Q and K


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nathansalce 3e
Posts: 52
Joined: Thu Jul 27, 2017 3:01 am

Q and K

Postby nathansalce 3e » Wed Feb 21, 2018 6:58 pm

So in the context of equilibrium from 14A and the context of this chapter how does the values of K and Q in reference to their value against 1 (If K is greater than 1, then x. If K is less than 1, then y). Are the concepts the same no matter the contexts? Or do they change depending on which chapter's context we are applying.

Humza_Khan_2J
Posts: 56
Joined: Thu Jul 13, 2017 3:00 am

Re: Q and K

Postby Humza_Khan_2J » Wed Feb 21, 2018 8:03 pm

These concepts are overarching within chemistry. If K is much larger than 1, then the reaction heavily favors the products(as written). If Q>K, then more reactants will be formed. Similarly, if Q<K then more product will be formed.

Alexandria Weinberger
Posts: 51
Joined: Fri Sep 29, 2017 7:03 am

Re: Q and K

Postby Alexandria Weinberger » Mon Feb 26, 2018 2:08 pm

The concept of Q and K should be the same throughout chemistry, since they are purely related to equilibrium, although can be applied to other topics.

Jennie Fox 1D
Posts: 66
Joined: Sat Jul 22, 2017 3:01 am

Re: Q and K

Postby Jennie Fox 1D » Mon Feb 26, 2018 4:24 pm

Q and K are constant throughout chemistry, having mainly to do with equilibrium.

andrewr2H
Posts: 29
Joined: Fri Sep 29, 2017 7:05 am

Re: Q and K

Postby andrewr2H » Mon Feb 26, 2018 9:10 pm

The concepts remain true throughout chemistry, but it is true that there may be additional methods such as Gibbs Free Energy that we may learn to determine if a reaction is at equilibrium and in which direction it will occur if it is not.

Sarah Sharma 2J
Posts: 33
Joined: Fri Sep 29, 2017 7:05 am

Re: Q and K

Postby Sarah Sharma 2J » Mon Feb 26, 2018 9:23 pm

The concepts of Q and K are the same the variable changes depending on the context of the question. Q is used when referring to two concentrations that are not at equilibrium and can be utilizded at any point of the reaction. Whereas K is used when referring to concentrations at equilibrium. Q can be compared to K when determining which way the reaction is favoring. I believe if Q> K the reaction favors the reactants and if Q<K the reaction favors the products. If Q=K then the reaction is at equilibrium because the ratio is the same.

Veronica Rasmusen 2B
Posts: 49
Joined: Sat Jul 22, 2017 3:01 am

Re: Q and K

Postby Veronica Rasmusen 2B » Mon Feb 26, 2018 10:37 pm

Q and K are usually associated with equilibrium therefore the concepts regarding K>1 (products are favored) or Q>K (reactants are favored) or Q<K (products favored) are also constant

Sophia Bozone 2G
Posts: 51
Joined: Fri Sep 29, 2017 7:07 am

Re: Q and K

Postby Sophia Bozone 2G » Mon Feb 26, 2018 10:46 pm

Q and K are the same in this context as in equilibrium, so the ideas around K>1 (products are favored), Q>K (reactants are favored), Q<K (products favored) are the same


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