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An industrial chemist puts 1.00 mole each of H2(g) and CO2(g) in a 1.00 L container...

An industrial chemist puts 1.00 mole each of H2(g) and CO2(g) in a 1.00 L container at a constant temperature of 800oC. This reaction occurs:

H2(g) + CO2(g) H2O(g) + CO(g)

When equilibrium is reached, 0.49 mole of CO2(g) is in the container. Find the value of Kc for the reaction.

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