5J.1

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Chloe Alviz 1E
Posts: 102
Joined: Sat Aug 17, 2019 12:17 am

5J.1

Postby Chloe Alviz 1E » Sun Jan 19, 2020 5:18 pm

I have a question on one part of this question:

Consider the equilibrium CO(g) + H2O(g) <--> CO2(g) + H2(g).

b) If the partial pressure of CO is decreased, what happens to the partial pressure of CO2?

Why would the partial pressure of CO2 decrease if the moles of gas on each side are equal?

Eugene Chung 3F
Posts: 142
Joined: Wed Nov 15, 2017 3:03 am

Re: 5J.1

Postby Eugene Chung 3F » Sun Jan 19, 2020 5:24 pm

Le Chatelier's principle tells us that chemical reactions adjust to minimize the effect of changes. Therefore, if CO (reactant) partial pressure increases, the reaction will want to minimize the effect of that change and shift left to produce more CO (kinda like compensating). The result of that is reduced partial pressure of CO2.

AniP_2D
Posts: 95
Joined: Sat Aug 17, 2019 12:17 am

Re: 5J.1

Postby AniP_2D » Sun Jan 19, 2020 8:56 pm

The reason why CO2 would decrease when CO decreases is because, according to Le Chatelier's principle, the system will shift to the left of the reaction in order to provide a balance, meaning that CO2 will decrease in order to contribute to this balance.

CalvinTNguyen2D
Posts: 102
Joined: Thu Jul 25, 2019 12:16 am

Re: 5J.1

Postby CalvinTNguyen2D » Sun Jan 19, 2020 9:19 pm

In order to balance the equilibrium, as the partial pressure of CO is decreased, the partial pressure of CO2 must decrease as well and will shift to the left.

Owen-Koetters-4I
Posts: 50
Joined: Fri Sep 28, 2018 12:16 am

Re: 5J.1

Postby Owen-Koetters-4I » Sun Jan 19, 2020 10:35 pm

The partial pressure of a reactant is decreased in this system in dynamic equilibrium. Therefore Q temporarily rises above K and the reactants are favored until Q=K. In this example this means the partial pressure of CO2 decreases until equilibrium is met.


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