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Understanding Q

Posted: Fri Jan 18, 2019 6:47 pm
by Cecilia Jardon 1I
Just to clarify, Q is the same chemical reaction but just in the state where it has not yet reached equilibrium?

Re: Understanding Q

Posted: Fri Jan 18, 2019 7:10 pm
by MaanasO 1A
Hi Cecilia!

So Q and K are calculated in the same way but with different concentrations. Think of K as the Q when the reaction is at equilibrium.

Hope that helps!

Re: Understanding Q

Posted: Fri Jan 18, 2019 7:16 pm
by Casandra
Q alone tells you nothing, but once compared to K, it tells you where the reaction is in terms of reaching the equilibrium concentration.

Re: Understanding Q

Posted: Sat Jan 19, 2019 1:57 am
by Cade Okohira 4K
You find Q and K in the same way, by dividing the concentrations of the products by the concentrations of the reactants. However, K is the equilibrium constant, while Q is the reaction quotient, which is the constant of the equation at any time. Q can then be compared to K to find out whether the equation is shifting to the left or right (or favoring the reactants or products).

Re: Understanding Q

Posted: Sat Jan 19, 2019 2:23 am
by Dayna Pham 1I
Adding onto what they all said, I’d like to relate this to Le Chatelier’s Principle. When pressure/volume/concentration change, it is Q that changes, not K. However, when temperature changes, then K changes.

Re: Understanding Q

Posted: Sat Jan 19, 2019 3:11 am
by 005113695
Hi!
Q is calculated the same way as K, but instead of being the equilibrium concentration, it can tell you which way the reaction is proceeding.

Re: Understanding Q

Posted: Sat Jan 19, 2019 10:24 am
by MichaelMoreno2G
Can someone clarify what the significance of Q<K is and vice-versa?

Re: Understanding Q

Posted: Sat Jan 19, 2019 12:32 pm
by Karishma_1G
K>Q and K<Q is significant because it helps us understand whether the reaction has reached equilibrium or not. Since Q (the reaction quotient) is calculated at a specific time during the span of a reaction, by comparing it to K we can see if the reaction has to form more products or reactants to reach equilibrium. If K>Q, the reaction will proceed to the products. If K<Q, the reaction will proceed to the reactants.

Re: Understanding Q

Posted: Sun Jan 20, 2019 3:38 pm
by Simmi Diwanji 2B
The significance of Q<K and vice versa is that it helps determine whether a reaction has reached equilibrium at a certain point in time. If it hasn't reached equilibrium (Q=K), than that means that the reaction will either favor the reactants or products in order to proceed towards equilibrium.

Re: Understanding Q

Posted: Sun Jan 20, 2019 4:21 pm
by Sapna Ramappa 1J
Comparing Q and K allows us to see whether or not the system is at equilibrium. If Q=K, then the system is at equilibrium. Otherwise, we can see if Q>K or if K>Q to determine whether the reaction favors the reactants or the products.