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For the gaseous reaction of xenon and fluorine to form xenon hexafluoride:(b) Assuming that ΔS° and ΔH° change little with temperature, calculate ΔG° at 500. K.

Respuesta :

ΔG° at 500. K ΔG°=  -197.5kJ/mol

The expression for the standard change in free energy is:

ΔG° = ΔH°-TΔS°

Where,

ΔG° is the change in the Gibbs free energy.

T is the absolute temperature. (T in kelvins)

ΔH° is the enthalpy change of the reaction.

ΔS° is the change in entropy.

We have,

at T = 500 K

Because ΔG° = ΔH°-TΔS°

at 500K, ΔG° = -197.5kJ/mol.

ΔG°= -402kJ/mol- (500K) (-0.409kJ/mol.K)

ΔG°= -197.5kJ/mol

hence at 500 K ΔG°=  -197.5kJ/mol

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