K and Q

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Deena Doan 2F
Posts: 100
Joined: Sat Aug 17, 2019 12:17 am

K and Q

Postby Deena Doan 2F » Sun Jan 12, 2020 11:44 pm

I know that they are solved the same way but what is the difference between solving for K and solving for Q?

ckilkeary 2G
Posts: 68
Joined: Fri Aug 09, 2019 12:16 am

Re: K and Q

Postby ckilkeary 2G » Sun Jan 12, 2020 11:51 pm

The only difference between the two is that Q is a term used when it hasn't reached equilibrium yet. Since they're solved the same way, Q and K are just different terms you use depending on the situation.

Posts: 7
Joined: Fri Sep 28, 2018 12:20 am

Re: K and Q

Postby Alexaaguilera » Sun Jan 12, 2020 11:55 pm

You can use Q at anytime, unlike K

Venus_Hagan 2L
Posts: 104
Joined: Fri Aug 02, 2019 12:16 am

Re: K and Q

Postby Venus_Hagan 2L » Sun Jan 12, 2020 11:56 pm

yes they are both solved using the same formula ([products]/[reactants]) but Q is using the concentrations when the reaction is not at equilibrium and K is when it is at equilibrium

Ashley Fang 2G
Posts: 102
Joined: Fri Aug 30, 2019 12:17 am

Re: K and Q

Postby Ashley Fang 2G » Mon Jan 13, 2020 9:26 am

To add to that, by solving for Q and comparing it to K, you can see what direction the reaction will proceed.
If Q<K, the reaction will proceed to the right (products side).
If Q>K, the reaction will proceed to the left (reactants side).
If Q=K, the reaction is at equilibrium.

Sam McNeill 1E
Posts: 110
Joined: Sat Aug 24, 2019 12:17 am

Re: K and Q

Postby Sam McNeill 1E » Mon Jan 13, 2020 10:33 am

In addition, K is a constant that will remain the same as long as no conditions such as temperature change, and Q varies in value depending on when you calculate it during the reaction.

Mitchell Koss 4G
Posts: 128
Joined: Sat Jul 20, 2019 12:17 am

Re: K and Q

Postby Mitchell Koss 4G » Mon Jan 13, 2020 11:35 am

K is definite eq constant but Q is just the value at some time.

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