Write the equation for a pseudo first order reaction. Write the rate law and the rate constant.
(N/A) pseudo first order reaction can be represented by the hydrolysis of an ester (e.g.,ethyl acetate) in the presence of an excess of water:
$CH_3COOC_2H_5 + H_2O \xrightarrow{H^+} CH_3COOH + C_2H_5OH$
Rate law:
$Rate = k[CH_3COOC_2H_5][H_2O]$
Since water is in large excess,its concentration remains practically constant throughout the reaction. Thus,we define $k' = k[H_2O]$,leading to:
$Rate = k'[CH_3COOC_2H_5]$
Where $k'$ is the pseudo first order rate constant.
$CH_3COOC_2H_5 + H_2O \xrightarrow{H^+} CH_3COOH + C_2H_5OH$
Rate law:
$Rate = k[CH_3COOC_2H_5][H_2O]$
Since water is in large excess,its concentration remains practically constant throughout the reaction. Thus,we define $k' = k[H_2O]$,leading to:
$Rate = k'[CH_3COOC_2H_5]$
Where $k'$ is the pseudo first order rate constant.
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$A + B \rightarrow \text{product}$. The rate of this reaction is given by $v = K[A]^2[B]^0$. What is the change in the rate of reaction when the concentration of $A$ is doubled and the concentration of $B$ is doubled?
For the reaction, $A + B \rightarrow P$, the rate law is $\text{rate} = k[A][B]^2$. The rate of reaction is $0.25 \text{ Ms}^{-1}$ when $[A] = 1 \text{ M}$ and $[B] = 0.2 \text{ M}$ at $25^\circ \text{C}$. Calculate the rate constant $k$ of the reaction at the same temperature.
DifficultMHT CET 2026
View SolutionThe three experimental data for determining the differential rate of reaction $Cl_{2(g)} + 2NO_{(g)} \rightarrow 2NOCl_{(g)}$ at $310 \ K$ temperature are provided. $(a)$ Derive the differential rate of reaction. $(b)$ Calculate the order of reaction. $(c)$ Calculate the value of the rate constant.
Medium
View SolutionThe bromination of acetone that occurs in acid solution is represented by this equation.
$CH_3COCH_{3(aq)} + Br_{2(aq)} \rightarrow CH_3COCH_2Br_{(aq)} + H^+_{(aq)} + Br^-_{(aq)}$
These kinetic data were obtained for given reaction concentrations.
Initial concentrations,$M$
$[CH_3COCH_3]$ $[Br_2]$ $[H^+]$ $0.30$ $0.05$ $0.05$ $0.30$ $0.10$ $0.05$ $0.30$ $0.10$ $0.10$ $0.40$ $0.05$ $0.20$
Initial rate,disappearance of $Br_2, M s^{-1}$
$5.7 \times 10^{-5}, 5.7 \times 10^{-5}, 1.14 \times 10^{-4}, 3.04 \times 10^{-4}$
Based on these data,the rate equation is
$CH_3COCH_{3(aq)} + Br_{2(aq)} \rightarrow CH_3COCH_2Br_{(aq)} + H^+_{(aq)} + Br^-_{(aq)}$
These kinetic data were obtained for given reaction concentrations.
Initial concentrations,$M$
| $[CH_3COCH_3]$ | $[Br_2]$ | $[H^+]$ |
| $0.30$ | $0.05$ | $0.05$ |
| $0.30$ | $0.10$ | $0.05$ |
| $0.30$ | $0.10$ | $0.10$ |
| $0.40$ | $0.05$ | $0.20$ |
Initial rate,disappearance of $Br_2, M s^{-1}$
$5.7 \times 10^{-5}, 5.7 \times 10^{-5}, 1.14 \times 10^{-4}, 3.04 \times 10^{-4}$
Based on these data,the rate equation is
For the non-stoichiometric reaction $2A + B \to C + D$,the following kinetic data were obtained in three separate experiments,all at $298 \ K$.
Initial Conc. $(A)$ Initial Conc. $(B)$ Initial rate of formation of $C \ (mol \ L^{-1} \ s^{-1})$ $0.1 \ M$ $0.1 \ M$ $1.2 \times 10^{-3}$ $0.1 \ M$ $0.2 \ M$ $1.2 \times 10^{-3}$ $0.2 \ M$ $0.1 \ M$ $2.4 \times 10^{-3}$
For the reaction,the rate of formation of $C$ will be:
| Initial Conc. $(A)$ | Initial Conc. $(B)$ | Initial rate of formation of $C \ (mol \ L^{-1} \ s^{-1})$ |
| $0.1 \ M$ | $0.1 \ M$ | $1.2 \times 10^{-3}$ |
| $0.1 \ M$ | $0.2 \ M$ | $1.2 \times 10^{-3}$ |
| $0.2 \ M$ | $0.1 \ M$ | $2.4 \times 10^{-3}$ |
For the reaction,the rate of formation of $C$ will be:
Medium
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