Gaseous Equilibria Changes

[905934067]

Can someone explain how Le Chatelier's Principle applies to changes in pressure for gaseous equilibria? And how would this affect both homogeneous and heterogeneous reactions? Thanks!

[Kyle_Phong_2J]

When pressure is increased, the system favors the side with fewer moles and vice versa. In heterogenous reactions, we would ignore reactants and products that are in the solid and liquid states.

[805777063]

Hi! You have to be careful with this, for example, adding more water as a liquid solvent would not affect the reaction. Make sure to identify what reactants and products are actually involved in the reaction and THEN apply Le Chatelier. When it comes to pressures, it is basically the same as applying Le Chatelier to concentrations. You can think of increasing the pressure of a reactant or product as "increasing its amount"

[Brian Cho 3E]

To add on, it is also important to keep in mind that the values for pressure and volume are not proportionate so if the system is compressed or the volume is decreased, then the pressure is increased, shifting to the side with less moles and vice versa.