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How would you find Keq for a reaction that has 0 concentration at equilibrium. If a...

How would you find Keq for a reaction that has 0 concentration at equilibrium. If a reactant had 0 concentration at equilibrium, if you plugged in the values for finding Keq, wouldnt you be dividing by 0 which you cant do?

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Answer #1

At the equilibrium the reagents and products have a constant concentration that divided gives the value of Keq. Theoretically, if your system is "open", i mean, the product is leaving the flask where the reactions is done for example, then one of the reagents will be consumed and the reaction stops.

But if your system is closed, then the reagents will react until the amount of product produced is enough to reach the Keq. So you will never have to divide by 0 in a closed system.

At equilibrium products transform into reagents and reagents into products at the same velocity, this makes the concentration of them constant.

Let me know if you have any doubt :)

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