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Effect of increasing pressure on reactions

Posted: Sun Jan 19, 2020 10:10 pm
by 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.

Re: Effect of increasing pressure on reactions

Posted: Sun Jan 19, 2020 10:13 pm
by 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.

Re: Effect of increasing pressure on reactions

Posted: Sun Jan 19, 2020 10:32 pm
by 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.

Re: Effect of increasing pressure on reactions

Posted: Sun Jan 19, 2020 10:35 pm
by 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.

Re: Effect of increasing pressure on reactions

Posted: Sun Jan 19, 2020 10:40 pm
by SimranSangha4I
The reaction would end up shifting towards the side in which there are fewer mole because that would effect the equilibrium!

Re: Effect of increasing pressure on reactions

Posted: Sun Jan 19, 2020 10:45 pm
by 005162520
Why isn't when you add inert gas, the concentrations and the equilibrium do not change ?

Re: Effect of increasing pressure on reactions

Posted: Sun Jan 19, 2020 11:27 pm
by 205154661_Dis2J
The reaction would shift towards the side with fewer moles!