Consider the reaction:
2Mg + O2 ------> 2MgO
The reaction is at equilibrium, the concentration of MgO is found to be 0.5.
What is the concentration of Mg and O2?
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Keq is not given... using the ICE table, I ended up with the following:
Keq = [MgO]^2 / [Mg]^2 * [O2]
Keq = [0.5]^2 / [2x - 0.5]^2 * [x - 0.5]
Keq = 0.25 / 2x(x - 1) + 0.25
Not sure what to do.. or if I'm even going in the right direction
1 answer
This question (and the duplicate just before) makes no sense to me. There is no Keq given because the equilibrium lies far to the right; i.e., it essentially goes to completion. Another problem is that concentration of a solid makes no sense either. A third problem is that even if this were an equilibrium problem solids don't appear in the Keq expression. I suspect you have misinterpreted the problem and posted your question based on that. If you posted the problem exactly as it appears in your homework it might make more sense to me.