Le Chatelier

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Tom Notcovich 3B
Posts: 13
Joined: Wed Sep 21, 2016 2:58 pm

Le Chatelier

Postby Tom Notcovich 3B » Thu Dec 01, 2016 9:58 am

Is there a way to describe Le Chaterlier in terms of proportionality on either side of the arrow?

Alexander Chen 3N
Posts: 36
Joined: Fri Jul 22, 2016 3:00 am
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Re: Le Chatelier

Postby Alexander Chen 3N » Thu Dec 01, 2016 11:12 am

That would be the equilibrium constant. For example, if and you add more B, then A would increase and B would decrease until you reach the equilibrium constant.

Greta Tobin 2F
Posts: 15
Joined: Wed Sep 21, 2016 2:57 pm

Re: Le Chatelier

Postby Greta Tobin 2F » Thu Dec 01, 2016 12:11 pm

Is there an easy way to remember how a change in pressure would effect the equilibrium? I am looking at the "quick way" in the course reader but still a little confused. Can someone explain in their own words?

Thanks!

YuniLee_1K
Posts: 23
Joined: Wed Sep 21, 2016 2:59 pm

Re: Le Chatelier

Postby YuniLee_1K » Fri Dec 02, 2016 1:00 am

An increase in pressure occurs when you decrease volume (smaller container = particles bounce off walls more often and thus create more pressure inside).

When volume decreases, the reaction will want to shift in a way to maintain equilibrium (i.e. make the moles of reactants roughly = moles of products). If more moles are on the left side (reactants), then the reaction moves to the right to even out the number of moles. If more moles are on the right side (products) then the reaction will move to the left.


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