Do I use an ICE box?

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Emma Edmond 3E
Posts: 29
Joined: Fri Sep 25, 2015 3:00 am

Do I use an ICE box?

Postby Emma Edmond 3E » Tue Nov 17, 2015 5:36 pm

For this problem, would I begin by setting up an ice box or can I just set up a proportion?

Consider the following reaction at 1200 K, for which you know Kc = 1.7 x 10-3.
Br2 (g) ⇌ 2 Br (g)
Your experimental setup is able to measure the equilibrium concentration of Br2 based on its color, but you are unable to measure the concentration of Br directly. If you measure at equilibrium [Br2] to be 1.02 x 10-4 M, calculate the equilibrium concentration of Br for this experiment.

Amanda Reshke 1D
Posts: 17
Joined: Fri Sep 25, 2015 3:00 am

Re: Do I use an ICE box?

Postby Amanda Reshke 1D » Tue Nov 17, 2015 6:20 pm

I might be wrong, but you can probably just set the K equal to [products]/[reactants] and solve for Br (the product) (?)

JasmineAlberto4J
Posts: 73
Joined: Fri Sep 25, 2015 3:00 am

Re: Do I use an ICE box?

Postby JasmineAlberto4J » Tue Nov 17, 2015 9:47 pm

Amanda Reshke 1E wrote:I might be wrong, but you can probably just set the K equal to [products]/[reactants] and solve for Br (the product) (?)

I agree. if you set up K= [R]/[P] you are given K and are given R solve for P

Chem_Mod
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Re: Do I use an ICE box?

Postby Chem_Mod » Wed Nov 18, 2015 3:00 am

Jasmine and Amanda are correct, you do not need to use an ICE box since you already know one of the equilibrium concentrations as well as the equilibrium constant.

tiffanyteguh1C
Posts: 20
Joined: Fri Sep 29, 2017 7:04 am

Re: Do I use an ICE box?

Postby tiffanyteguh1C » Tue Nov 28, 2017 6:06 am

For this question, do we have to divide by the coefficient of Br, 2?


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