(B) The rate law is expressed as $r = k[A]^x[B]^y$.From the data:$0.045 = k(0.05)^x(0.05)^y$ ...... $(1)$$0.090 = k(0.10)^x(0.05)^y$ ...... $(2)$$0.72

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(B) The rate law is expressed as $r = k[A]^x[B]^y$.From the data:$0.045 = k(0.05)^x(0.05)^y$ ...... $(1)$$0.090 = k(0.10)^x(0.05)^y$ ...... $(2)$$0.72 = k(0.20)^x(0.10)^y$ ...... $(3)$Dividing $(2)$ by $(1)$:$\frac{0.090}{0.045} = \left( \frac{0.10}{0.05} \right)^x$ $\Rightarrow 2 = 2^x$ $\Rightarrow x = 1$.Dividing $(3)$ by $(2)$:$\frac{0.72}{0.090} = \left( \frac{0.20}{0.10} \right)^x \left( \frac{0.10}{0.05} \right)^y$$8 = (2)^1 \times (2)^y$$8 = 2 \times 2^y$ $\Rightarrow 4 = 2^y$ $\Rightarrow y = 2$.Thus,the rate law is $r = k[A][B]^2$.

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

Difficult

For the reaction $2A + B \to C$,the values of initial rate at different reactant concentrations are given in the table below: The rate law for the reaction is

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

$0.05$ $0.05$ $0.045$

$0.10$ $0.05$ $0.090$

$0.20$ $0.10$ $0.72$

JEE MAIN 2019 All JEE MAIN

A
Rate $= k[A]^2[B]^2$
B
Rate $= k[A][B]^2$
C
Rate $= k[A][B]$
D
Rate $= k[A]^2[B]$

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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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JEE MAIN 2019 Paper All JEE MAIN years →

For the first order decomposition reaction of $N_2O_5$,it is found that -
$(a)$ $2N_2O_5 \rightarrow 4NO_{2(g)} + O_{2(g)}$ ; $-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$
$(b)$ $N_2O_5 \rightarrow 2NO_{2(g)} + 1/2 O_{2(g)}$ ; $-\frac{d[N_2O_5]}{dt} = k'[N_2O_5]$
Which of the following is true?

Medium

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For a reaction $A + B \to \text{Products}$,the rate law is: $\text{Rate} = k[A][B]^{3/2}$. Can the reaction be an elementary reaction? Explain.

Easy

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The reaction $2X + Y \to X_2Y$ follows the mechanism given below:
$2X \rightleftharpoons X_2$ (Fast)
$X_2 + Y \to X_2Y$ (Slow)
Determine the order of the reaction.

Medium

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$A$ complex reaction takes place in $2$ steps:
$(I)$ $NO_{2(g)} + F_{2(g)} \rightarrow NO_2F_{(g)} + F_{(g)}$ (slow)
$(II)$ $F_{(g)} + NO_{2(g)} \rightarrow NO_2F_{(g)}$ (fast)
Identify the reaction intermediate.

EasyMHT CET 2022

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Select the rate law that corresponds to the data shown for the following reaction $A + B \to C$

$Expt. \ No.$ $[A]$ $[B]$ $Initial \ Rate$

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

$2$ $0.024$ $0.070$ $0.80$

$3$ $0.024$ $0.035$ $0.10$

$4$ $0.012$ $0.070$ $0.80$

$Expt. \ No.$	$[A]$	$[B]$	$Initial \ Rate$
$1$	$0.012$	$0.035$	$0.10$
$2$	$0.024$	$0.070$	$0.80$
$3$	$0.024$	$0.035$	$0.10$
$4$	$0.012$	$0.070$	$0.80$

DifficultAIIMS 2012

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$[A] \ (mol \ L^{-1})$	$[B] \ (mol \ L^{-1})$	Initial Rate $(mol \ L^{-1} \ s^{-1})$
$0.05$	$0.05$	$0.045$
$0.10$	$0.05$	$0.090$
$0.20$	$0.10$	$0.72$

Similar Questions

For the first order decomposition reaction of $N_2O_5$,it is found that -$(a)$ $2N_2O_5 \rightarrow 4NO_{2(g)} + O_{2(g)}$ ; $-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$$(b)$ $N_2O_5 \rightarrow 2NO_{2(g)} + 1/2 O_{2(g)}$ ; $-\frac{d[N_2O_5]}{dt} = k'[N_2O_5]$Which of the following is true?

For a reaction $A + B \to \text{Products}$,the rate law is: $\text{Rate} = k[A][B]^{3/2}$. Can the reaction be an elementary reaction? Explain.

The reaction $2X + Y \to X_2Y$ follows the mechanism given below:$2X \rightleftharpoons X_2$ (Fast)$X_2 + Y \to X_2Y$ (Slow)Determine the order of the reaction.

$A$ complex reaction takes place in $2$ steps:$(I)$ $NO_{2(g)} + F_{2(g)} \rightarrow NO_2F_{(g)} + F_{(g)}$ (slow)$(II)$ $F_{(g)} + NO_{2(g)} \rightarrow NO_2F_{(g)}$ (fast)Identify the reaction intermediate.

Select the rate law that corresponds to the data shown for the following reaction $A + B \to C$ $Expt. \ No.$ $[A]$ $[B]$ $Initial \ Rate$ $1$ $0.012$ $0.035$ $0.10$ $2$ $0.024$ $0.070$ $0.80$ $3$ $0.024$ $0.035$ $0.10$ $4$ $0.012$ $0.070$ $0.80$

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For the first order decomposition reaction of $N_2O_5$,it is found that -
$(a)$ $2N_2O_5 \rightarrow 4NO_{2(g)} + O_{2(g)}$ ; $-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$
$(b)$ $N_2O_5 \rightarrow 2NO_{2(g)} + 1/2 O_{2(g)}$ ; $-\frac{d[N_2O_5]}{dt} = k'[N_2O_5]$
Which of the following is true?

The reaction $2X + Y \to X_2Y$ follows the mechanism given below:
$2X \rightleftharpoons X_2$ (Fast)
$X_2 + Y \to X_2Y$ (Slow)
Determine the order of the reaction.

$A$ complex reaction takes place in $2$ steps:
$(I)$ $NO_{2(g)} + F_{2(g)} \rightarrow NO_2F_{(g)} + F_{(g)}$ (slow)
$(II)$ $F_{(g)} + NO_{2(g)} \rightarrow NO_2F_{(g)}$ (fast)
Identify the reaction intermediate.

Select the rate law that corresponds to the data shown for the following reaction $A + B \to C$

$Expt. \ No.$ $[A]$ $[B]$ $Initial \ Rate$

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

$2$ $0.024$ $0.070$ $0.80$

$3$ $0.024$ $0.035$ $0.10$

$4$ $0.012$ $0.070$ $0.80$