At 1000 K, Kp = 19.9 for the following reaction:
Fe2O3(s)+3CO(g)⇌2Fe(s)+3CO2(g)
What are the equilibrium partial pressures of CO and CO2 if CO is the only gas present initially, at a partial pressure of 0.982 atm ?
Kp = [CO2]^3/[CO]^3
initial [CO] = 0.982 atm
let x be the change in pressure at equilibrium
19.9 = (3x^2)^3/(0.982 - 3x)^3
(0.982 - 3x) (0.982 - 3x) (0.982 - 3x)
0.964 - 5.892x + 9x^2
0.9466 - 2.892x - 5.786x + 17.676x^2 + 8.838x^2 - 27x^3 = 27x^3
54x^3 - 26.514x^2 + 8.678x - 0.9466 = 0
x = 0.163 atm
So the equilibrium concentration for,
[CO] = 0.982 - 3 x 0.163 = 0.493 atm
[CO2] = 0.489 atm
At 1000 K, Kp = 19.9 for the following reaction: Fe2O3(s)+3CO(g)⇌2Fe(s)+3CO2(g) What are the equilibrium partial...
At 1000 K, Kp = 19.9 for the reaction Fe2O3(s)+3CO(g)⇌2Fe(s)+3CO2(g). What are the equilibrium partial pressures of CO and CO2 if CO is the only gas present initially, at a partial pressure of 0.986 atm ? Enter your answers numerically separated by a comma.
At 1000 KK, KpKp = 19.9 for the reaction Fe2O3(s)+3CO(g)⇌2Fe(s)+3CO2(g)Fe2O3(s)+3CO(g)⇌2Fe(s)+3CO2(g). Part A What are the equilibrium partial pressures of COCO and CO2CO2 if COCO is the only gas present initially, at a partial pressure of 0.954 atmatm ?
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