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The temperature at which the following process reaches equilibrium at 1.0 atm is the normal melting point for phosphoric acid. Use the following data to calculate the temperature, in K, at equilibrium. H3PO4(s) =H3PO4(1) H3PO4(s) AHp = -1288.5 kJ/mol S = 107.3 J/K*mol H3PO4(1) AHt = -1271.8 kJ/mol S = 141.5 J/K*mol Given the following data C3H3(g) AGF = -33.2 kJ/mol CO2(g) AGF = -379.8 kJ/mol H2O(1) AGP = -242.9 kJ/mol Calculate the Gibb's free energy, AGrxn, in kJ/mol, for the reaction below. C3H2(g) + 5 O2(g) + 3 CO2(g) + 4H2O(1)