Medium
What is a pseudo first order reaction? Give an example of a pseudo first order reaction.
(N/A) pseudo first order reaction is a reaction that is actually of a higher order (usually second order) but behaves as a first order reaction under certain experimental conditions,such as when one reactant is present in a large excess.
Example: The acid-catalyzed hydrolysis of ethyl acetate $(CH_3COOC_2H_5 + H_2O \xrightarrow{H^+} CH_3COOH + C_2H_5OH)$.
In this reaction,the concentration of water is in such a large excess that it remains effectively constant throughout the reaction. Therefore,the rate law becomes $Rate = k[CH_3COOC_2H_5][H_2O] \approx k'[CH_3COOC_2H_5]$,where $k' = k[H_2O]$.
Example: The acid-catalyzed hydrolysis of ethyl acetate $(CH_3COOC_2H_5 + H_2O \xrightarrow{H^+} CH_3COOH + C_2H_5OH)$.
In this reaction,the concentration of water is in such a large excess that it remains effectively constant throughout the reaction. Therefore,the rate law becomes $Rate = k[CH_3COOC_2H_5][H_2O] \approx k'[CH_3COOC_2H_5]$,where $k' = k[H_2O]$.
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Similar Questions
Identify the correct statement regarding the order of reaction from the following.
The data for the reaction $A + B \to C$ is given below. The rate law corresponding to the above data is:
$Exp.$ $[A]_0$ $[B]_0$ Initial rate $(1)$ $0.012$ $0.035$ $0.10$ $(2)$ $0.024$ $0.070$ $0.80$ $(3)$ $0.024$ $0.035$ $0.10$ $(4)$ $0.012$ $0.070$ $0.80$
| $Exp.$ | $[A]_0$ | $[B]_0$ | Initial rate |
|---|---|---|---|
| $(1)$ | $0.012$ | $0.035$ | $0.10$ |
| $(2)$ | $0.024$ | $0.070$ | $0.80$ |
| $(3)$ | $0.024$ | $0.035$ | $0.10$ |
| $(4)$ | $0.012$ | $0.070$ | $0.80$ |
MediumAIPMT 1994
View SolutionThe reaction $2NO + O_2 \rightarrow 2NO_2$ is an example of which order of reaction?
Easy
View SolutionThe rate constant for a second order reaction is $8 \times 10^{-5} \ M^{-1} \ min^{-1}$. How long will it take a $1 \ M$ solution to be reduced to $0.5 \ M$?
Medium
View SolutionFor the reaction ${H_{2(g)} + I_{2(g)} \to 2HI_{(g)}}$,the possible mechanism is given below:
$I_2 \underset{k_{-1}}{\stackrel{k_1}{\rightleftharpoons}} 2 I$ (fast step)
${2I + H_2 \xrightarrow{K_2} 2HI}$ (slow step)
Determine the rate law for the reaction.
$I_2 \underset{k_{-1}}{\stackrel{k_1}{\rightleftharpoons}} 2 I$ (fast step)
${2I + H_2 \xrightarrow{K_2} 2HI}$ (slow step)
Determine the rate law for the reaction.
Medium
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