Partial Pressures

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Sara Lakamsani 4D
Posts: 61
Joined: Fri Sep 28, 2018 12:29 am

Partial Pressures

Postby Sara Lakamsani 4D » Sat Mar 16, 2019 10:12 pm

When applying Le Chateliers to partial pressures, should we think about it in terms of compressing the entire reaction or changing the amount of a given reactant or product present?

Noah Cook 3O
Posts: 31
Joined: Fri Sep 28, 2018 12:20 am

Re: Partial Pressures

Postby Noah Cook 3O » Sat Mar 16, 2019 10:43 pm

Le Chatelier's principle is generally referring to equilibrium so you should treat it like an amount of a given substance, which is represented by the partial pressure.

Posts: 108
Joined: Sat Jul 20, 2019 12:17 am

Re: Partial Pressures

Postby KBELTRAMI_1E » Wed Jan 08, 2020 8:01 pm

Is anyone able to give a simple, direct description of this concept?

Sydney Myers 4I
Posts: 100
Joined: Fri Aug 09, 2019 12:17 am

Re: Partial Pressures

Postby Sydney Myers 4I » Wed Jan 08, 2020 8:16 pm

When it comes to partial pressures, there are two ways that a system at equilibrium can change.
1) The entire volume of the container is being reduced. This would increase pressure on all of the molecules in the system and it would respond by shifting the equilibrium to whichever side has a smaller number of gas molecules.
2) There is a change in the amount of a certain gas. You would treat this as if the concentration was increased or decreased and the equilibrium should react in the same way.

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