partial pressures


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Savannah Mance 4G
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Joined: Fri Aug 30, 2019 12:17 am

partial pressures

Postby Savannah Mance 4G » Sun Jan 12, 2020 6:29 pm

In 5G.9 it says in two containers, one with 0.1 mol of O3 and the other with 0.5 mol of O3 with the rxn 2O3(g)<--->3O2(g) taking place will ratio of PO2/PO3 be the same (part b). I understand that the ratio won't be the same for the two containers because the partial pressures of the O3 as well as the O2 won't be the same in the two containers. But the next part asks if the ratio (PO2)^3/(PO2)^2 will be the same and the answer is yes but I don't understand why. Can someone please explain why?

KSong_1J
Posts: 101
Joined: Thu Jul 11, 2019 12:17 am

Re: partial pressures

Postby KSong_1J » Sun Jan 12, 2020 6:38 pm

The ratio will be the same because (PO2)^3/(PO3)^2 is the formula for its equilibrium constant, K, which always stays the same whether more moles are added or not

205007651
Posts: 53
Joined: Tue Nov 13, 2018 12:17 am

Re: partial pressures

Postby 205007651 » Sun Jan 12, 2020 6:53 pm

Just to add on to the previous reply, the only reason k will change will be because of a change in temperature.

Alondra
Posts: 36
Joined: Tue Feb 26, 2019 12:15 am

Re: partial pressures

Postby Alondra » Sun Jan 12, 2020 8:19 pm

K is a constant. I believe a change in pressure does not affect K but a change in temperature can.

RasikaObla_4I
Posts: 100
Joined: Thu Jul 25, 2019 12:15 am

Re: partial pressures

Postby RasikaObla_4I » Sun Jan 12, 2020 8:38 pm

The ratio (PO2)^3/(PO3)^2 represents the equilibrium constant K so it stays the same. As a result changing the concentrations of the products and reactants would not change the constant.

kevinolvera1j
Posts: 103
Joined: Fri Aug 02, 2019 12:15 am

Re: partial pressures

Postby kevinolvera1j » Sun Jan 12, 2020 10:02 pm

A change to concentrations does not change the equilibrium constant. That is why K remains the same even when concentrations increase or decrease. What should be noted is that K is only for reactions at equilibrium, what that means is that if you add or take away products or reactants and therefore change the concentrations, you will have to wait for the system to reach equilibrium again.

Shrayes Raman
Posts: 129
Joined: Sat Jul 20, 2019 12:15 am

Re: partial pressures

Postby Shrayes Raman » Sun Jan 12, 2020 11:50 pm

The second part ratio represents K and K will be the same regardless of quantity

Eunice Nguyen 4I
Posts: 100
Joined: Sat Aug 17, 2019 12:17 am

Re: partial pressures

Postby Eunice Nguyen 4I » Mon Jan 13, 2020 1:13 am

The ratio represented the equilibrium constant K, so it'll remain the same.


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