A Kc Equilibrium Calculation

[Ttan]

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For the water-gas reaction (C(s)+H2O(g)<---->CO(g)+H2(g), Kc=.111 @ 1100K.
If .1 mol H2O(g) and .1 mol H2(g) are mixed with excess C(s) at this temperature and equilibrium is established, how many moles of CO(g) will be present? No CO(g) is present initially.

Forget/cant find the method for doing this when there is a 0-value initially on one of the concentrations.

Thank you much.

 

[PiBond]

Keq = Products / reactants (stoichiometric coefficients become exponents but there are none here)
We leave out solids because they're constant

Make an ICE chart

Initially: CO(g) is zero. H20 and H2 are .1 moles
Change: subtract x from H20, add x to CO and H2
Equilibrium conc: set your concentrations equal to your equilibrium constant (given in problem); solve for x which will give you the amount of CO(g) present at equilibrium

 

[kidkay]

For the water-gas reaction (C(s)+H2O(g)<---->CO(g)+H2(g), Kc=.111 @ 1100K.
If .1 mol H2O(g) and .1 mol H2(g) are mixed with excess C(s) at this temperature and equilibrium is established, how many moles of CO(g) will be present? No CO(g) is present initially.

Forget/cant find the method for doing this when there is a 0-value initially on one of the concentrations.

Thank you much.

What's your volume? You will need the volume(unless we assuming the volume is one liter) for the Molarity formula. M=mol/L. You'll need the molarity (equilibrium concentration), when solving....