Calculating concentrations at equilibrium

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Philip
Posts: 100
Joined: Sat Sep 07, 2019 12:16 am

Calculating concentrations at equilibrium

Postby Philip » Mon Mar 09, 2020 4:57 pm

One mole of COBr2 was injected in a 1L flask at a certain temperature. The equilibrium mixture was then analyzed and found to contain 0.304 moles of CO.
Calculate the concentration of each species at equilibrium.

chemboi
Posts: 101
Joined: Sat Jul 20, 2019 12:16 am

Re: Calculating concentrations at equilibrium

Postby chemboi » Mon Mar 09, 2020 9:40 pm

Are you asking how to set this up? If the reaction is COBr2 -> CO + Br2, then it's an ICE table setup.

WGaines_2E
Posts: 47
Joined: Mon Nov 18, 2019 12:18 am

Re: Calculating concentrations at equilibrium

Postby WGaines_2E » Tue Mar 10, 2020 9:25 pm

so the reaction looks like its gonna be COBr2 <> CO(g) + Br2(g)
you have the final concentration of CO
solve using ICE table

kennedyp
Posts: 56
Joined: Tue Nov 13, 2018 12:18 am

Re: Calculating concentrations at equilibrium

Postby kennedyp » Sat Mar 14, 2020 9:50 pm

WGaines_2E wrote:so the reaction looks like its gonna be COBr2 <> CO(g) + Br2(g)
you have the final concentration of CO
solve using ICE table

I figured it was an ice table question, but how would we solve if we weren't given K? Unless the og poster accidentally left K out?

Frank He 4G
Posts: 50
Joined: Tue Nov 12, 2019 12:19 am

Re: Calculating concentrations at equilibrium

Postby Frank He 4G » Sat Mar 14, 2020 10:10 pm

kennedyp wrote:
WGaines_2E wrote:so the reaction looks like its gonna be COBr2 <> CO(g) + Br2(g)
you have the final concentration of CO
solve using ICE table

I figured it was an ice table question, but how would we solve if we weren't given K? Unless the og poster accidentally left K out?


Well do we? I could be wrong about this, but if we know that we started with 1 mole of COBr2 and at the end we had 0.304 mol of CO, then following the stoichiometry of the equation, we also have 0.304 mol of Br2, and 1-0.304 mol of COBr2.


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