The value of δg∘ at 201.0∘c for the formation of phosphorous trichloride from its constituent elements, p2(g)+3cl2(g)→2pcl3(g) is kj/mol. at 25.0∘c for this reaction, δh∘ is −720.5kj/mol, δg∘ is −642.9kj/mol, and δs∘ is −263.7j/k.

The value of ΔG° at 201.0∘C for the formation of phosphorous trichloride is -595.5 kJ/mol.

Explanation:

Gibbs free energy of the reaction = ΔG° = -642.9 kJ/mol = -642,900 J/mol

Enthalpy of the reaction = ΔH° = -720.5 kJ/mol = -720,500 J/mol

Change in entropy of the reaction = ΔS° = -263.7 J/mol

Gibbs free energy of the reaction at 201.0°C = ΔG° = ?

T = 201.0°C  = 474.15 K

Using Gibbs's energy equation:

The value of ΔG° at 201.0∘C for the formation of phosphorous trichloride is -595.5 kJ/mol.

i do not get it   at all