Pt 2 - How do I calculate the partial pressure?

Question

Calculate the partial pressure (in atm) of CH3OH at equilibrium when 52.3g of Co and 2.67 atm of CO2 react at 1000K according to:

Co (s) + CO2 (g) ⇔ CoO (s) + CO (g)

kp= 7.04 x 10^-2

Answer 1

K_P = P_CO/P_CO2 at equilibrium

Let x be the the partial pressure of CO₂ that reacts in order to achieve equilibrium

P_CO,eq = 2.67 - x and P_CO2,eq = x

so

.0704 = x/(2.87 -x) We can assume that 52.3 g of solid is enough to provide the Co necessary to reach equilibrium (we really don't have enough data to check, need volume of container)

multiply out and solve for x which is P_CO (Did you mean CO rather CH₃OH?)

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