Gibbs free energy spontaneity 2

Chemistry Level pending

Ethanol’s enthalpy of vaporization is 38.7 38.7 kJ mol − 1 ^{-1} at its normal boiling point 78 78 °C. Calculate Δ G Δ G when 2.00 2.00 mol ethanol is vaporized reversibly at 78.0 78.0 °C and 1.0 1.0 atm.

Assume that the vapor is an ideal gas, and the volume of the liquid ethanol relative to the volume of its vapor is negligibly small.

0.00 kJ 0.00\text{ kJ} 35.80 kJ 35.80\text{ kJ} 38.70 kJ 38.70\text{ kJ} − 2.92 kJ -2.92\text{ kJ}

Krishna Singh by Krishna Singh , 22, India

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1 solution

Mayank Holmes
Jun 5, 2014

in a reversible process (^G) = 0

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