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Posted: Sun Jan 12, 2020 10:30 pm
by Karina Kong 2H
A sample of ozone, O3, amounting to .10 mol, is placed in a sealed container of volume 1.0 L and the reaction 2 O3(g) --> 3 O2 (g) is allowed to reach equilibrium. Without doing any calculations, predict which of the following will be different in the two containers at equilibrium. Which will be the same?

(a) amount of O2
(b) partial equilibrium of O2
(c) the ratio P O2/ P O3
(d) the ratio (P O2)^3/ (P O3)^2
(e) the ratio (P O3)^2/ (P O2)^3

Re: 5G.9

Posted: Sun Jan 12, 2020 11:18 pm
by alex_4l
Do you want the answers to this or is there some particular part of the problem you don't understand?

Re: 5G.9

Posted: Sun Jan 12, 2020 11:29 pm
by JNie1L
Only D and E will be the same. D and E are the expressions for K in both the forward and reverse reactions. K is always constant at a certain temperature, so those values will stay constant. A, B, and C are all dependent on the amount of moles or specific partial pressures and will differ between the two containers.

Re: 5G.9

Posted: Sun Jan 12, 2020 11:34 pm
by Ashley Nguyen 2L
D and E will remain the same. Both are equation used to find K of the reaction in the forward and reverse direction. This ratio is a fixed constant.