Module Part 2 Question

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taywebb
Posts: 60
Joined: Fri Sep 28, 2018 12:15 am

Module Part 2 Question

Postby taywebb » Sun Jan 13, 2019 3:00 pm

Can anyone explain what I am doing wrong on this question:
29. A researcher fills a 1.00 L reaction vessel with 1.84 x 10-4 mol of BrCl gas and heats it to 500 K. At equilibrium, only 18.3 % of the BrCl gas remains. Calculate the equilibrium constant, assuming the following reaction is taking place.
2BrCl(g) ⇌ Br2 (g) + Cl2(g)

I created my ICE table and get my x to be 7.52x10^-5, but for some reason, I keep getting a Kc that is not one of the answer choices. I am solving Kc = [7.52x10^-5][7.52x10^-5]/[3.36x10^-5]^2 and I keep getting 6.

Lexie Baughman 2C
Posts: 30
Joined: Sat Oct 06, 2018 12:16 am

Re: Module Part 2 Question

Postby Lexie Baughman 2C » Sun Jan 13, 2019 3:09 pm

I set up my ICE table the same way you did and got the same values for the equilibrium constant equation, but when I plugged it into my calculator, I got 4.983. Is that an option? Maybe it was just a mistake in entering the values into the calculator.

LorenzoDuvergne3I
Posts: 60
Joined: Fri Sep 28, 2018 12:25 am

Re: Module Part 2 Question

Postby LorenzoDuvergne3I » Sun Jan 13, 2019 3:20 pm

I also got about 5. I think it is because of a misplaced parentheses between the first and second reactants since your number is higher than what it should be. Make sure it is
(7.516E-5)^2/
(3.3672E-5)^2


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