(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 $(mol \ L^{-1} \ s^{-1})$

$0.05$ $0.05$ $0.045$

$0.10$ $0.05$ $0.090$

$0.20$ $0.10$ $0.72$

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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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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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What is the order of reaction if the unit of the rate constant is $s^{-1}$?

EasyMHT CET 2022

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Consider the following reaction: $A \longrightarrow \text{Products}$. This reaction is completed in $100 \ min$. The rate constant of this reaction at $t_1 = 10 \ min$ is $10^{-2} \ min^{-1}$. What is the rate constant (in $min^{-1}$) at $t_2 = 20 \ min$?

MediumAP EAMCET 2022

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For a second-order reaction where both reactants have the same initial concentration,it takes $500 \ s$ for the reaction to be $20\%$ complete. How many seconds will it take for the reaction to be $80\%$ complete (in $s$)?

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If the concentration of reactant $B$ is doubled,the rate of the reaction between reactants $A$ and $B$ becomes $1/4$ of the initial rate. The order of the reaction with respect to reactant $B$ is ......

Medium

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For a reaction $A + B \longrightarrow P$,the following data are provided. The rate constant for this reaction in standard units is:
Entry $[A]$ in $M$ $[B]$ in $M$ Initial rate $(M/s)$
$1$ $0.02$ $0.02$ $2 \times 10^{-2}$
$2$ $0.02$ $0.04$ $4 \times 10^{-2}$
$3$ $0.04$ $0.04$ $8 \times 10^{-2}$

Entry	$[A]$ in $M$	$[B]$ in $M$	Initial rate $(M/s)$
$1$	$0.02$	$0.02$	$2 \times 10^{-2}$
$2$	$0.02$	$0.04$	$4 \times 10^{-2}$
$3$	$0.04$	$0.04$	$8 \times 10^{-2}$

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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

What is the order of reaction if the unit of the rate constant is $s^{-1}$?

Consider the following reaction: $A \longrightarrow \text{Products}$. This reaction is completed in $100 \ min$. The rate constant of this reaction at $t_1 = 10 \ min$ is $10^{-2} \ min^{-1}$. What is the rate constant (in $min^{-1}$) at $t_2 = 20 \ min$?

For a second-order reaction where both reactants have the same initial concentration,it takes $500 \ s$ for the reaction to be $20\%$ complete. How many seconds will it take for the reaction to be $80\%$ complete (in $s$)?

If the concentration of reactant $B$ is doubled,the rate of the reaction between reactants $A$ and $B$ becomes $1/4$ of the initial rate. The order of the reaction with respect to reactant $B$ is ......

For a reaction $A + B \longrightarrow P$,the following data are provided. The rate constant for this reaction in standard units is:Entry$[A]$ in $M$$[B]$ in $M$Initial rate $(M/s)$$1$$0.02$$0.02$$2 \times 10^{-2}$$2$$0.02$$0.04$$4 \times 10^{-2}$$3$$0.04$$0.04$$8 \times 10^{-2}$

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For a reaction $A + B \longrightarrow P$,the following data are provided. The rate constant for this reaction in standard units is:
Entry $[A]$ in $M$ $[B]$ in $M$ Initial rate $(M/s)$
$1$ $0.02$ $0.02$ $2 \times 10^{-2}$
$2$ $0.02$ $0.04$ $4 \times 10^{-2}$
$3$ $0.04$ $0.04$ $8 \times 10^{-2}$