he molar enthalpy of fusion of ice at 273.15 K and one atm is ΔfusHm (H2O)=6.01 kJ mol-1 , and the molar entropy of fusion under the same conditions is ΔfusSm (H2O)=22.0 J K-1 mol-1 . Show that (a) ΔfusGm (H2O)=0 at 273.15 K and one atm, (b) ΔfusG,m (H2O) < 0 when the temperature is greater than 273.15 K, and (c) ΔfusGm (H2O) > 0 when the temperature is less than 273.15 K.

he molar enthalpy of fusion of ice at 273.15 K and one atm is ΔfusHm (H2O)=6.01 kJ mol-1 , and the molar entropy of fusion under the same conditions is ΔfusSm (H2O)=22.0 J K-1 mol-1 . Show that (a) ΔfusGm (H2O)=0 at 273.15 K and one atm, (b) ΔfusG,m (H2O) < 0 when the temperature is greater than 273.15 K, and (c) ΔfusGm (H2O) > 0 when the temperature is less than 273.15 K.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section: Chapter Questions

Problem 89QRT: Determine the standard Gibbs free energy change, rG, for the reactions of liquid methanol, of CO(g),...

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