...state what the equilibrium partial pressure of CO is and hence calculate the equilibrium constant.?

Question

Part of the process by which coal can be converted into a combustible mixture of gases involves passing steam over white hot coke:

H2O (g) + C (s) = H2 )g + CO (g); ΔH = +131 kJ mol^-1

When steam was passed over coke at 730°C, the following partial pressures were measured at equilibrium:

p(H2O) = 90 kPa
p(H2) = 183 kPa

State what the equilibrium partial pressure of carbon monoxide is and hence calculate the equilibrium constant.

I'm pretty much able to write the expression for Kp - the equilibrium constant and suchlike, but I'm confused as to how to find both the PP of CO at equilibrium and the equilibrium constant when they're both unknowns, the way I see it. A little help, please? Thank you. :)

Answer 1

The molar ratio is 2:2 or 1:1

Partial Pressure (CO) = p(H2) = 183kPa

Kp = (183)^2/(90^2) = 4.13 [-]

(the [-] indicates it is dimensionless (no units))

i think thats right anyway...