(D) Let the rate law be $Rate = k[A]^x[B]^y$.From experiment $1$: $2 \times 10^{-3} = k(0.1)^x(0.1)^y$ $(i)$From experiment $2$: $8 \times 10^{-3} =

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(D) Let the rate law be $Rate = k[A]^x[B]^y$.From experiment $1$: $2 \times 10^{-3} = k(0.1)^x(0.1)^y$ $(i)$From experiment $2$: $8 \times 10^{-3} = k(0.4)^x(0.1)^y$ (ii)Dividing (ii) by $(i)$: $4 = (4)^x \implies x = 1$.From experiment $3$: $1.6 \times 10^{-2} = k(0.1)^x(0.2)^y$ (iii)Dividing (iii) by $(i)$: $8 = (2)^y \implies y = 3$.Total order of reaction = $x + y = 1 + 3 = 4$.

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

Medium

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 $(mol \ L^{-1} \ s^{-1})$
$1$	$0.1$	$0.1$	$2 \times 10^{-3}$
$2$	$0.4$	$0.1$	$0.8 \times 10^{-2}$
$3$	$0.1$	$0.2$	$1.6 \times 10^{-2}$

A
$1$
B
$2$
C
$3$
D
$4$

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Class 12 Questions

Class 12

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

The rate constant of a reaction is $1.388 \times 10^{-3} \ mol^{-2} \ L^{2} \ s^{-1}$. The order of the reaction is:

Medium

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For a chemical reaction $A + B \rightarrow \text{Product}$,the order is $1$ with respect to $A$ and $B$.
Rate $(mol \ L^{-1} \ s^{-1})$ $[A]$ $(mol \ L^{-1})$ $[B]$ $(mol \ L^{-1})$
$0.10$ $20$ $0.5$
$0.40$ $x$ $0.5$
$0.80$ $40$ $y$

What is the value of $x$ and $y$?

Rate $(mol \ L^{-1} \ s^{-1})$	$[A]$ $(mol \ L^{-1})$	$[B]$ $(mol \ L^{-1})$
$0.10$	$20$	$0.5$
$0.40$	$x$	$0.5$
$0.80$	$40$	$y$

MediumJEE MAIN 2023

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If $a$ is the initial concentration of the reactant,the half-life period of the reaction of $n^{th}$ order is inversely proportional to

Medium

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The rate for the reaction $A + B \rightarrow \text{product}$ is $1.8 \times 10^{-2} \ mol \ dm^{-3} \ s^{-1}$. Calculate the rate constant if the reaction is second order in $A$ and first order in $B$,given $[A] = 0.2 \ M$ and $[B] = 0.1 \ M$.

MediumMHT CET 2023

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Write the differential rate expression for the following reactions and determine their order of reaction:
$1. CHCl_3 + Cl_2 \rightarrow CCl_4 + HCl$
$2. CH_3COOC_2H_5 + H_2O \rightarrow CH_3COOH + C_2H_5OH$

Medium

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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 $.5$)

Similar Questions

The rate constant of a reaction is $1.388 \times 10^{-3} \ mol^{-2} \ L^{2} \ s^{-1}$. The order of the reaction is:

For a chemical reaction $A + B \rightarrow \text{Product}$,the order is $1$ with respect to $A$ and $B$.Rate $(mol \ L^{-1} \ s^{-1})$$[A]$ $(mol \ L^{-1})$$[B]$ $(mol \ L^{-1})$$0.10$$20$$0.5$$0.40$$x$$0.5$$0.80$$40$$y$What is the value of $x$ and $y$?

If $a$ is the initial concentration of the reactant,the half-life period of the reaction of $n^{th}$ order is inversely proportional to

The rate for the reaction $A + B \rightarrow \text{product}$ is $1.8 \times 10^{-2} \ mol \ dm^{-3} \ s^{-1}$. Calculate the rate constant if the reaction is second order in $A$ and first order in $B$,given $[A] = 0.2 \ M$ and $[B] = 0.1 \ M$.

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$

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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 $.5$)

For a chemical reaction $A + B \rightarrow \text{Product}$,the order is $1$ with respect to $A$ and $B$.
Rate $(mol \ L^{-1} \ s^{-1})$ $[A]$ $(mol \ L^{-1})$ $[B]$ $(mol \ L^{-1})$
$0.10$ $20$ $0.5$
$0.40$ $x$ $0.5$
$0.80$ $40$ $y$

What is the value of $x$ and $y$?

Write the differential rate expression for the following reactions and determine their order of reaction:
$1. CHCl_3 + Cl_2 \rightarrow CCl_4 + HCl$
$2. CH_3COOC_2H_5 + H_2O \rightarrow CH_3COOH + C_2H_5OH$