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For the reaction CO(g) + H_{2}O(g)CO_{2}(g) + H_{2}(g), K_{c} = 23.3 at 600 K. If 0.250 mol each of CO and H_{2}O are introduced into a reaction vessel and equilibrium is established, how many moles each of CO_{2} and H_{2} will be present at equilibrium? (Hint: Does the volume of the reaction mixture matter?)
Set up a table of concentrations and solve from there.










Initial 





Change 





Equilibrium 




Note that the volume of the container does not matter in this problem (this is not always true):
Because the stoichiometry of the reactants and products is the same, the volume terms cancel out.
To solve the problem:
So the number moles of CO_{2} = the number of moles of H_{2} = 0.207 mol