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Entropy Change in Phase Transition
Appears in
Concepts tested here
- Entropy of fusion 2
All Questions
2003 AIPMT 1 question
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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 $0^\circ C$)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$^{-1}$
2000 AIPMT 1 question
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At $27^\circ C$ latent heat of fusion of a compound is 2930 J/mol. Entropy change is :For fusion at the melting point: $\Delta S = \dfrac{\Delta H_{fus}}{T}$
$T = 27 + 273 = 300$ K
$\Delta S = \dfrac{2930}{300} = 9.77$ J/mol K