(A) The given reaction is $2A + B_{2} \rightarrow 2AB$.Since it is an elementary reaction,the rate law is given by $r_{1} = k[A]^{2}[B_{2}]$.When the

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(A) The given reaction is $2A + B_{2} \rightarrow 2AB$.Since it is an elementary reaction,the rate law is given by $r_{1} = k[A]^{2}[B_{2}]$.When the volume of the reaction vessel is reduced by a factor of $3$,the concentration of each reactant increases by a factor of $3$ (since $C = n/V$).Let the new concentrations be $[A]' = 3[A]$ and $[B_{2}]' = 3[B_{2}]$.The new rate $r_{2}$ is $r_{2} = k(3[A])^{2}(3[B_{2}])$.$r_{2} = k \cdot 9[A]^{2} \cdot 3[B_{2}] = 27 \cdot k[A]^{2}[B_{2}] = 27 \cdot r_{1}$.Thus,the rate of reaction increases by a factor of $27$.

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

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The reaction $2A + B_{2} \rightarrow 2AB$ is an elementary reaction. For a certain quantity of reactants,if the volume of the reaction vessel is reduced by a factor of $3,$ the rate of the reaction increases by a factor of $.....$. (Round off to the Nearest Integer).

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A
$27$
B
$37$
C
$47$
D
$57$

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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The rate law of the reaction $A + 2B \to \text{Product}$ is given by $\frac{d[B]}{dt} = k[B^2]$. If $A$ is taken in excess,the order of the reaction will be

Medium

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The reaction $2A + B_{2} \rightarrow 2AB$ is an elementary reaction. For a certain quantity of reactants,if the volume of the reaction vessel is reduced by a factor of $3,$ the rate of the reaction increases by a factor of $.....$. (Round off to the Nearest Integer).

Similar Questions

The rate law of the reaction $A + 2B \to \text{Product}$ is given by $\frac{d[B]}{dt} = k[B^2]$. If $A$ is taken in excess,the order of the reaction will be

The hypothetical reaction : $2A + B \to C + D$ is catalyzed by $E$ as indicated in the possible mechanism below -Step-$1$ : $A + E \rightleftharpoons AE$ (fast)Step-$2$ : $AE + A \to A_2 + E$ (slow)Step-$3$ : $A_2 + B \to C + D$ (fast)What rate law best agrees with this mechanism?

For a gaseous reaction $2A + B \rightarrow C + D$,the rate of reaction is given by $Rate = K[A][B]$. If the volume of the container is reduced to $1/4$ of its original volume,what will be the ratio of the new rate to the original rate?

For the decomposition reaction $2NH_3(g) \rightarrow N_2(g) + 3H_2(g)$,if the rate constant $k = 2.6 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$,calculate the rate of formation of $N_2$ and $H_2$.

Identify the rate law expression for the reaction $2 NO_{(g)} + Cl_{2(g)} \rightarrow 2 NOCl_{(g)}$ if the reaction is second order in $NO$ and first order in $Cl_2$.

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The hypothetical reaction : $2A + B \to C + D$ is catalyzed by $E$ as indicated in the possible mechanism below -
Step-$1$ : $A + E \rightleftharpoons AE$ (fast)
Step-$2$ : $AE + A \to A_2 + E$ (slow)
Step-$3$ : $A_2 + B \to C + D$ (fast)
What rate law best agrees with this mechanism?