(A) The initial rate is given by $R = k[A]^n[B]^m$. When the concentration of $A$ is doubled $([A]' = 2[A])$ and the concentration of $B$ is halved $(

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(A) The initial rate is given by $R = k[A]^n[B]^m$. When the concentration of $A$ is doubled $([A]' = 2[A])$ and the concentration of $B$ is halved $([B]' = \frac{B}{2})$,the new rate $R'$ is: $R' = k[2A]^n[\frac{B}{2}]^m$ $R' = k \cdot 2^n [A]^n \cdot 2^{-m} [B]^m$ $R' = k[A]^n[B]^m \cdot 2^{n - m}$ $R' = R \cdot 2^{n - m}$ Therefore,the ratio of the new rate to the earlier rate is: $\frac{R'}{R} = 2^{n - m}$.

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

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The rate law for a reaction between the substances $A$ and $B$ is given by,$rate = k[A]^n[B]^m$. On doubling the concentration of $A$ and halving the concentration of $B$,the ratio of the new rate to the earlier rate of the reaction will be as

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A
$2^{(n - m)}$
B
$2^{(m - n)}$
C
$2^{(n + m)}$
D
$2^{(m + n)}$

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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 $2A + B \rightarrow \text{Product}$,the following mechanism is given. What is the order of the reaction?
$2A \rightleftharpoons A_2$ (fast)
$A_2 + B \rightarrow P$ (slow)

Medium

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The rate law for the reaction below is given by the expression $Rate = k[A][B]$.
$A + B \to \text{Product}$
If the concentration of $B$ is increased from $0.1 \ M$ to $0.3 \ M$,keeping the concentration of $A$ constant at $0.1 \ M$,the rate constant $(k)$ will be:

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The hydrolysis of ethyl acetate is a reaction of $.........$ order.
$CH_3COOEt + H_2O \xrightarrow{H^{+}} CH_3COOH + EtOH$

Medium

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The rate of a reaction depends upon the

Easy

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The mechanism of the decomposition of nitramide $(NH_2NO_2)$ in aqueous solution is given below:
$NH_2NO_2(aq) + OH^-(aq) \to NHNO_2^-(aq) + H_2O(l)$
$NHNO_2^-(aq) \to N_2O(aq) + OH^-(aq)$
Identify the catalyst for this reaction.

Medium

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The rate law for a reaction between the substances $A$ and $B$ is given by,$rate = k[A]^n[B]^m$. On doubling the concentration of $A$ and halving the concentration of $B$,the ratio of the new rate to the earlier rate of the reaction will be as

Similar Questions

For the reaction $2A + B \rightarrow \text{Product}$,the following mechanism is given. What is the order of the reaction? $2A \rightleftharpoons A_2$ (fast)$A_2 + B \rightarrow P$ (slow)

The rate law for the reaction below is given by the expression $Rate = k[A][B]$.$A + B \to \text{Product}$If the concentration of $B$ is increased from $0.1 \ M$ to $0.3 \ M$,keeping the concentration of $A$ constant at $0.1 \ M$,the rate constant $(k)$ will be:

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The mechanism of the decomposition of nitramide $(NH_2NO_2)$ in aqueous solution is given below:$NH_2NO_2(aq) + OH^-(aq) \to NHNO_2^-(aq) + H_2O(l)$$NHNO_2^-(aq) \to N_2O(aq) + OH^-(aq)$Identify the catalyst for this reaction.

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For the reaction $2A + B \rightarrow \text{Product}$,the following mechanism is given. What is the order of the reaction?
$2A \rightleftharpoons A_2$ (fast)
$A_2 + B \rightarrow P$ (slow)

The rate law for the reaction below is given by the expression $Rate = k[A][B]$.
$A + B \to \text{Product}$
If the concentration of $B$ is increased from $0.1 \ M$ to $0.3 \ M$,keeping the concentration of $A$ constant at $0.1 \ M$,the rate constant $(k)$ will be:

The hydrolysis of ethyl acetate is a reaction of $.........$ order.
$CH_3COOEt + H_2O \xrightarrow{H^{+}} CH_3COOH + EtOH$

The mechanism of the decomposition of nitramide $(NH_2NO_2)$ in aqueous solution is given below:
$NH_2NO_2(aq) + OH^-(aq) \to NHNO_2^-(aq) + H_2O(l)$
$NHNO_2^-(aq) \to N_2O(aq) + OH^-(aq)$
Identify the catalyst for this reaction.