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  4. What is the entropy change (in JK1 mol1) when one mole of ice is converted into water at 0°C ?(The enthalpy change for the conversion of ice to liquid water is 6.0 kJ mol-1 at 0°C)

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Q. What is the entropy change (in $JK^1\, mol^1$) 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 $0^{\circ}C$)

AIPMTAIPMT 2003Thermodynamics

Solution:

$ \Delta H = 6.0 \,kJ \,mol^{-1} = 6 \times 10^3 \,J \, mol^{-1}$

$T = 0^\circ C = 273\, K$

$\Delta S = \frac{\Delta H}{T}$ (For a reversible process)

$\Delta S = \frac{6 \times 10^3 \, J \, mol^{-1}}{273 \, K} = 21.98 \, JK^{-1} \, mol^{-1}$