# 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.

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###### FREE Expert Solution

$\overline{){\mathbf{∆}}{{\mathbf{S}}}_{{\mathbf{univ}}}{\mathbf{=}}{\mathbf{∆}}{{\mathbf{S}}}_{{\mathbf{sys}}}{\mathbf{+}}{\mathbf{∆}}{{\mathbf{S}}}_{{\mathbf{surr}}}}$

Step 1Determine ΔSsys:

38700 J/mol

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

###### 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.