Q vs. K

Moderators: Chem_Mod, Chem_Admin

Ava Harvey 2B
Posts: 54
Joined: Fri Sep 29, 2017 7:04 am

Q vs. K

Postby Ava Harvey 2B » Sun Nov 26, 2017 10:43 am

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?

AtreyiMitra2L
Posts: 169
Joined: Fri Sep 29, 2017 7:03 am
Been upvoted: 1 time

Re: Q vs. K

Postby AtreyiMitra2L » Sun Nov 26, 2017 11:24 am

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.

Alissa Stanley 3G
Posts: 22
Joined: Fri Sep 29, 2017 7:06 am
Been upvoted: 1 time

Re: Q vs. K

Postby Alissa Stanley 3G » Sun Nov 26, 2017 11:27 am

So it is possible for Q and K to be equal, if Q is at equilibrium?

AtreyiMitra2L
Posts: 169
Joined: Fri Sep 29, 2017 7:03 am
Been upvoted: 1 time

Re: Q vs. K

Postby AtreyiMitra2L » Sun Nov 26, 2017 11:31 am

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.


Return to “Equilibrium Constants & Calculating Concentrations”

Who is online

Users browsing this forum: No registered users and 1 guest