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Chemistry Forums for Students => High School Chemistry Forum => Topic started by: sparkly on March 23, 2009, 11:18:58 AM

Title: How to calculate Kp
Post by: sparkly on March 23, 2009, 11:18:58 AM
The only way the book showed to do equilibrium is to do Keq = [A]^a [ B]^b / [C]^c
but that isnt even possible here. When I asked the teacher, he said I should be able to do this with some basic Algebra I. I am completely lost. Please help

 Consider the equilibrium

N2(g) + O2(g) + Br2(g) <===> 2 NOBr(g)

Calculate the equilibrium constant Kp for this reaction, given the following information (at 298 K):

2 NO(g) + Br2(g) <===> 2 NOBr(g) Kp = 0.49

2 NO(g) <===> N2(g) + O2(g) Kp = 2.1 x 1030
Title: Re: How to calculate Kp
Post by: sjb on March 23, 2009, 12:43:22 PM
Note that [ B ] (without the spaces) is a formatting code for bold text, but that's a software issue.

Consider your first equilibrium, what is your expression for Keq, and then similarly with the partial equilibriums you list later?
Title: Re: How to calculate Kp
Post by: Las on March 24, 2009, 07:52:12 AM
are you sure there's enough information here to do this question? :(
Title: Re: How to calculate Kp
Post by: sjb on March 24, 2009, 07:57:14 AM
Quote from: Las on March 24, 2009, 07:52:12 AM
are you sure there's enough information here to do this question? :(

Yes!

What's the expression for Kp for the reaction 2 NO(g) + Br2(g)  ::equil:: 2 NOBr(g) ?

Repeat for the other reactions, and see where that gets you.
Title: Re: How to calculate Kp
Post by: Las on March 24, 2009, 08:09:22 AM
LOL..I got it:) that's one funny question :P All you have to know is how to write the expressions for Kp:)