Problem: A (l) → A (g)                       ΔH°vap = -42.55 kJ/mol Calculate the entropy of vaporization, ΔSvap, for A(/) at 250°C given that the boiling point of A is 76.53°C, and the molar heat capacity of A() is 116.59 J/(mol K). Assume that the molar heat capacity of A(g) is 6.7% of that of A(l). Calculate the standard Gibbs free energy of vaporization, ΔG°vap, at 25.0°C. Determine the equilibrium constant, K, for the vaporization at 179.0°C. 

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A (l) → A (g)                       ΔH°vap = -42.55 kJ/mol 

Calculate the entropy of vaporization, ΔSvap, for A(/) at 250°C given that the boiling point of A is 76.53°C, and the molar heat capacity of A() is 116.59 J/(mol K). Assume that the molar heat capacity of A(g) is 6.7% of that of A(l). 

Calculate the standard Gibbs free energy of vaporization, ΔG°vap, at 25.0°C. 

Determine the equilibrium constant, K, for the vaporization at 179.0°C. 


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