Understanding Q

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Emma Randolph 1J
Posts: 65
Joined: Fri Sep 28, 2018 12:29 am

Understanding Q

Postby Emma Randolph 1J » Sat Jan 12, 2019 9:20 pm

When solving for Q and comparing it to K, why is it that if Q < K it means that more products are formed and if Q > K it means more reactants are formed? I'm confused trying to figure this out conceptually.

Brian Chhoy 4I
Posts: 66
Joined: Fri Sep 28, 2018 12:16 am

Re: Understanding Q

Postby Brian Chhoy 4I » Sat Jan 12, 2019 10:03 pm

Recall that you solve for K=(products)/(reactants). Thus when Q<K, to increase Q and get the reaction to equilibrium, you would have to increase the numerator(products) and decrease the denominator(reactants). That is why more products are formed. The same can be said for when Q>K, to decrease Q and get the reaction to equilibrium, you would have to decrease the products and increase the reactants, forming more reactants.

Anjali_Kumar1F
Posts: 62
Joined: Fri Sep 28, 2018 12:25 am

Re: Understanding Q

Postby Anjali_Kumar1F » Sat Jan 12, 2019 10:48 pm

What is quotient and what is the difference between quotient and K if they are calculated the same way.

Brian Chhoy 4I
Posts: 66
Joined: Fri Sep 28, 2018 12:16 am

Re: Understanding Q

Postby Brian Chhoy 4I » Fri Jan 18, 2019 2:05 pm

The quotient (Q), is simply the ratio of products:reactants at that point in the reaction. Eventually Q will have to approach K and thus we can make assumptions about how the reaction will proceed using the Q.


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