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The vaporization of compound A is described by the given chemical equation. A(l)⟶A(g)ΔHvap∘=42.69 kJ/mol Calculate the...

The vaporization of compound A is described by the given chemical equation.

A(l)⟶A(g)ΔHvap∘=42.69 kJ/mol

Calculate the entropy of vaporization, ΔSvap , for A(l) at 25.0 °C given that the boiling point of A is 78.99 °C , and the molar heat capacity of A(l) is 118.41 J/(mol⋅K) . Assume that the molar heat capacity of A(g) is 53.7% of that of A(l) .

ΔSvap=

J⋅mol−1⋅K−1

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 181.0 °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?

less than T

greater than T

Expert Solution

queen_honey_blossom answered 1 year ago

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