question 5i.19

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Athena L 1B
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Joined: Fri Sep 28, 2018 12:18 am

question 5i.19

Postby Athena L 1B » Thu Jan 24, 2019 10:08 pm

Can someone explain this question?
A reaction mixture that consisted of 0.400 mol H2 and 1.60 mol I2 was introduced into a flask of volume 3.00 L and heated. At equilibrium, 60% of the hydrogen gas had reacted. What is the equilibrium constant K for the reaction H2(g) + I2(g) <=> 2HI(g) at this temp?

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Re: question 5i.19

Postby Chem_Mod » Thu Jan 24, 2019 10:16 pm

Set up an ice table and the change is given (60% is reacted) you can find the equilibrium concentration for all the gas and calculate K

Ethan Breaux 2F
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Re: question 5i.19

Postby Ethan Breaux 2F » Fri Jan 25, 2019 3:13 pm

Don't forget to use c = n/V and that at equilibrium 40% of hydrogen is left.

Cade Okohira 4K
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Joined: Fri Sep 28, 2018 12:15 am

Re: question 5i.19

Postby Cade Okohira 4K » Sun Jan 27, 2019 12:14 am

First, you would need to convert the mol amounts into molarity, or mol/L by dividing the mol amounts by the amount of L, which is 3 L. Then, you can create an ICE table, knowing that 60% of the H2 had converted into product. Then, you can find Kc by calculating [HI]^2/[H2][I2].

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