a.)Calculate the enthalpy, entropy, and gibbs free energy changes when 10g of supercooled liquid silver solidifies isothermally at 1133K and 1atm. Show that the second law is obeyed.
b.)Another 10 gram sample of liquid Ag is placed in an adiabatic container at 1133K and 1atm and solid Ag nucleates. Calculate the entropy change for the ensuing process. For Ag: Tmp=1234K deltaH=11,090J/mole
Cp(solid)=21.30 +8.54x10^-3 T+1.51x10^5 T^-2 J/mole K
Cp(liquid)=30.50 J/mole K