First consider the melting of gallium:

Ga(s)  →  Ga(l)

a.    Consider the following entropy data for gallium.

S°(liquid)	59.25  J/mol*K
S°(solid)	40.83  J/mol*K

Calculate the entropy change for the system. Show labelled  work!

b.    The ΔH^o_fusion for gallium is +5.58 kJ/mol.  Calculate the entropy change for the surroundings, assuming T=25 ^oC.  Show labelled  work!

c.     Calculate the total entropy change, ΔS_universe, for melting (assuming T=25 ^oC)

d.    From a thermodynamics perspective then, based on your value for ΔS_universe , why is gallium a solid at room temperature?  What could be done to make melting more favorable? (to make the products more probable?)  Explain your reasoning.