Problem: The reaction of chloroethane with water in the gas phase to produce ethanol and hydrogen chloride has ΔH° = +26.6 kJ mol -1 and ΔS° = +4.81 J K-1 mol-1 at 25°C. (d) In aqueous solution the equilibrium constant is very much larger than the one you just calculated. How can you account for this fact?

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Problem Details

The reaction of chloroethane with water in the gas phase to produce ethanol and hydrogen chloride has ΔH° = +26.6 kJ mol -1 and ΔS° = +4.81 J K-1 mol-1 at 25°C. (d) In aqueous solution the equilibrium constant is very much larger than the one you just calculated. How can you account for this fact?

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