Answer:
the value of the free energy change ΔG = 339.975 kJ
Explanation:
The equation for the reaction is given as :
[tex]2POCl_{3(g)} \ + \ 2 PCl_{3(g)} \ + \ O_{2(g)}[/tex]
Equilibrium Constant K:
[tex]K = \frac{[PCl_3]^2[O_2]}{[POCl_3]^2}\\\\K = \frac{(0.0150)^2*(0.0100)}{(10.00)^2}\\ \\K = 2.25*10^{-8}[/tex]
ΔGº = 489.75 kJ = 489750 J
T (temperature) = 750.0ºC = ( 750.0 + 273 )K
T (temperature) = 1023 K
R( rate constant) = [tex]8.314 \ J K^{-1} mol^{-1}[/tex]
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
