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

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(A) The rate law for the reaction is given by: $Rate = k[A]^1[B]^2$. If the concentration of $B$ is increased two times,the new concentration becomes $[B'] = 2[B]$. The new rate $Rate'$ will be: $Rate' = k[A]^1[2B]^2 = 4 \times k[A]^1[B]^2$. Therefore,the rate of reaction increases by $4-$Times. Hence,the correct option is $A$.

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

Easy

$A$ reaction is first order in terms of $A$ and second order in terms of $B$. What will be the rate of reaction,if the concentration of $B$ is increased two times?

GUJCET 2023 All GUJCET

A
$4-$Times
B
$2-$Times
C
$8-$Times
D
$16-$Times

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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$A$ reaction is first order in terms of $A$ and second order in terms of $B$. What will be the rate of reaction,if the concentration of $B$ is increased two times?

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For a reaction,$AB_5 \to AB + 4B$,the rate can be expressed in the following ways:$-\frac{d[AB_5]}{dt} = K[AB_5]$ ; $\frac{d[B]}{dt} = K_1[AB_5]$What is the correct relation between $K$ and $K_1$?

At what concentration of the reactant (in $M$) are the rate constants for first-order,second-order,and third-order reactions equal?

Higher order $(> 3)$ reactions are rare due to:

For an elementary reaction,$2A + B \to C + D$,the molecularity is:

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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For a reaction,$AB_5 \to AB + 4B$,the rate can be expressed in the following ways:
$-\frac{d[AB_5]}{dt} = K[AB_5]$ ; $\frac{d[B]}{dt} = K_1[AB_5]$
What is the correct relation between $K$ and $K_1$?

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 $= k[NO]^2$