At 1000 K, Kp = 19.9 for the reaction Fe2O3(s)+3CO(g)⇌2Fe(s)+3CO2(g). What are the equilibrium partial pressures...
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.
Homework Answers
Sol.
Reaction :
Fe2O3(s) + 3CO(g) <-----> 2Fe(s) + 3CO2(g)
initial 0.986 0
change - 3x + 3x
equilibrium 0.986 - 3x 3x
So , Kp = (PCO2)3 / (PCO)3
19.9 = (3x)3 / (0.986 - 3x)3
3x / (0.986 - 3x ) = (19.9)1/3 = 2.709
3x = 2.709 ( 0.986 - 3x ) = 2.671 - 8.127x
x = 2.671 / 11.127 = 0.240
Therefore ,
Equilibrium partial Pressures are :
PCO = 0.986 - 3 × 0.240 = 0.266 atm
PCO2 = 3 × 0.240 = 0.720 atm
Add Answer to:
At 1000 K, Kp = 19.9 for the reaction
Fe2O3(s)+3CO(g)⇌2Fe(s)+3CO2(g).
What are the equilibrium partial pressures...
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