(B) The rate law for the reaction is given by: $r = k[A]^1[B]^2$. If the concentration of $B$ is increased $3$ times,the new concentration becomes $[B

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(B) The rate law for the reaction is given by: $r = k[A]^1[B]^2$. If the concentration of $B$ is increased $3$ times,the new concentration becomes $[B'] = 3[B]$. The new rate is $r_{new} = k[A][3B]^2$. $r_{new} = k[A] \times 9[B]^2 = 9 \times (k[A][B]^2)$. $r_{new} = 9r$. Therefore,the reaction rate increases $9$ times.

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

Medium

$A$ reaction is first order with respect to $A$ and second order with respect to $B$. What is the effect on the reaction rate if the concentration of $B$ is increased $3$ times?

MHT CET 2021 All MHT CET

A
Rate increases $6$ times
B
Rate increases $9$ times
C
Rate increases $2$ times
D
Rate increases $3$ times

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Class 12 Questions

Class 12

Chemistry Questions

Chapter

Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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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 following are the rate constants of two different reactions. What is the overall order of reaction for each?
$(a)$ $2.418 \times 10^{-5} \ hr^{-1}$
$(b)$ $7.1 \times 10^{-4} \ atm \ s^{-1}$

Medium

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The given plots represent the variation of the concentration of a reactant $R$ with time for two different reactions $(i)$ and $(ii).$ The respective orders of the reactions are

DifficultJEE MAIN 2019

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$A$ study of chemical kinetics of the reaction $A + B \to$ Products,gave the following data at $25 \ ^oC$.

$Exp. \ No.$ $[A]$ $[B]$ $Rate$

$1.$ $1.0$ $0.15$ $4.2 \times 10^{-6}$

$2.$ $2.0$ $0.15$ $8.4 \times 10^{-6}$

$3.$ $1.0$ $0.20$ $5.6 \times 10^{-6}$

Find out the rate law.

Medium

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From the rate expression for the following reaction,determine its order of reaction and the dimensions of the rate constant.
$(i)$ $3 NO_{(g)} \rightarrow N_2O_{(g)}$ Rate $= k[NO]^2$

Medium

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$Exp. \ No.$	$[A]$	$[B]$	$Rate$
$1.$	$1.0$	$0.15$	$4.2 \times 10^{-6}$
$2.$	$2.0$	$0.15$	$8.4 \times 10^{-6}$
$3.$	$1.0$	$0.20$	$5.6 \times 10^{-6}$

$A$ reaction is first order with respect to $A$ and second order with respect to $B$. What is the effect on the reaction rate if the concentration of $B$ is increased $3$ times?

Similar Questions

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 following are the rate constants of two different reactions. What is the overall order of reaction for each?$(a)$ $2.418 \times 10^{-5} \ hr^{-1}$$(b)$ $7.1 \times 10^{-4} \ atm \ s^{-1}$

The given plots represent the variation of the concentration of a reactant $R$ with time for two different reactions $(i)$ and $(ii).$ The respective orders of the reactions are

$A$ study of chemical kinetics of the reaction $A + B \to$ Products,gave the following data at $25 \ ^oC$. $Exp. \ No.$ $[A]$ $[B]$ $Rate$ $1.$ $1.0$ $0.15$ $4.2 \times 10^{-6}$ $2.$ $2.0$ $0.15$ $8.4 \times 10^{-6}$ $3.$ $1.0$ $0.20$ $5.6 \times 10^{-6}$ Find out the rate law.

From the rate expression for the following reaction,determine its order of reaction and the dimensions of the rate constant.$(i)$ $3 NO_{(g)} \rightarrow N_2O_{(g)}$ Rate $= k[NO]^2$

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The following are the rate constants of two different reactions. What is the overall order of reaction for each?
$(a)$ $2.418 \times 10^{-5} \ hr^{-1}$
$(b)$ $7.1 \times 10^{-4} \ atm \ s^{-1}$

$A$ study of chemical kinetics of the reaction $A + B \to$ Products,gave the following data at $25 \ ^oC$.

$Exp. \ No.$ $[A]$ $[B]$ $Rate$

$1.$ $1.0$ $0.15$ $4.2 \times 10^{-6}$

$2.$ $2.0$ $0.15$ $8.4 \times 10^{-6}$

$3.$ $1.0$ $0.20$ $5.6 \times 10^{-6}$

Find out the rate law.

From the rate expression for the following reaction,determine its order of reaction and the dimensions of the rate constant.
$(i)$ $3 NO_{(g)} \rightarrow N_2O_{(g)}$ Rate $= k[NO]^2$