Neco Model Questions Vol1 2019 Chemistry Question 38

Esterification of two different carboxylic acids with ethanol is carried out under standard conditions (298 K). The standard Gibbs free energies of formation (kJ mol⁻¹) are: \(\Delta G_f^{\circ}(\text{CH}_3\text{COOH}) = -389\), \(\Delta G_f^{\circ}(\text{C}_2\text{H}_5\text{COOH}) = -384\), \(\Delta G_f^{\circ}(\text{C}_2\text{H}_5\text{OH}) = -174\), \(\Delta G_f^{\circ}(\text{CH}_3\text{COOCH}_2\text{CH}_3) = -447\), \(\Delta G_f^{\circ}(\text{C}_2\text{H}_5\text{COOCH}_2\text{CH}_3) = -452\), and \(\Delta G_f^{\circ}(\text{H}_2\text{O}) = -237\).\ (i) Calculate \(\Delta G^{\circ}\) for each esterification reaction (acid + ethanol ⇌ ester + water).\ (ii) Determine the equilibrium constant \(K = e^{-\Delta G^{\circ}/RT}\) for each reaction at 298 K (use \(R = 8.314\) J mol⁻¹ K⁻¹).\ (iii) Assuming 1 mol of each acid and 1 mol of ethanol are present initially, which ester will have the higher equilibrium concentration?