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Posted: Sun Jan 12, 2020 2:07 pm
by Alicia Lin 2F
State whether reactants or products will be favored by an increase in the total pressure (resulting from compression) on each of the following equilibria. If there is no change, explain why that is so.
d. 2HD(g)+H2(g)⇌D2(g)

The answer is no change. I would expect the products to be favored since there are less moles of gas. Can anyone explain this to me?

Re: 5J:1d

Posted: Sun Jan 12, 2020 2:12 pm
by Sanjana Borle 2K
As we learned in class, change in pressure generally does not change state of equlibrium.

Re: 5J:1d

Posted: Sun Jan 12, 2020 2:19 pm
by JonathanS 1H
Because it is an increase in pressure by compression, the moles of each gas does not change, but the volume does. The reaction shifts right for a little bit, but the overall K value does not change.