Partial Pressure

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Leslie Almaraz 4G
Posts: 99
Joined: Fri Aug 02, 2019 12:16 am

Partial Pressure

Postby Leslie Almaraz 4G » Thu Jan 23, 2020 11:53 pm

Does increasing the partial pressure of one element, affect the partial pressure of another? Or does this only apply when increasing the overall pressure?

Jacey Yang 1F
Posts: 101
Joined: Fri Aug 09, 2019 12:17 am

Re: Partial Pressure

Postby Jacey Yang 1F » Fri Jan 24, 2020 12:35 am

Increasing the partial pressure of one element causes an increase in partial pressure on the other side of the reaction in order to minimize the effect of the change. This also applies when increasing the overall pressure, where the equilibrium shifts in the direction that decreases the number of molecules and lowers the pressure.

Eugene Chung 3F
Posts: 142
Joined: Wed Nov 15, 2017 3:03 am

Re: Partial Pressure

Postby Eugene Chung 3F » Fri Jan 24, 2020 3:23 am

If partial pressure of reactant is increased, then, the reaction will favor products to make up for the change and vice versa.
If overall pressure is increased, meaning that the volume decreased, the side with less gases will be favored (check the stoichiometric coefficients of the gases) and vice versa.

Jocelyn Thorp 1A
Posts: 103
Joined: Wed Sep 18, 2019 12:20 am

Re: Partial Pressure

Postby Jocelyn Thorp 1A » Fri Jan 24, 2020 1:37 pm

changing the pressure will cause the reaction to shift to minimize the change, as per le chatlier's principle

HuyHa_2H
Posts: 100
Joined: Wed Sep 11, 2019 12:15 am

Re: Partial Pressure

Postby HuyHa_2H » Sat Jan 25, 2020 2:34 am

Increasing the partial pressure of something from one side causes the partial pressure of whatever else is on that same side to decrease and everything on the opposite side increases, and vice versa to maintain the proper ratio.

Rodrigo2J
Posts: 102
Joined: Sat Jul 20, 2019 12:16 am

Re: Partial Pressure

Postby Rodrigo2J » Sat Jan 25, 2020 10:26 am

Partial pressure works similarly to the way that concentrations do in le chatelier's principle. For example, if you increase the partial pressure of a reactant, the equilibrium will shift towards the products. Likewise if you decrease the partial pressure of a reactant, the equilibrium will shift towards reactants.


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