What is the entropy change (in J K⁻¹ mol⁻¹) when one mole of ice is converted into water at 0 ºC? (The enthalpy change for the conversion of ice to liquid water is 6.0 kJ mol⁻¹ at 0 ºC)
20.13
2.013
2.198
21.98
For a reversible phase transition at constant temperature and pressure, the entropy change (\Delta S) is given by the ratio of the enthalpy change (\Delta H) to the temperature (T) in Kelvin. Given: Enthalpy change, \Delta H = 6.0 kJ mol⁻¹ = 6000 J mol⁻¹ Temperature, T = 0 ºC = 273 K
Using the formula: \Delta S = \Delta H / T \Delta S = 6000 J mol⁻¹ / 273 K \Delta S = 21.978 J K⁻¹ mol⁻¹ ≈ 21.98 J K⁻¹ mol⁻¹
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