The initial pressure for the compounds involved in the reaction displayed were determined to be P(SO2(g)) = 0.5932 atm, P(O2(g)) = 0.4886 atm, P(SO3(g)) = 0.09287 atm. Calculate the value of the equilibrium constant (Kp) at 1000 K if the equilibrium pressure of O2(g) was 0.4924 atm.
2SO2(g)+O2(g) = 2SO3(g)
so you said that SO3 is decreased by 2*.0038, O2 is increased by .0038 but shouldnt SO2 increased by 2x.0038 since it has 2 moles
(.08527)^2/(.4924x.6008^2)
1 answer
Of course. 0.6008 is correct for pSO2. If I didn't type in the 2 it was a miscue on my part. What you have looks ok to me.
2 answers