Question

For a phase change, AH = 31 kJ/mol and Sº= 0.093 kJ/(K-mol). What are
AG and the spontaneity of the phase change at 300 K?
OA. AG 3.1 kJ; nonspontaneous
OB. AG=59 KJ; spontaneous
OC. AG= 3.1 kJ; spontaneous
O D. AG= 59 KJ; nonspontaneous

Answer 1

Based on the calculations, the Gibbs's free energy and spontaneity of the phase change are equal to: C. ΔG° = 3.1 kJ; spontaneous.

Given the following data:

• Enthalpy of reaction (ΔH°) = 31 kJ/mol.

• Temperature = 300 K.

• Entropy of reaction (ΔS°) = 0.093 kJ/mol.

How to calculate Gibbs's free energy?

Mathematically, the Gibbs's free energy for this chemical reaction can be calculated by using this formula:

ΔG° = ΔH° - ΔS°

Substituting the given parameters into the formula, we have;

ΔG° = 31 × 10³ - (300 × 0.093)

ΔG° = 31 × 10³ - 27.9 × 10³

ΔG° = 3.1 kJ.

Read more on Gibbs's free energy here: brainly.com/question/18752494

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