The vaporization of compound A is described by the following chemical equation. A(I)A(g)Hyap(75.17C)=35.93kJ/mol Calculate the entropy of vaporization, Svap, for A(1) at 25.0C given that the boiling point of A is 75.17C, and the molar heat capacity of A(l) is 117.63J/(molK). Assume that the molar heat capacity of A(g) is 56.5% of that of A(l). Calculate the standard enthalpy of vaporization, Hvap, for A(l) at 25.0C. Hvap= Calculate the standard Gibbs free energy of vaporization, Gvapap, at 25.0C. Gvaps= Determine the equilibrium constant, K, for the vaporization at 173.0C. K Determine the temperature at which the vaporization of A(1) becomes spontaneous. Assume that the enthalpy and entropy of vaporization change very little with temperature. T= Is the vaporization of A(1) spontancous at temperatures greater than or less than T ? Calculate the standard enthalpy of vaporization, Hvap, for A(I) at 25.0C. Hvap J/mol Calculate the standard Gibbs free energy of vaporization, Gvapb, at 25.0C. GV Jetermine the equilibrium constant, K, for the vaporization at 173.0C. K= Determine the temperature at which the vaporization of A(1) becomes spontaneous. Assume that the enthalpy and entropy of vaporization change very little with temperature. T= Is the vaporization of A(1) spontaneous at temperatures greater than or less than T ? less than T greater than T