Consider the reaction: H2(g) + CO2(g) ⇄ H2O(g) + CO(g)
0.80 mole of H2 and 0.80 mole of CO2 are placed in a 5-dm3 container at 1650 oC. At equilibrium, 0.25 mole of CO was found in the equilibrium mixture. Calculate the equilibrium constant Kc.

Question

Consider the reaction: H2(g) + CO2(g) ⇄ H2O(g) + CO(g)
0.80 mole of H2 and 0.80 mole of CO2 are placed in a 5-dm3 container at 1650 oC. At equilibrium, 0.25 mole of CO was found in the equilibrium mixture. Calculate the equilibrium constant Kc.

jfraser · Answer

If you've formed 0.25mol of CO, then you must have stoichiometrically lost the same amount of H2 and CO2. You must also have formed the same amount of H2O. Use that info (and the volume of the container) to find the concentrations of the reactants and products, then plug into the general equilibrium expression equation

anonymous · Answer

then what is mol of H2O??

jfraser · Answer

what's the balanced reaction say? if you form 0.25mol of CO, then you must also form 0.25mol of H2O