Question

Consider the heterogeneous equilibrium process shown below.
C(s) + CO2(g) 2 CO(g)
At 700.°C, the total pressure of the system is found to be 3.87 atm. If the equilibrium constant KP is 1.52, calculate the equilibrium partial pressures of CO2 and CO.

Answer 1

I assume that at equilibrium Ptotal = 3.87 atm.
.........C(s) + CO2(g) ==> 2CO(g)
E...............3.87-p......p..

If Ptotal = 3.87, if we call CO p then CO2 is 3.87-p. Substitute into Kp expression and solve.