The melting point of a certain metal is 400 K and its molar enthalpy of fusion is 9.6 kJ mol ⁻¹ . The entropy of fusion of the metal is _______ J K ⁻¹ mol ⁻¹ . (Nearest Integer)

Step-by-step solution

At the melting point, the solid and liquid phases are in equilibrium, which implies G = 0 . Using the thermodynamic relation G = H - T S , we get: S = H T Given data: H = 9.6 kJ mol ⁻¹ = 9600 J mol ⁻¹ T = 400 K S = 9600 400 = 24 J K ⁻¹ mol ⁻¹ Answer: 24