Q1. [6 points] The hydrolysis of esters yields carboxylic acid and alcohol. A typical reaction is the saponification reaction between ethyl acetate \( \left(\mathrm{CH}_{3} \mathrm{COOC}_{2} \mathrm{H}_{5}\right) \) and sodium hydroxide \( \mathrm{NaOH} \). a) Write a balanced chemical equation for the reaction. b) What is the overall order of the reaction? c) Predict the rate law in rate constant \( k \) and concentration. d) Given that rate constant \( \mathrm{K} \) is \( 4000 \mathrm{M}^{-1} \mathrm{~s}^{-1} \) at \( 650 \mathrm{~K} \), and \( 1700 \mathrm{M}^{-1} \mathrm{~s}^{-1} \) at \( 625 \mathrm{~K} \) Using the Arrhenius equation estimate the \( E_{a} \) and the pre-exponential factor A.
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The ester methyl acetate, $\mathrm{CH}_{3} \mathrm{COOCH}_{3}$, reacts with base to break one of the $\mathrm{C}-\mathrm{O}$ bonds. <smiles>CC(=O)OCC(O)C(C)O</smiles> <smiles>CC(=O)OCCOCCC(=O)O</smiles> The rate law is rate $=k\left[\mathrm{CH}_{3} \mathrm{COOCH}_{3}\right]\left[\mathrm{OH}^{-}\right]$ where $$ k=0.14 \mathrm{~L} \mathrm{~mol}^{-1} \mathrm{~s}^{-1} \text {at } 25^{\circ} \mathrm{C} $$ (a) Calculate the initial rate at which the methyl acetate is converted to products when both reactants, $\mathrm{CH}_{3} \mathrm{COOCH}_{3}$ and $\mathrm{OH}^{-}$, have a concentration of $0.025 \mathrm{M}$. (b) Calculate the rate at which methyl alcohol, $\mathrm{CH}_{3} \mathrm{OH}$, initially appears in the solution.
The rate constants for the forward and backward reactions of hydrolysis of ester are $1.1 \times 10^{-2}$ and $1.5 \times 10^{-3}$ mol $\mathrm{L}^{-1} \mathrm{~s}^{-1}$ respectively. The equilibrium constant of the reaction, $\mathrm{CH}_{3} \mathrm{COOC}_{2} \mathrm{H}_{5}+\mathrm{H}^{+} \rightleftharpoons \mathrm{CH}_{3} \mathrm{COOH}+$ $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$ is (a) $6.53$ (b) $7.34$ (c) $7.75$ (d) $8.33$
The rate constants for the forward and backward reactions of hydrolysis of ester are $1.1 \times 10^{-2}$ and $1.5 \times$ $10^{-3} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}$ respectively. The equilibrium constant of the reaction, $\mathrm{CH}_{3} \mathrm{COOC}_{2} \mathrm{H}_{5}+\mathrm{H}^{+} \rightleftharpoons \mathrm{CH}_{3} \mathrm{COOH}+$ $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}$ is: (a) $6.53$ (b) $7.34$ (c) $7.75$ (d) $8.33$
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