What is the entropy change (in J K⁻¹ mol⁻¹) when one mole of ice is converted into water at 0°C? (The enthalpy change for the conversion of ice to liquid water is 6.0 kJ mol⁻¹ at 0°C)

Question

Accepted Answer

21.98. The entropy change (ΔS) is calculated using the formula ΔS = ΔH/T. Here, ΔH = 6.0 kJ mol⁻¹ = 6000 J mol⁻¹ and T = 0°C = 273 K. Substituting, ΔS = 6000/273 ≈ 21.98 J K⁻¹ mol⁻¹.

What is the entropy change (in J K⁻¹ mol⁻¹) when one mole of ice is converted into water at 0°C? (The enthalpy change for the conversion of ice to liquid water is 6.0 kJ mol⁻¹ at 0°C)

Solution

Related NEET Chemistry questions