The water-gas shift reaction is crucial to many industrial processes: H2O(g) + CO(g) ↔ H2(g) + CO2(g) The equilibrium constant for this reaction is K = 2.993787 at 806.0 K. If a vessel is initially charged with 6 bar each of H2O(g) and CO(g), what is the final equilibrium pressure of H2(g)?

Chemistry: The Molecular Science
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Chapter12: Chemical Equilibrium
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The water-gas shift reaction is crucial to many industrial processes:
H2O(g) + CO(g) ↔ H2(g) + CO2(g)
The equilibrium constant for this reaction is K = 2.993787 at 806.0 K. If a vessel is initially charged with 6 bar each of H2O(g) and CO(g), what is the final equilibrium pressure of H2(g)?

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