5J #5 part d

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Bailey Giovanoli 1L
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Joined: Wed Sep 30, 2020 9:50 pm

5J #5 part d

Postby Bailey Giovanoli 1L » Thu Jan 07, 2021 10:14 pm

In question 5 of section 5J it asks you to identify whether products or reactants are favored if total pressure is increased. From what I gathered with Le Chatelier’s principle, if total pressure is increased, the side of the reaction with less moles will be favored. I think this is because if there are more moles on one side and pressure is increased the interaction between those molecules will increase due to less space to more freely. However, I am confused because part d gives the following reaction:
2HD (g) + H2-><- D2
I’m first concerned as to how the Hydrogens completely disappeared from the reaction on the product side. I wasn’t told to, but do I need to add them in and balance the equation? If I were to add the Hydrogens to The products, I would have 2 moles of H2, right? Because if I did it that would balance the equation and make the number of moles the same, justifying the answer.
If that is not the case, then I am confused as to why neither would be favored when there are 3 moles of reactant and only one mole of product.

Shanna Yu 1C
Posts: 101
Joined: Wed Sep 30, 2020 9:36 pm
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Re: 5J #5 part d

Postby Shanna Yu 1C » Thu Jan 07, 2021 11:29 pm

Hi!

The thing you pointed out in part D is actually a typo; the H2 should be on the right side, alongside the D2. Your proposed alternative explanation is correct in that having H2 on the other side would justify the given answer!

Asia Yamada 2B
Posts: 93
Joined: Wed Sep 30, 2020 9:36 pm

Re: 5J #5 part d

Postby Asia Yamada 2B » Mon Jan 25, 2021 12:53 pm

That’s a typo! You can refer to the correct chemical equation here: https://lavelle.chem.ucla.edu/wp-conten ... rs_7Ed.pdf


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