I am sitting with some exercises and having trouble with the calculation of equilibrium partial pressures.
The excercise is from Zumdahl's "Chemical Principles" 4th ed, ch. 6 ex. 31.
"At 1100 K, Kp= 0.25 atm-1 for the following reaction:
2SO2(g) + O2(g) <-> 2SO3(g)
Calculate the equilibrium partial pressures of SO2, O2 and SO3 produced from an initial mixture in which
P(SO2)=P(O2)=0.5 atm and P(SO3)=0"
Now, I get that the reaction will move right and that the equilibrium equation is:
Kp= P(SO3)^2 / P(SO2)^2*P(O2)
I have tried to solve the resulting equation but I go wrong somewhere and I don't know where.
I am assuming that, at equilibrium, the new partial pressures are:
SO2: 0.5 - 2x
I believe I am doing something fundamentally wrong, but don't know where.
I am pulling my hair so I would really appreciate some help.