Consider the condensation of 0.50 mol of ethanol vapor at 38.3 o C and 1 bar. Ca

Question

Consider the condensation of 0.50 mol of ethanol vapor at 38.3oC and 1 bar.

Calculate the heat, the entropy change for the system, the entropy change for the surroundings and the total entropy change for the universe. What does the sign of DRSo Universe tell you?

The boiling point of ethanol under a pressure of 1 bar is 78.3oC and at this temperature DvapHo = 39.3 kJ.mol%u20101. The standard molar heat capacities at constant pressure for ethanol liquid and vapor are 111.46 and 65.44 J/K.mol, respectively.

Explanation / Answer

heat = 0.5 x(39.3 + 111.46 x 40) = 2248.85 kJ

entropy change of system = 0.5 x 39.3/351.3 + 0.5 x 111.46 x 40/311.3 = 7.216 kJ/K

entropy change of surroundings = -7.216 kJ/k

entopy change of unvierse = 0

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