The equilibrium constant Kp for the reaction C(s)+H2O(g)?CO(g)+H2(g) is 2.44 at 1000 K. What are the equilibrium partial pressures of H2O, CO, and H2 if the initial partial pressures are PCO= 1.25 atm, and PH2= 1.60 atm?
What is the equilibrium partial pressure of H2O?
What is the equilibrium partial pressure of CO?
What is the equilibrium partial pressure of H2?
Balanced equation with ICE table
C(s) + H2O(g) = CO(g) + H2(g)
I 1.25 1.60
C - x +x +x
E - x 1.25+x 1.60+x
Equilibrium constant expression of the reaction
Kp = PCO x PH2 / PH2O
2.44 = (1.25+x)(1.60+x)/(-x)
-2.44x = 2 + 1.25x + 1.60x + x2
x2 + 5.29x + 2 = 0
x = - 0.4098
x is negative because the reaction Wil be in the reverse direction
equilibrium partial pressure of H2O = - x = 0.4098 atm
equilibrium partial pressure of CO = 1.25 - 0.4098 = 0.8402 atm
equilibrium partial pressure of H2 = 1.60 - 0.4098 = 1.1902 atm
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