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Q vs. K

Posted: Sun Nov 26, 2017 10:43 am
by Ava Harvey 2B
What exactly is the difference between the reaction quotient, Q, and the equilibrium constant, K? Also, what’s the difference in terms of solving for them?

Re: Q vs. K

Posted: Sun Nov 26, 2017 11:24 am
by AtreyiMitra2L
Q can be the concentrations of the reactants and products at any point in the reaction. K can only be the concentrations of the reactants at equilibrium. You go about solving them the same way. By using both Q and K, we can determine which way the reaction is more likely to proceed.

Re: Q vs. K

Posted: Sun Nov 26, 2017 11:27 am
by Alissa Stanley 3G
So it is possible for Q and K to be equal, if Q is at equilibrium?

Re: Q vs. K

Posted: Sun Nov 26, 2017 11:31 am
by AtreyiMitra2L
Alissa Stanley 3G wrote:So it is possible for Q and K to be equal, if Q is at equilibrium?


Yes! If Q and K are equal, we know that the mixture has equilibrium composition and has no tendency to change in either direction.