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kfowler_117623
Joined: 16 May 2010
Posts: 3
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 Posted: Tue Jun 08, 2010 9:58 am Post subject: |
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| wallstng1442 wrote: | | I think you have the pressure thing backwards. If you have an increase in pressure, the volume decreases and the system will go to the side with fewer moles in order to equilibrate. |
If pressure is increased the system will shift to decrease the pressure(LCP). So if pressure is increased the system will shift to decrease the number of moles of GAS. Therefore, shifting away from the side of the reaction with the largest number of gaseous moles towards the the side of the reaction with the fewest number of gas molecules. |
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kevnm678961
Joined: 20 Nov 2010
Posts: 1
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| Posted: Sun Nov 21, 2010 11:18 am Post subject: ? |
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| The equilibrium is unaffected by solids but in the video it states an increase in solid introduces stress pushing the equilibrium to the right. Is this a mistake or am i missing something? |
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mcat_premed3832
Joined: 19 Oct 2006
Posts: 429
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| Posted: Sun Nov 21, 2010 4:20 pm Post subject: |
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If you have liquid and gas on both sides of an equilibrium, they are so incredibly more active in chemical reactions compared to solid, then indeed solid is ignored (and in fact left out of equilibrium equations).
However, from Le Chetalier's point of view, the following controlled reaction in a closed vessel of a single substance (not a chemical reaction between different compounds) was presented in the video:
solid <-> liquid + gas
This equilibrium is relevant in the context of Phase Diagrams.
www.chemguide.co.uk/physical/phaseeqia/phasediags.html |
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