(A) The rate of a reaction is determined by the slowest step in the mechanism. The rate law for the slow step is $R = k_3[A][B]$. Since $B$ is an inte

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(A) The rate of a reaction is determined by the slowest step in the mechanism. The rate law for the slow step is $R = k_3[A][B]$. Since $B$ is an intermediate formed in the fast equilibrium step $A \underset{k_2}{\stackrel{k_1}{\rightleftharpoons}} B$,we have the equilibrium constant $K_{eq} = \frac{[B]}{[A]} = \frac{k_1}{k_2}$. This gives $[B] = \frac{k_1}{k_2}[A]$. Substituting this into the rate expression: $R = k_3[A](\frac{k_1}{k_2}[A]) = \frac{k_3 k_1}{k_2}[A]^2$. Thus,the rate is proportional to $[A]^2$.

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

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For a hypothetical reaction,$A \rightarrow C$. The mechanism is: $A \underset{k_2}{\stackrel{k_1}{\rightleftharpoons}} B$ (Fast),$A + B \xrightarrow{k_3} C$ (Slow). The rate law for this reaction is:

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A
$\propto [A]^2$
B
$\propto [A][B]$
C
$\propto [A]^2[B]^2$
D
$\propto [A]^2[B]$

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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

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For the reaction $A + B \to C$,it is found that doubling the concentration of $A$ increases the rate by $4$ times,and doubling the concentration of $B$ doubles the reaction rate. What is the overall order of the reaction?

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In the reaction $X \to Y$,if the concentration of reactant $X$ is increased by $1.5$ times,the rate of reaction increases by $1.837$ times. Determine the order of the reaction with respect to $X$.

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Write the unit of the rate constant for the following reactions:
$1.$ $\frac{1}{2}$ order
$2.$ $\frac{3}{2}$ order

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Ozone decomposes into oxygen as follows:
$O_3 \rightleftharpoons O_2 + [O]$
$O_3 + [O] \to 2O_2$ (slow)
Determine the order of the reaction $2O_3 \to 3O_2$.

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For the reaction $A + B \rightarrow C$, we have the following data:
Initial concentration of $A$ $(M)$ Initial concentration of $B$ $(M)$ Initial Rate $(M \cdot s^{-1})$
$1$ $10$ $100$
$1$ $1$ $1$
$10$ $1$ $10$

The order of the reaction with respect to $A$ and $B$ are:

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Initial concentration of $A$ $(M)$	Initial concentration of $B$ $(M)$	Initial Rate $(M \cdot s^{-1})$
$1$	$10$	$100$
$1$	$1$	$1$
$10$	$1$	$10$

For a hypothetical reaction,$A \rightarrow C$. The mechanism is: $A \underset{k_2}{\stackrel{k_1}{\rightleftharpoons}} B$ (Fast),$A + B \xrightarrow{k_3} C$ (Slow). The rate law for this reaction is:

Similar Questions

For the reaction $A + B \to C$,it is found that doubling the concentration of $A$ increases the rate by $4$ times,and doubling the concentration of $B$ doubles the reaction rate. What is the overall order of the reaction?

In the reaction $X \to Y$,if the concentration of reactant $X$ is increased by $1.5$ times,the rate of reaction increases by $1.837$ times. Determine the order of the reaction with respect to $X$.

Write the unit of the rate constant for the following reactions:$1.$ $\frac{1}{2}$ order$2.$ $\frac{3}{2}$ order

Ozone decomposes into oxygen as follows:$O_3 \rightleftharpoons O_2 + [O]$$O_3 + [O] \to 2O_2$ (slow)Determine the order of the reaction $2O_3 \to 3O_2$.

For the reaction $A + B \rightarrow C$, we have the following data: Initial concentration of $A$ $(M)$Initial concentration of $B$ $(M)$Initial Rate $(M \cdot s^{-1})$$1$$10$$100$$1$$1$$1$$10$$1$$10$The order of the reaction with respect to $A$ and $B$ are:

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Write the unit of the rate constant for the following reactions:
$1.$ $\frac{1}{2}$ order
$2.$ $\frac{3}{2}$ order

Ozone decomposes into oxygen as follows:
$O_3 \rightleftharpoons O_2 + [O]$
$O_3 + [O] \to 2O_2$ (slow)
Determine the order of the reaction $2O_3 \to 3O_2$.

For the reaction $A + B \rightarrow C$, we have the following data:
Initial concentration of $A$ $(M)$ Initial concentration of $B$ $(M)$ Initial Rate $(M \cdot s^{-1})$
$1$ $10$ $100$
$1$ $1$ $1$
$10$ $1$ $10$

The order of the reaction with respect to $A$ and $B$ are: