For a phase change, h = -44 kj/mol and so = -0.12 kj/(k•mol). what are g and the spontaneity of the phase change at 350 k?

ΔG = - 2.0 kJ/mol and the reaction is spontaneous.

Explanation:

∵ ΔG = ΔH - TΔS,

ΔH = - 44.0 kJ/mol, T = 350.0 K, ΔS = - 0.12 kJ/K.mol.

∴ ΔG = ΔH - TΔS = (- 44.0 kJ/mol) - (350.0 K)(- 0.12 kJ/K.mol) = - 2.0 kJ/mol.

The sign of ΔG assigns the spontaneity of the reaction:

∵ ΔG has a negative value, so the reaction is spontaneous.

ΔG = - 2.0 kJ/mol and the reaction is spontaneous.