The value of delta g at 141.0 degrees celsius for the formation of phosphorous trichloride from its constituent elements,

p2(g) + 3cl2(g) > 2pcl3(g)

is kj/mol. at 25.0 degrees celsius for this reaction, delta h is -720.5 kj/mol, delta g is -642.9 kj/mol, and delta s is -263.7 j/k.

a.) -829.7

b.) 1.08 x 10^5

c.) 3.65 x 10^4

d.) -683.3

e.) -611.3

The correct answer is option E.

Explanation:

The Gibbs free energy is given by expression:

ΔG = ΔH - TΔS

ΔH = Enthalpy change of the reaction

T = Temperature of the reaction

ΔS = Entropy change

We have :

ΔH = -720.5 kJ/mol =  -720500 J/mol (1 kJ = 1000 J)

ΔS = -263.7 J/K

T = 141.0°C = 414.15 K

The Gibb's free energy of the given reaction at 141.0°C is -611.3 kJ/mol.

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