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Chris Tai 1B
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Joined: Sat Aug 24, 2019 12:16 am


Postby Chris Tai 1B » Fri Jan 17, 2020 4:19 pm

Dissociation of a diatomic molecule, X2(g) <-> 2 X(g) occurs at 500 K. The equilibrium state of the reaction is shown in 1 and the equilibrium state in the same container after a change has occurred is shown in 2. Which of the following changes will produce the composition shown? (a) Increasing the temperature. (b) Adding X atoms. (c) Decreasing the volume. (d) Adding a catalyst. Explain your selections.

It makes sense to me why increasing the temperature would result in the change shown in the diagram, but why wouldn't adding X atoms or adding a catalyst also result in the same change in container 2?

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Joined: Wed Feb 20, 2019 12:18 am

Re: 5.33

Postby CameronDis2K » Fri Jan 17, 2020 4:24 pm

I believe because its the same ideology like adding an extra compound or atom that's different/not in the original equilibrium equation, will not change the K value or the reaction process. No shift occurs and it will be like the original equilibrium conditions.

Posts: 50
Joined: Sat Aug 24, 2019 12:16 am

Re: 5.33

Postby 705302428 » Fri Jan 17, 2020 6:42 pm

I believe Dr. Lavelle said that a catalyst only pertains to how quickly the reaction happens. It doesn't have anything to do with the actual components of the reaction.

Edmund Zhi 2B
Posts: 118
Joined: Sat Jul 20, 2019 12:16 am

Re: 5.33

Postby Edmund Zhi 2B » Sat Jan 18, 2020 1:54 pm

Adding X atoms would cause more reactants to form to relieve stress on the equilibrium from an increase in products, but in the image there are actually less X2 molecules in container 2, so that answer is incorrect.

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