(D) The rate of the reaction is determined by the slowest step,which is Step-$II$: $\text{Rate} = K_2[X][B]$.From the fast equilibrium step (Step-$I$)

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(D) The rate of the reaction is determined by the slowest step,which is Step-$II$: $\text{Rate} = K_2[X][B]$.From the fast equilibrium step (Step-$I$): $K_{eq} = \frac{[X]}{[A]^2}$,so $[X] = K_{eq}[A]^2$.Substituting the value of $[X]$ into the rate expression for the slow step:$\text{Rate} = K_2(K_{eq}[A]^2)[B] = K[A]^2[B]$,where $K = K_2 \times K_{eq}$.

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

Medium

$A$ chemical reaction proceeds through the following steps:
Step-$I$: $2A \rightleftharpoons X$ (fast)
Step-$II$: $X + B \rightarrow Y$ (slow)
Step-$III$: $Y + B \rightarrow \text{Product}$ (fast)
The rate law for the overall reaction is:

A
Rate $= K[A]^2$
B
Rate $= K[B]^2$
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

For a particular reaction,the rate expression is given as $r = k[A][B]^{0.5}$. If the volume of the vessel is reduced to one-fourth of the initial volume,the rate of reaction would

Medium

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Identify the order of the following reaction:
$2H_2O_{2(aq)} \longrightarrow 2H_2O_{(l)} + O_{2(g)}$

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If the rate expression for a chemical reaction is given by $\text{Rate} = k[A]^m[B]^n$,what is the order of the reaction?

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For the hypothetical reaction $2X + G \to Q + 2M$,the rate expression is $\frac{d[Q]}{dt} = k[X]^2$. Which of the following is the most likely mechanism?

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For the reaction $3 \, A_{(g)} \xrightarrow{K} B_{(g)} + C_{(g)}$,$K$ is $10^{-14} \, L/mol \cdot min$. If $[A] = 0.5 \, M$,then the value of $-\frac{d[A]}{dt}$ (in $M/sec$) is:

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$A$ chemical reaction proceeds through the following steps:Step-$I$: $2A \rightleftharpoons X$ (fast)Step-$II$: $X + B \rightarrow Y$ (slow)Step-$III$: $Y + B \rightarrow \text{Product}$ (fast)The rate law for the overall reaction is:

Similar Questions

For a particular reaction,the rate expression is given as $r = k[A][B]^{0.5}$. If the volume of the vessel is reduced to one-fourth of the initial volume,the rate of reaction would

Identify the order of the following reaction: $2H_2O_{2(aq)} \longrightarrow 2H_2O_{(l)} + O_{2(g)}$

If the rate expression for a chemical reaction is given by $\text{Rate} = k[A]^m[B]^n$,what is the order of the reaction?

For the hypothetical reaction $2X + G \to Q + 2M$,the rate expression is $\frac{d[Q]}{dt} = k[X]^2$. Which of the following is the most likely mechanism?

For the reaction $3 \, A_{(g)} \xrightarrow{K} B_{(g)} + C_{(g)}$,$K$ is $10^{-14} \, L/mol \cdot min$. If $[A] = 0.5 \, M$,then the value of $-\frac{d[A]}{dt}$ (in $M/sec$) is:

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$A$ chemical reaction proceeds through the following steps:
Step-$I$: $2A \rightleftharpoons X$ (fast)
Step-$II$: $X + B \rightarrow Y$ (slow)
Step-$III$: $Y + B \rightarrow \text{Product}$ (fast)
The rate law for the overall reaction is:

Identify the order of the following reaction:
$2H_2O_{2(aq)} \longrightarrow 2H_2O_{(l)} + O_{2(g)}$