$\overline{){\mathbf{\u2206}}{{\mathbf{S}}}_{{\mathbf{univ}}}{\mathbf{=}}{\mathbf{\u2206}}{{\mathbf{S}}}_{{\mathbf{sys}}}{\mathbf{+}}{\mathbf{\u2206}}{{\mathbf{S}}}_{{\mathbf{surr}}}}$

**Step 1. **Determine ΔS_{sys}:

$\mathbf{\u2206}{\mathbf{H}}_{\mathbf{vap}}\mathbf{=}\frac{\mathbf{38}\mathbf{.}\mathbf{7}\mathbf{}\overline{)\mathbf{kJ}}}{\mathbf{mol}}\mathbf{\times}\frac{{\mathbf{10}}^{\mathbf{3}}\mathbf{}\mathbf{J}}{\mathbf{1}\mathbf{}\overline{)\mathbf{kJ}}}\mathbf{=}$**38700 J/mol**

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

The enthalpy of vaporization of ethanol is 38.7 kJ/mol at its boiling point (78°C). Determine ΔS_{sys}, ΔS_{surr}, and ΔS_{univ} when 1.00 mole of ethanol is vaporized at 78°C and 1.00 atm.

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