To determine the equilibrium partial pressure of O2 (g) at 350 degrees Celsius, we can use the expression for the equilibrium constant (Kp):
Kp = (PO2)^n / (PSO3)^m
Where n and m are the coefficients of O2 and SO3 in the balanced equation, respectively.
From the balanced equation:
2SO3 (g) -> 2SO2 (g) + O2 (g)
We can see that n = 1 (coefficient of O2) and m = 2 (coefficient of SO3).
Given that Kp = 1.79 x 10^-5, we can substitute the known values into the equation:
1.79 x 10^-5 = (PO2)^1 / (0.200 atm)^2
To solve for PO2, let's rearrange the equation:
PO2 = (1.79 x 10^-5) * (0.200 atm)^2
PO2 = 7.16 x 10^-8 atm
Therefore, the partial pressure of O2 (g) at equilibrium is approximately 7.16 x 10^-8 atm.