Chemistry: 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

i would help but its in spanish sorryExplanation:...

Calculate the value of the free energy change, ΔG,

hardwick744

23.01.2022

the value of the free energy change ΔG = 339.975 kJ

Explanation:

The equation for the reaction is given as :

$2POCl_{3(g)} \ + \ 2 PCl_{3(g)} \ + \ O_{2(g)}$

Equilibrium Constant K:

$K = \frac{[PCl_3]^2[O_2]}{[POCl_3]^2}\\\\K = \frac{(0.0150)^2*(0.0100)}{(10.00)^2}\\ \\K = 2.25*10^{-8}$

ΔGº = 489.75 kJ = 489750 J

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

T (temperature) = 1023 K

R( rate constant) = $8.314 \ J K^{-1} mol^{-1}$

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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