Q vs K

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vanessas0123
Posts: 100
Joined: Wed Sep 11, 2019 12:17 am

Q vs K

Postby vanessas0123 » Thu Jan 09, 2020 3:15 pm

What's the difference between Q and K?

Jada Brown 2H
Posts: 100
Joined: Sat Aug 17, 2019 12:15 am

Re: Q vs K

Postby Jada Brown 2H » Thu Jan 09, 2020 3:16 pm

K is the ratio of products to reactants at equilibrium, while Q is the ratio of products to reactants at any given point in the reaction (not necessarily equilibrium).

Ally Huang- 1F
Posts: 103
Joined: Thu Jul 25, 2019 12:16 am

Re: Q vs K

Postby Ally Huang- 1F » Thu Jan 09, 2020 3:17 pm

K is the constant you get for the ratio of the concentration of products at equilibrium to the concentration of reactants at equilibrium. Q is the ratio of products to reactants at any time. Q is used as a point of comparison to K to determine which direction the reaction will proceed to reach equilibrium.
Last edited by Ally Huang- 1F on Thu Jan 09, 2020 3:23 pm, edited 1 time in total.

Cooper Baddley 1F
Posts: 100
Joined: Wed Sep 18, 2019 12:19 am

Re: Q vs K

Postby Cooper Baddley 1F » Thu Jan 09, 2020 3:17 pm

K is the ratio of products over reactants at equilibrium, Q is the same thing not at equilibrium

Grace Jansen 2A
Posts: 28
Joined: Sat Jul 20, 2019 12:16 am

Re: Q vs K

Postby Grace Jansen 2A » Thu Jan 09, 2020 4:08 pm

Q is used when the reaction is not at equilibrium and K is the ratio of products to reactant when the system is at equilibrium.

Ellis Song 4I
Posts: 102
Joined: Thu Jul 11, 2019 12:17 am

Re: Q vs K

Postby Ellis Song 4I » Thu Jan 09, 2020 4:15 pm

Q and K are calculated the same but Q is the value at any point during the reaction while K is the value at equilibrium.

KnarGeghamyan1B
Posts: 102
Joined: Fri Aug 09, 2019 12:15 am

Re: Q vs K

Postby KnarGeghamyan1B » Thu Jan 09, 2020 4:23 pm

If Q is less than K at some time during the reaction, then compared to the equilibrium concentrations [R] > [P] and the forward reaction is favored, and vice versa.

MeeraBhagat
Posts: 95
Joined: Sat Aug 24, 2019 12:15 am

Re: Q vs K

Postby MeeraBhagat » Thu Jan 09, 2020 6:14 pm

Q is used to evaluate the concentration of reactants and products at any given point in a reaction. If Q = K, then the reaction is in equilibrium at that time. If Q>K, then that means there are more reactants present at that time than there would be if the reaction was in equilibrium. If Q<K, that means that there are more products at that point than there would be if the reaction was in equilibrium.


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