Asked by Alan
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.
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.
Answers
Answered by
DrBob222
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.
.........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.
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