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For the reaction below determine what is ΔG° and if the reaction is spontaneous?


PCl_5(g) → PCl_3(g) + Cl2(g) at 298 K, [Keq = 1.87 × 10^-7, ΔS° = 1.8192 J/(mol ∙K)]


A.

3.84 × 10^4 kJ/mol, No


B.

7.68 kJ/mol, No


C.

-7.68 kJ/mol, Yes


D.

38.4 kJ/mol, No


E.

-38.4 kJ/mol, Yes

Answer :

The answer to the question is ΔG° = 7.68 kJ/mol and the reaction is not spontaneous. The ΔG° for the given reaction is 7.68 kJ/mol and the reaction is not spontaneous because ΔG° is positive.

In Chemistry, the Gibbs free energy change, denoted as ΔG°, can help us predict whether a reaction is spontaneous. It's possible to calculate ΔG° using the formula ΔG° = -RTln(Keq), where R = 8.3145 J/(mol•K), T is the temperature in Kelvin, and Keq is the equilibrium constant.

In your problem, T=298 K and Keq=1.87 x 10^-7. Putting these values in, ΔG° equals 7.68 kJ/mol. The positive ΔG° value tells us that the reaction is not spontaneous.

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