Pressure affects only gas reactions?

[Kelly Yun 2I]

Hi! I feel like the change in pressure should only have an affect on reactions where the moles of gases on either side are different, but would that also apply to reactions where the moles of gases are equal on both sides but one side has more moles of a substance in a different phase? I don't know if this question makes sense but I hope someone can answer this haha

[Leo Naylor 2F]

Pressure does not really affect liquids or solids because liquids and solids are essentially incompressible. So the answer to your question is no, a change in pressure will not affect a reaction as long as the reaction has the same number of moles of gas on both sides.

[Karl Yost 1L]

Changing pressure only affects gas reactions, as only gases can be compressed. We just say that the compression of solids and liquids is negligible.

[Kelly Yun 2I]

Ohh I see. Thank you!

[Kyle Walsh 2J]

I believe that it's not the pressure that affects gas reactions, it's the volume changing. But the pressure change is just a byproduct of the changing volume.

[SophiaNguyen_2L]

I just want to emphasize what the person above me is saying ^^! If pressure changes due to the addition of an inert gas (like helium or xenon gas), then Le Chatalier's principle wouldn't be applicable and the system's equilibrium won't change.

[Aarushi Verma 2I]

If there is an equal amount of moles on both sides, then any pressure changes won't affect the reaction because pressure only affects gases, not liquids and solids.

[Shreyank Kadadi 3K]

Yes, only gases are affected by changes in pressure due to the incompressibility of the other phases.

[Armen_Isayan_2L]

Hello! It is evident that pressure does not tka significant effect upon liquids or solids. This is mainly because of the fact that pressure tends to effect only gases, and not liquids and solids, hence a change in pressure will to affect a reaction, in the case that a reaction contains the exact similar number of moles on both sides.

[haley f]

You are correct! When pressure increases the reaction will favor the side with fewer moles of gas because solids and liquids won't change their volume when pressure is increased or decreased because it is very hard to do so.

[Ansh Patel 2I]

Hi! Gases are the only phase that are affected my pressure because it is able to be compressed, unlike other phases.

[Kelly Tran 1J]

Hi! Changes in pressure (by changing the volume) only affects gases since gases are compressible. If the pressure increases (decreasing the volume), the equilibrium would shift to the side with less amount of moles of gas, but if there are equal moles of gases on both sides of the reaction, the equilibrium will not shift.

[Joshua_Chan_3K]

Remember what he said in lecture. Pressure doesn't necessarily affect anything (ie. a n inert gas is added). Volume is what changes. If you look at concentration, volume will obviously change the concentration of a gas. If concentration changes, the reaction quotient will shift.

[Sonel Raj 3I]

A change in pressure aka a change in volume only affects gases- solids and liquids are not affected by changes in pressure. You see this when you look at the ideal gas law equation; changing the pressure affects the concentration of the gas, which therefore affects equilibrium.

[Geethika Janga 1L]

Yes technically pressure on affects gas reactions because compounds can only be compressed in their gaseous state

[Earl Garrovillo 2L]

Yup, since solids and liquids basically don't change concentration ever, while concentrations of aqueous things only change when solvent or solute is added, pressure will only affect the gases. Gases fill up the container they're in so if they're compressed, their concentrations change. If there's equal amounts of gas on each side, regardless of the states of other reactants/products, these gases change concentration by the same factor and there's no change in equilibrium when pressure is changed.

[AlbertGu_2C]

Only gases can be compressed, so you only count the gaseous state of the element in question.

[Jack_Pearce_2H]

Pressure does not really affect liquids or solids much, so shifts in equilibrium based on the pressure of a container would only apply to gasses.

[Constance Newell]

I believe it only effects gasses..... I could be wrong but I don't think it effects inert gasses tho.

[Aditya Sundaram 3D]

Since we use partial pressures for reactions with gasses, changing pressure would definitely impact that. But when we are using concentrations of liquids and solids, not much really changes.

[Massimo_Capozza_1G]

It only affects the gas reaction. Solid and liquids aren't really affected because their volume is independent of pressure, I think.

[Aditya Sundaram 3D]

It only affects the gas reaction. Solid and liquids aren't really affected because their volume is independent of pressure, I think.

Yeah, these were my thoughts exactly. Concentration is relative and not based on pressure like gasses are.

[Ashley Wagner 2A]

Yes pressure only affect gas reactions. Liquid and solids are incompressible and values are independent of pressure

[Sejal Parsi 3K]

A change in pressure (a change in volume) only affects gases. Solids and liquids are not affected because they are essentially incompressible.