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?
- AAcid $A$ is a weaker acid than acid $B$.
- BAcid $A$ is a stronger acid than acid $B$.
- CBoth acids have the same acidic strength.
- DThe catalytic effect of both acids is due to their conjugate bases.
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Similar Questions
State whether the following sentences are true $(T)$ or false $(F)$:
$(a)$ There is more than one reactant in a pseudo first order reaction.
$(b)$ In a pseudo first order reaction,the concentration of both reactants is the same.
$(c)$ In a pseudo first order reaction,the concentration of one reactant is very high.
$(a)$ There is more than one reactant in a pseudo first order reaction.
$(b)$ In a pseudo first order reaction,the concentration of both reactants is the same.
$(c)$ In a pseudo first order reaction,the concentration of one reactant is very high.
Medium
View SolutionThe half-life period of a gaseous reactant undergoing thermal decomposition was measured for various initial pressures $P_0$ as follows:
$P_0 \text{ (mmHg)}$ $250$ $300$ $t_{1/2} \text{ (minutes)}$ $135$ $112.5$
The order of reaction is -
| $P_0 \text{ (mmHg)}$ | $250$ | $300$ |
| $t_{1/2} \text{ (minutes)}$ | $135$ | $112.5$ |
The order of reaction is -
Medium
View SolutionWhat is the molecularity and order of the following reaction if the rate law is $\text{rate} = k[O_3][O]$ respectively?
$O_{3(g)} + O_{(g)} \longrightarrow 2O_{2(g)}$
$O_{3(g)} + O_{(g)} \longrightarrow 2O_{2(g)}$
The rate of reaction between two reactants $A$ and $B$ decreases by a factor of $4$ if the concentration of reactant $B$ is doubled. The order of this reaction with respect to reactant $B$ is
DifficultAIPMT 2005
View SolutionThe reaction between $X$ and $Y$ is first order with respect to $X$ and zero order with respect to $Y$.
$Experiment$ $[X] / (mol \ L^{-1})$ $[Y] / (mol \ L^{-1})$ $\text{Initial rate} / (mol \ L^{-1} \ min^{-1})$ $I$ $0.1$ $0.1$ $2 \times 10^{-3}$ $II$ $0.2$ $0.2$ $4 \times 10^{-3}$ $III$ $0.4$ $0.4$ $M \times 10^{-3}$ $IV$ $0.1$ $0.2$ $2 \times 10^{-3}$
Examine the data of the table and calculate the ratio of the numerical value of $M$ to $0.2$.
| $Experiment$ | $[X] / (mol \ L^{-1})$ | $[Y] / (mol \ L^{-1})$ | $\text{Initial rate} / (mol \ L^{-1} \ min^{-1})$ |
| $I$ | $0.1$ | $0.1$ | $2 \times 10^{-3}$ |
| $II$ | $0.2$ | $0.2$ | $4 \times 10^{-3}$ |
| $III$ | $0.4$ | $0.4$ | $M \times 10^{-3}$ |
| $IV$ | $0.1$ | $0.2$ | $2 \times 10^{-3}$ |
Examine the data of the table and calculate the ratio of the numerical value of $M$ to $0.2$.
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