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Equilibrium and Gases

Posted: Mon Jan 06, 2020 9:49 pm
by alicechien_4F
Why does the equilibrium shift to the side with less moles of gas when pressure is increased?

Re: Equilibrium and Gases

Posted: Mon Jan 06, 2020 10:20 pm
by Charisse Vu 1H
When pressure is increased by decreasing the volume, equilibrium shifts to to the side with less moles of gas because the concentrations of each compound is being increased according to the equation P=n/v. If pressure is increased by decreasing the volume, then the concentration increases since v is a smaller number. Therefore, equilibrium will shift to the side with less moles of gas.

Re: Equilibrium and Gases

Posted: Tue Jan 07, 2020 11:34 am
by Rida Ismail 2E
I remembered that when the pressure was increased it moved to the side with fewer moles because if there is more pressure, the gas wants more area to spread out. If there are fewer moles with more pressure the moles of gas are not as cramped.

Re: Equilibrium and Gases

Posted: Thu Jan 09, 2020 7:36 pm
by Ryan Yee 1J
When pressure is increased it forces gas molecules closer together, so if the gas atoms can form more complex molecules to take up less space (for more movement) then they can.