We’re given the following equilibrium:
CO(g) + H2O(g) ⇌ CO2(g) + H2(g)
At equilibrium, we have a 1.00-L container with 0.200 mol of CO and H2O and 0.700 mol of CO2 and H2. Recall that molarity is given by:
[CO] = [H2O] = 0.200 M
[CO2] = [H2] = 0.700 M
The Kc expression for this reaction is:
Note that each concentration is raised by the stoichiometric coefficient: [CO], [H2O], [CO2] and [H2] are raised to 1. Solving for Kc:
An equilibrium mixture contains 0.700 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00-L container.
CO (g) + H2O (g) ⇌ CO2 (g) + H2 (g)
How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.300 mol once equilibrium has been reestablished?
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