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Calculate the entropy change in melting 1 mole of ice at $273 \mathrm{~K}, \Delta \mathrm{H}_{\mathrm{f}}^{\mathrm{o}}=6.025 \mathrm{~kJ} /$ mole-
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$22.1 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}$
$\Delta \mathrm{S}_{\mathrm{f}}=\frac{\Delta \mathrm{H}_{\mathrm{f}}}{\mathrm{T}}=\frac{6025 \mathrm{~J} \mathrm{~mol}^{-1}}{273 \mathrm{~K}}=22.1 \mathrm{JK}^{-1}$ $\mathrm{mol}^{-1}$
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