A laboratory synthesis generates ethyl acetate according to the balanced equation…

CHEMISTRY · Multi-part · CBSE · Chemistry · Thermodynamics · Thermodynamics

Problem

A laboratory synthesis generates ethyl acetate according to the balanced equation

\text{CH}_3\text{COOH}\,(l) + \text{C}_2\text{H}_5\text{OH}\,(l) \rightarrow \text{CH}_3\text{COOC}_2\text{H}_5\,(l) + \text{H}_2\text{O}\,(l)

Selected absolute molar entropies at 298 K are listed.

Substance	$S^\circ$ (J mol $^{-1}$ K $^{-1}$ )
$\text{CH}_3\text{COOH}\,(l)$	159
$\text{C}_2\text{H}_5\text{OH}\,(l)$	161
$\text{CH}_3\text{COOC}_2\text{H}_5\,(l)$	274
$\text{H}_2\text{O}\,(l)$	70

(a) Calculate the standard entropy change,

\Delta S^\circ_{298}

, for the synthesis of ethyl acetate. Include appropriate units. (b) Benzoic acid,

\text{C}_6\text{H}_5\text{COOH}\,(s)

, can react with ethanol in an analogous esterification. Predict, with justification, whether the sign of

\Delta S^\circ

for that reaction is likely to be more positive, less positive, or approximately the same as the value you calculated in part (a). (c) Explain how the magnitude and sign of

\Delta S^\circ

for an esterification influence industrial decisions about operating temperature when maximizing product yield.

Related theory

Browse the problem library