the "quick way"

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Emily Orozco L4
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Joined: Fri Sep 28, 2018 12:29 am

the "quick way"

Postby Emily Orozco L4 » Sun Jan 12, 2020 5:21 pm

Could someone explain the "quick way" Dr. Lavelle described in lecture when talking about changes in pressure? What are the circumstances in which it can be used?

Jacob Puchalski 1G
Posts: 97
Joined: Fri Aug 09, 2019 12:16 am

Re: the "quick way"

Postby Jacob Puchalski 1G » Sun Jan 12, 2020 5:26 pm

I think what you're talking about is whether the reaction shifts left or right? If the volume decreases and more moles of gas are added to the reactants, then the reaction shifts right. If the volume decreases and more moles of gas are added to the products, then the reaction shifts left.

Aarushi Solanki 4F
Posts: 107
Joined: Sat Jul 20, 2019 12:17 am

Re: the "quick way"

Postby Aarushi Solanki 4F » Sun Jan 12, 2020 5:30 pm

The quick way you're referring to has to do with changes in pressure. The basic rule is that when pressure increases (volume decreased), the reaction will want to shift to the side (reactant vs. product) with less total moles. When pressure decreases (volume increased), the reaction will shift to the side with more moles.

405268063
Posts: 102
Joined: Thu Jul 25, 2019 12:17 am

Re: the "quick way"

Postby 405268063 » Sun Jan 12, 2020 6:06 pm

I like to think of the "quick way" Dr. Lavelle referred to in class as just a balancing act. If there's more pressure on one side, the reaction will want to go to the other, if that makes sense.

William Chan 1D
Posts: 102
Joined: Sat Sep 14, 2019 12:15 am

Re: the "quick way"

Postby William Chan 1D » Sun Jan 12, 2020 6:27 pm

The "quick" way refers to looking at the moles of gas on each side of the equation, and when pressure changes, let's say increased, then the reaction will shift toward the side with fewer moles of gas because it "relieves" some of the pressure.


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