At 298 K the esterification of acetic acid and ethanol proceeds according to…

CHEMISTRY · Multi-part · A Level · Chemistry · Chemical equilibria (Le Chatelier’s principle and Kc) · Chemical equilibria (Le Chatelier’s principle and Kc)

Problem

At 298 K the esterification of acetic acid and ethanol proceeds according to CH3COOH(l)+C2H5OH(l)⇌CH3COOC2H5(l)+H2O(l)\mathrm{CH_3COOH(l)} + \mathrm{C_2H_5OH(l)} \rightleftharpoons \mathrm{CH_3COOC_2H_5(l)} + \mathrm{H_2O(l)} with Kc=3.2K_c = 3.2. A calorimetric investigation of the forward reaction under standard conditions gives ΔH∘=−1.84 kJ mol−1\Delta H^{\circ} = -1.84\,\text{kJ mol}^{-1}. Assume R=8.314 J mol−1K−1R = 8.314\,\text{J mol}^{-1}\text{K}^{-1} and that ΔH∘\Delta H^{\circ} is temperature-independent between 298 K and 310 K. (a) Predict whether KcK_c at 310 K will be greater than, less than, or equal to 3.2. Explain your reasoning. (b) Calculate the numerical value of KcK_c at 310 K. (c) A reaction mixture is prepared at 310 K by combining 1.0 mol CH3COOH\mathrm{CH_3COOH} and 1.0 mol C2H5OH\mathrm{C_2H_5OH} in a total volume of 1.00 L with no initial products present. Define a single algebraic variable and set up (but do not solve) the expressions needed to determine the equilibrium concentrations of all species. (d) Describe an experimental measurement that would allow you to verify the predicted shift in equilibrium position when the temperature is raised from 298 K to 310 K.

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