Le Chatelier

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Brian_Ho_2B
Posts: 221
Joined: Fri Aug 09, 2019 12:16 am

Le Chatelier

Postby Brian_Ho_2B » Mon Jan 13, 2020 4:02 pm

In class, we've gone over how changes to pressure and to concentration may shift the direction of the reaction and how changing the temperature actually changes the equilibrium constant of a certain reaction. Is there possibly another way to change the value of K? Is there another parameter not discussed in class or in the PV=nRT equation?

McKenna_4A
Posts: 115
Joined: Sat Aug 24, 2019 12:18 am

Re: Le Chatelier

Postby McKenna_4A » Mon Jan 13, 2020 4:05 pm

Increasing the total pressure of the system will cause equilibrium to shift to the side with fewer moles

Dina Marchenko 2J
Posts: 54
Joined: Thu Jul 25, 2019 12:16 am

Re: Le Chatelier

Postby Dina Marchenko 2J » Mon Jan 13, 2020 6:53 pm

The value of K itself will not be changed by anything except temperature. Other parameters such as pressure or concentration will cause the position of equilibrium to change but not the value of the equilibrium constant for that chemical equation for that temperature.

Qiu Ya Wu 4I
Posts: 107
Joined: Fri Sep 20, 2019 12:17 am

Re: Le Chatelier

Postby Qiu Ya Wu 4I » Mon Jan 13, 2020 6:58 pm

McKenna_4A wrote:Increasing the total pressure of the system will cause equilibrium to shift to the side with fewer moles


Changing the pressure of a system will not change the equilibrium constant k itself, but it will cause a net increase in the equilibrium concentration of the side of a reaction with less moles due to the change in concentration that occurs as a result of the change in volume.


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