Answer:
Explanation:
In the equilibrium:
CO(g) + H₂O(g) ⇄ CO₂(g) + H₂(g)
Kc is:
Kc = 1.845 = [CO₂] [H₂] / [CO] [H₂O]
<em>Where [] are equilibrium concentrations of each species</em>
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Initial concentrations:
[CO] = 0.500mol / 1.00L = 0.500M
[H₂O] = 0.500mol / 1.00L = 0.500M
In equilibrium, concentrations will be:
[CO] = 0.500M - X
[H₂O] = 0.500M - X
[CO₂] = X
[H₂] = X
<em>Where X is reaction coordinate. The amount of reactant that reacts producing products.</em>
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Replacing in Kc expression:
1.845 = [CO₂] [H₂] / [CO] [H₂O]
1.845 = [X] [X] / [0.500M - X] [0.500M - X]
1.845 = X² / X² - X + 0.25
1.845X² - 1.845X + 0.46125 = X²
0.845X² - 1.845X + 0.46125 = 0
Solving for X:
X = 0.288M; Right solution
X = 1.9M; False solution: Produce negative concentrations.
Replacing, equilibrium concentrations are:
[CO] = 0.500M - X = 0.212M
[H₂O] = 0.500M - X = 0.212M
[CO₂] = X = 0.288M
[H₂] = X = 0.288M
