Q vs K

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Donna Nguyen 2L
Posts: 100
Joined: Sat Aug 24, 2019 12:17 am

Q vs K

Postby Donna Nguyen 2L » Thu Jan 09, 2020 12:51 am

What's the difference between Q and K? Or, how are they similar?

Diana_Diep2I
Posts: 130
Joined: Sat Aug 17, 2019 12:17 am

Re: Q vs K

Postby Diana_Diep2I » Thu Jan 09, 2020 12:57 am

Q is for when the reaction isn't at equilibrium. K is for when the reaction is at equilibrium.

ng1D
Posts: 43
Joined: Wed Sep 18, 2019 12:17 am

Re: Q vs K

Postby ng1D » Thu Jan 09, 2020 1:19 am

Q and K are similar in that they are calculated in the same way, Q = [P]/[R] and K = [P]/[R].

WesleyWu_1C
Posts: 117
Joined: Thu Jul 25, 2019 12:16 am

Re: Q vs K

Postby WesleyWu_1C » Thu Jan 09, 2020 1:29 am

The difference between Q and K is that K is the equilibrium constant which in other words is when the reaction has reached equilibrium. Q, the reaction quotient, is something you can do during anytime of the reaction. By comparing Q to K, you can see the direction of the reaction. If Q=K, then you know equilibrium has been reached.

Kayli Choy 2F
Posts: 100
Joined: Sat Aug 24, 2019 12:17 am

Re: Q vs K

Postby Kayli Choy 2F » Thu Jan 09, 2020 10:21 am

Additionally, if
- Q<K, the reaction will proceed forward to create more products
- Q>K, the reaction will proceed in reverse to create more reactants

Bryce Barbee
Posts: 103
Joined: Wed Sep 18, 2019 12:20 am

Re: Q vs K

Postby Bryce Barbee » Thu Jan 09, 2020 11:07 am

Q and K are essentially the same when it comes to calculating them. The difference is that K is the value when the reaction is at equilibrium while Q can be found at anytime during the reaction to see if the action is at equilibrium or not.

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805329408
Posts: 49
Joined: Wed Nov 20, 2019 12:21 am

Re: Q vs K

Postby 805329408 » Thu Jan 09, 2020 11:21 am

The reason why the reaction moves forward when the reaction quotient (Q) is less than the equilibrium constant (K) is because the lesser value means that there is less product than there should be when the reaction reaches equilibrium and thus more product is needed, so the reaction moves forward. As for when Q is greater than K, the reaction moves in the reverse direction because there is now more product than there is at equilibrium and thus you need to move backwards.

504939134
Posts: 103
Joined: Wed Sep 18, 2019 12:21 am

Re: Q vs K

Postby 504939134 » Thu Jan 09, 2020 2:25 pm

Q is not at equilibrium, it is just products over reactants at any given time during the reaction. K is the equilibrium constant of the products over her reactants.

Diana Andrade_4F
Posts: 50
Joined: Tue Nov 05, 2019 12:18 am

Re: Q vs K

Postby Diana Andrade_4F » Thu Jan 09, 2020 10:08 pm

K is an equilibrium constant, while Q is a reaction quotient. K is found when the reaction is at equilibrium, but Q can be calculated at any time during the reaction. You can compare the reaction quotient, Q, to the equilibrium constant, K, to determine the direction of the reaction.


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