Calculate the value of the free energy change, ΔG, for the reaction below at 750.0ºC when the pressures of POCl3 (g) = 10.00 atm, PCl3 (g) = 0.0150 atm, and O2 (g) = 0.0100 atm.

2 POCl3 (g) →2 PCl3 (g) + O2 (g)

ΔGº = 489.75 kJ

ΔHº = 542.8 kJ

ΔSº = 177.93 J/K

the value of the free energy change ΔG =  339.975 kJ

Explanation:

The equation for the reaction is given as :

Equilibrium Constant K:

ΔGº = 489.75 kJ = 489750 J

T (temperature) = 750.0ºC = ( 750.0 + 273 )K

T (temperature) = 1023 K

R( rate constant) =

Using the equation :

ΔG = ΔG° + RT ㏑ K

ΔG =  (489750) + ( 8.314)(1023)㏑ ( 2.25 × 10⁻⁸)

ΔG =  489750 + 8505.22 × (-17.6098)

ΔG = 339974.78 J

ΔG =  339.975 kJ

Thus, the value of the free energy change ΔG =  339.975 kJ

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