Q vs. K

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Ellen Hsieh 3F
Posts: 4
Joined: Fri Sep 25, 2015 3:00 am

Q vs. K

Postby Ellen Hsieh 3F » Sun Nov 15, 2015 11:07 pm

What is the difference between a reaction quotient (Q) and an equilibrium constant (K)?

Neel Patel - 2A
Posts: 48
Joined: Fri Sep 25, 2015 3:00 am

Re: Q vs. K

Postby Neel Patel - 2A » Sun Nov 15, 2015 11:14 pm

K is essentially the reaction quotient at equilibrium. The reaction quotient can be used to determine if there are more products or reactants present in relation to equilibrium. If K is found to be greater than Q, then there are more products relative to reactants at equilibrium. If K is found to be smaller than Q, then there are more reactants relative to products at equilibrium.

604607619
Posts: 22
Joined: Fri Sep 25, 2015 3:00 am

Re: Q vs. K

Postby 604607619 » Tue Dec 01, 2015 2:59 pm

also, K is fixed value and is the same if the reaction is done under the same temperature regardless of how much reactant you start with.

Laila Sathe 1D
Posts: 27
Joined: Fri Sep 25, 2015 3:00 am

Re: Q vs. K

Postby Laila Sathe 1D » Tue Dec 01, 2015 3:42 pm

Q and K represent the same kind of value, but they're used at different times. K is the equilibrium constant, meaning it represents the ratio of products to reactants at equilibrium. Q is the reaction quotient, meaning it represents the ratio of products to reactants at some other point, not necessarily at equilibrium.


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