order of reaction on the basis of following data for the reaction $A + B \to C$.
Exp. $[A]$ $[B]$ Rate of reaction $(mol \ L^{-1} \ s^{-1})$
$1$ $0.1$ $0.1$ $2 \times 10^{-3}$
$2$ $0.4$ $0.1$ $0.8 \times 10^{-2}$
$3$ $0.1$ $0.2$ $1.6 \times 10^{-2}$
(in $.5$)

$A$ chemical reaction proceeds through the following steps:
Step-$I$: $2A \rightleftharpoons X$ (fast)
Step-$II$: $X + B \rightarrow Y$ (slow)
Step-$III$: $Y + B \rightarrow \text{Product}$ (fast)
The rate law for the overall reaction is: