If a reaction system has come to equilibrium, the concentration of products can be increased by doing what?

Answer 1

By a miracle........

The equilibrium reaction is in your possession.

#A+BrightleftharpoonsC+D#

And #K_(eq)=([C][D])/([A][B])#; now #K_(eq)# may or may not be affected by temperature; and typically we specify standard conditions. But by definition, #"equilibrium"#, equality of forward and reverse rates, is A CONSTANT. We could add a catalyst so that the condition of equilibrium is achieved FASTER, but neither #K_(eq)# nor the equilibrium concentrations could be altered.

Of course, in the given equilibrium, we could drive the reaction to completion, by removing the products #C# and #D#, but here we manipulate an equilibrium, and do not change its value.

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Answer 2

Wyatt Adkins

By removing some of the products from the reaction mixture, according to Le Chatelier's Principle, the equilibrium will shift to the right to replace the removed products, thereby increasing the concentration of products.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.