Calculate the change in entropy for fusion of 1 mole of ice. The melting point of ice is 273 K and molar enthalpy of fusion for ice = 6.0 kJ mole−1
A
△Sf =21.97 JK−1mol−1
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B
△Sf =21.87 JK−1mol−1
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C
△Sf =21.78 JK−1mol−1
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D
△Sf =21.79 JK−1mol−1
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Solution
The correct option is A△Sf =21.97 JK−1mol−1 For entropy change of fusion we know that the entropy change is given by, ΔSf=ΔHfT
Given values are, ΔHf=6×103Jmol−1; T=273K
Therefore ΔSf=(6×103273) ΔSf =21.97 JK−1mol−1