Q vs. K

sallina_yehdego 2E
Posts: 75
Joined: Sun Apr 29, 2018 3:00 am

Q vs. K

What's the difference between Q and K??

Posts: 37
Joined: Mon Apr 23, 2018 3:00 am

Re: Q vs. K

K is the equilibrium constant while Q is the reaction quotient. So when you calculate Q, the reaction is not necessarily at equilibrium, though the equation to solve for Q and K are the same. You can then compare the values of Q and K to determine which direction the reaction will go.

I am Sodium Funny
Posts: 65
Joined: Fri Sep 28, 2018 12:26 am

Re: Q vs. K

K is a value for the the rate of the reaction at equilibrium.

Q is a meusurement of the the rate of the reaction at any given time. But we know that the reaction will always try to attain equilibrium so the value of Q will be driven towards K. Anna O 2C
Posts: 98
Joined: Fri Sep 28, 2018 12:19 am

Re: Q vs. K

Q is calculated in the same way as K, only it can be taken at anytime during the reaction instead of K which is exclusively valued at the time of equilibrium. Because Q is the same ratio as K, you can utilize its value in relation to K to determine where the reaction lies in its accordance to the given equilibrium.

Henry_Phan_4L
Posts: 68
Joined: Fri Sep 28, 2018 12:24 am

Re: Q vs. K

Can Q fluctuate around K so that it could be higher at one point and lower at another point?

A De Castro 14B 2H
Posts: 75
Joined: Fri Sep 28, 2018 12:29 am

Re: Q vs. K

Henry_Phan_4L wrote:Can Q fluctuate around K so that it could be higher at one point and lower at another point?

I believe that Q can fluctuate around K, depending on the specific given time you measure Q. For instance, if you measure Q a few seconds after products are added to the system, Q will be greater than K (the system will shift to the left). On the other hand, if you measure Q a few seconds after reactants are added to the system, Q will be less than K (the system will shift to the right).

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