Answer:
0 kJ/mol
Explanation:
Step 1: Given data
- Enthalpy change (ΔH): 27 kJ/mol
- Entropy change (ΔS): 0.09 kJ/mol.K
- Absolute temperature (T): 300 K
Step 2: Calculate the Gibbs free energy change (ΔG)
We can calculate the Gibbs free energy change using the following expression.
ΔG = ΔH - T × ΔS
ΔG = 27 kJ/mol - 300 K × 0.09 kJ/mol.K = 0 kJ/mol
Since ΔG = 0 kJ/mol, the process in not spontaneous nor non-spontaneous.
