(B) The acid-catalyzed hydrolysis of an ester is a pseudo-first-order reaction where the rate of reaction is directly proportional to the concentratio

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Acid $A$ is a stronger acid than acid $B$.

(B) The acid-catalyzed hydrolysis of an ester is a pseudo-first-order reaction where the rate of reaction is directly proportional to the concentration of $H^+$ ions.Since the reaction is catalyzed by $H^+$ ions,the rate constant $K$ is directly proportional to the concentration of $H^+$ ions produced by the acid.Therefore,$K \propto [H^+]$.Given $K_A > K_B$,it implies that $[H^+]_A > [H^+]_B$.Since a stronger acid dissociates more to provide a higher concentration of $H^+$ ions,acid $A$ must be a stronger acid than acid $B$.

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

Medium

The hydrolysis of an ester is catalyzed by dilute acids $A$ and $B$. The rate constants for the two processes are $K_A$ and $K_B$ respectively. If $K_A > K_B$,which of the following statements is correct?

A
Acid $A$ is a weaker acid than acid $B$.
B
Acid $A$ is a stronger acid than acid $B$.
C
Both acids have the same acidic strength.
D
The catalytic effect of both acids is due to their conjugate bases.

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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 reaction,$A + B \longrightarrow$ Product; the rate law is given by $r = k[A]^2[B]^{1/2}$. What is the order of the reaction?

Medium

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The rate law equation for a reaction between $A$,$B$ and $C$ is $r = k[A][B][C]^2$. What will be the new rate of reaction if the concentration of both $A$ and $B$ are doubled (in $r$)?

MediumMHT CET 2021

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For a reaction,$A + 2B \rightarrow$ Products,when the concentration of $B$ alone is increased,the half-life remains the same. If the concentration of $A$ alone is doubled,the rate remains the same. The unit of the rate constant for the reaction is:

MediumKCET 2021

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For a reaction $A + B \rightarrow \text{Product}$,the order with respect to $A$ is $2$ and with respect to $B$ is $3$. If the concentration of both is doubled,by how much will the rate increase?

Easy

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By giving three examples,explain whether the exponents of the concentration terms in a rate law are the same as their stoichiometric coefficients in the balanced chemical reaction.

Difficult

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The hydrolysis of an ester is catalyzed by dilute acids $A$ and $B$. The rate constants for the two processes are $K_A$ and $K_B$ respectively. If $K_A > K_B$,which of the following statements is correct?

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For a reaction,$A + B \longrightarrow$ Product; the rate law is given by $r = k[A]^2[B]^{1/2}$. What is the order of the reaction?

The rate law equation for a reaction between $A$,$B$ and $C$ is $r = k[A][B][C]^2$. What will be the new rate of reaction if the concentration of both $A$ and $B$ are doubled (in $r$)?

For a reaction,$A + 2B \rightarrow$ Products,when the concentration of $B$ alone is increased,the half-life remains the same. If the concentration of $A$ alone is doubled,the rate remains the same. The unit of the rate constant for the reaction is:

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