Problem: The enthalpy of vaporization of ethanol is 38.7 kJ/mol at its boiling point (78°C). Determine ΔSsys, ΔSsurr, and ΔSuniv when 1.00 mole of ethanol is vaporized at 78°C and 1.00 atm.

FREE Expert Solution

Suniv=Ssys+Ssurr


Step 1Determine ΔSsys:

Hvap=38.7 kJmol×103 J1 kJ=38700 J/mol

T = °C + 273.15 = 78 + 273.15 = 351.15 K

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Problem Details

The enthalpy of vaporization of ethanol is 38.7 kJ/mol at its boiling point (78°C). Determine ΔSsys, ΔSsurr, and ΔSuniv when 1.00 mole of ethanol is vaporized at 78°C and 1.00 atm.

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