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Question

Chemistry Question on Thermodynamics

What is the entropy change (in JK1 mol1JK^1\, mol^1) when one mole of ice is converted into water at 0∘C0^{\circ}C ?(The enthalpy change for the conversion of ice to liquid water is 6.0 kJ mol−16.0 \, kJ \, mol^{-1} at 0∘C0^{\circ}C)

A

21.98

B

20.13

C

2.013

D

2.198

Answer

21.98

Explanation

Solution

ΔH=6.0 kJ mol−1=6×103 J mol−1 \Delta H = 6.0 \,kJ \,mol^{-1} = 6 \times 10^3 \,J \, mol^{-1}
T=0∘C=273 KT = 0^\circ C = 273\, K
ΔS=ΔHT\Delta S = \frac{\Delta H}{T} (For a reversible process)

ΔS=6×103 J mol−1273 K=21.98 JK−1 mol−1\Delta S = \frac{6 \times 10^3 \, J \, mol^{-1}}{273 \, K} = 21.98 \, JK^{-1} \, mol^{-1}