CO2(g) + H2(g) ⇀↽ H2O(g) + CO(g) equilibrium?
The system
CO2(g) + H2(g) ⇀↽ H2O(g) + CO(g)
is at equilibrium at some temperature. At
equilibrium a 4.00 L vessel contains 1.00 mole
CO2, 1.00 mole H2, 2.40 moles H2O, and 2.40
moles CO. How many moles of CO2 must be
added to the system to bring the equilibrium
CO concentration to 0.753 mol/L? Answer in
units of moles.
Im confused and don't know how to go about the problem. Thank You for your help
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Verified answer
You need to calculate the equilibrium constant, Keq, by taking your initial concentrations and multiplying the molar concentrations of the products and then dividing by the product of the reactants, [H2O] x [CO] / [CO2] x [H2]. Adding CO2 to the system will stress the equilibrium according to LeChatlier's principle. If you substitute the new CO value in the Keq equation, then re-arrange to solve for the new unknown CO2, you can calculate the new CO2.
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