What is the entropy change (in J K⁻¹ mol⁻¹) when one mole of ice is converted into water at 0 ºC? (The enthalp

Question

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)

Accepted Answer

For a reversible phase transition at constant temperature and pressure, the entropy change (ΔS) is given by the ratio of the enthalpy change (ΔH) to the temperature (T) in Kelvin.
Given:
Enthalpy change, ΔH = 6.0 kJ mol⁻¹ = 6000 J mol⁻¹
Temperature, T = 0 ºC = 273 K

Using the formula:
ΔS = ΔH / T
ΔS = 6000 J mol⁻¹ / 273 K
ΔS = 21.978 J K⁻¹ mol⁻¹ ≈ 21.98 J K⁻¹ mol⁻¹

Step-by-Step Solution

Practice All CHEMISTRY Questions