Consider the chemical system CO + Cl2 = COCl2;K = 4.6 • 10^9L/Mol If the concent

Question

Consider the chemical system CO + Cl2 = COCl2;K = 4.6 • 10^9L/Mol
If the concentration of the product were to double, what would happen to the equilibrium constant? Consider the chemical system CO + Cl2 = COCl2;K = 4.6 • 10^9L/Mol
If the concentration of the product were to double, what would happen to the equilibrium constant? Consider the chemical system CO + Cl2 = COCl2;K = 4.6 • 10^9L/Mol
If the concentration of the product were to double, what would happen to the equilibrium constant?
If the concentration of the product were to double, what would happen to the equilibrium constant?

Explanation / Answer

answer

The position of equilibrium is changed if you change the concentration of something present in the mixture. According to Le Chatelier's Principle, the position of equilibrium moves in such a way as to tend to undo the change that you have made.

so if we increase the concentration of product then reaction moves backword and change the concentration of reactants and reaction again comes in equlibirium . so there has no change in equlibirium if the concentration of product is double.

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