Hw 5I.1

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Amy Luu 2G
Posts: 105
Joined: Wed Sep 18, 2019 12:19 am

Hw 5I.1

Postby Amy Luu 2G » Fri Jan 10, 2020 10:53 pm

At 500. K, the equilibrium constant for the reaction Cl2(g) + Br2(g) 2 BrCl(g) is Kc 5 0.031. If the equilibrium
composition is 0.495 mol/L Cl2 and 0.145 mol/L BrCl, what is the equilibrium molar concentration of Br2?
I am unsure how to solve this problem. Do I create the equilibrium table?

Fiona Latifi 1A
Posts: 102
Joined: Sat Sep 14, 2019 12:16 am

Re: Hw 5I.1

Postby Fiona Latifi 1A » Sat Jan 11, 2020 9:41 am

No, you do not create an ICE table. You simply set K equal to (BrCl)^2/((Cl2)*(Br2)) and solve for the equilibrium concentration of Br2. This question just involves some simple algebra.

Hui Qiao Wu 1I
Posts: 56
Joined: Fri Aug 30, 2019 12:16 am

Re: Hw 5I.1

Postby Hui Qiao Wu 1I » Sat Jan 11, 2020 9:57 am

Technically, you can use the ICE table for this problem, but it will take more time and work. ICE tables provides other information like the change in concentrations due to the process of the reaction.

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Re: Hw 5I.1

Postby ayushibanerjee06 » Sat Jan 11, 2020 1:37 pm

You do not have to create an ice table. I find that if they give you the equilibrium concentrations of the product(s) and all of the reactants except for the one they are asking about and vice versa, you should set up K and solve for the concentration for you are trying to find.

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Re: Hw 5I.1

Postby JChen_2I » Sat Jan 11, 2020 9:37 pm

For this problem, you can just set the given K value equal to [products]/[reactants] and solve for the [Br2]

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