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What is the entropy change (in J K$^{-1}$ mol$^{-1}$) when one mole of ice is converted into water at $0^\circ C$ ? (The enthalpy change for the conversion of ice to liquid water is 6.0 kJ mol$^{-1}$ at $0^\circ C$)
A
20.13
B
2.013
C
2.198
D
21.98
Detailed Solution
Melting at the melting point is a reversible process at constant temperature, so $\Delta S = \dfrac{\Delta H_{fus}}{T}$.
$\Delta H_{fus} = 6.0$ kJ mol$^{-1}$ $= 6000$ J mol$^{-1}$, $T = 273$ K
$\Delta S = \dfrac{6000}{273} = 21.98$ J K$^{-1}$ mol$^{-1}$
$\Delta H_{fus} = 6.0$ kJ mol$^{-1}$ $= 6000$ J mol$^{-1}$, $T = 273$ K
$\Delta S = \dfrac{6000}{273} = 21.98$ J K$^{-1}$ mol$^{-1}$