The vaporization of compound AA is described by the following chemical equation. A(l)⟶A(g) Δ𝐻∘vap(77.77

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The vaporization of compound AA is described by the
following chemical equation.
A(l)⟶A(g)
Δ𝐻∘vap(77.77 °C)=45.15 kJ/mol
Calculate the entropy of vaporization, Δ𝑆vap, for A(l)
at 25.0°C given that the boiling point of A is
77.77 °C, and the molar heat capacity of A(l)
is 114.37 J/(mol⋅K). Assume that the molar heat
capacity of A(g) is 57.3% of that of A(l).
Δ𝑆vap= J⋅mol−1⋅K−1
Calculate the standard enthalpy of vaporization, Δ⁢Hvap∘,
for A(l) at 25.0 °C.
Δ𝐻∘vap= kJ/mol
Calculate the standard Gibbs free energy of
vaporization, Δ𝐺∘vap , at 25.0 °C .
Δ𝐺∘vap= kJ/mol
Determine the equilibrium constant, K, for the vaporization
at 195.0 °C.
K=
Determine the temperature at which the vaporization
of A(l) becomes spontaneous. Assume that the enthalpy and
entropy of vaporization change very little
with temperature.
𝑇= °C
Is the vaporization of A(l) spontaneous at temperatures
greater than or less than 𝑇?
greater than 𝑇
less than 𝑇