First slide

Gibb's Helmholtz equation

Question

One mole of ice is converted in to water at 273K. The entropies of H₂O_(s) and H₂O_(l) are 38.20 and 60.01 J mole^-1K^-1 respectively. The enthalpy change for this conversion is

Moderate

A

595.4 J mol^-1
B

59.54 J mol^-1
C

320.6 J mol^-1
D

5954 J mol^-1

Solution

$\begin{array}{l} {H_2}{O_{(s)}} \to {H_2}{O_{(l)}}\\\\ \Delta {S_r} = \sum {S_{products}} - \sum {S_{reac\tan ts}}\\ \,\,\,\,\,\,\,\,\, = {S_{{H_2}{O_{(l)}}}} - {S_{{H_2}{O_{(s)}}}}\\ \,\,\,\,\,\,\,\, = \,60.01 - 38.20 = 21.81J/mole/K \end{array}$
$\Delta H=T\Delta S$ = 273 X 21.81 = 5954J

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