Pressure and Volume

[Haley Dveirin 1E]

do changes in pressure and volume affect K? if not, why not? if it does, how does it affect it?

[Sarah Zhari 1D]

Changing the pressure of a container by decreasing or increasing its volume does not affect K. This is because the partial pressures of all the gases involved in calculating K change by a common factor when a gas is compressed or otherwise, therefore the overall ratio of products to reactants remains the same.

[Jessica Esparza 2H]

It does not affect K. I believe it can affect the concentration of products and reactants but not the ratio between them.

[aishwarya_atmakuri]

The value of K would depend on whether pressure would change from a change in volume (would change) or addition of an inert gas (no change) based on how concentration would change.

[Katie Kyan 2K]

Changes in pressure do not affect K as Dr. Lavelle mentioned in class. Adding an inert gas to increase pressure does not affect the moles of the reactant or product and the volume remains constant. Similarly, changes in volume also do not affect K as the system will try to restore equilibrium through Le Chatelier's Principle.

[Hannah Pham]

Changes in pressure and volume do not affect value of the equilibrium constant.

[Kylie Lim 4G]

Equilibrium constant for a single reaction is affected by temperature changes, not pressure

[Ellen Amico 2L]

Changes in pressure or volume cause changes in concentration (due to PV=nRT), and changes in concentration don't affect K due to Le Chatelier's Principle, so that's why pressure and volume don't affect K, only temperature.

[Anna Heckler 2C]

Changing the pressure does not affect K, as K is a constant and all of the pressures would change by the same factor. Temperature DOES change K.