Effect of increasing pressure on reactions

[JesseAuLec1Dis1G]

Can someone explain to me what happens if you increase pressure on a reaction? Increasing pressure decreases volume so wouldn't products be favored? From my notes I have that increasing pressure doesn't favor products or reactants.

[Deepika Reddy 1A]

If the pressure is increased, then the reaction favors the side of the reaction that has fewer moles of gas. In class, he gave us C=n/V and said that the change in concentration caused by the change in volume is what affects the reaction.

[Ashley Wang 4G]

I think the situation your notes are referring to is when you pump an inert gas into a vessel of fixed volume. Because the concentrations of the reactants and products don't change in this case, neither the forward nor the reverse reaction are favored.
In the case where you change the pressure via a change in volume (compression or expansion), the system will response in the way described by the previous comment.

[Anushka Chauhan2B]

If the pressure is increased, equilibrium is disrupted. As a result, the reaction would shift to the side with the fewest number of moles.

[SimranSangha4I]

The reaction would end up shifting towards the side in which there are fewer mole because that would effect the equilibrium!

[005162520]

Why isn't when you add inert gas, the concentrations and the equilibrium do not change ?

[205154661_Dis2J]

The reaction would shift towards the side with fewer moles!