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### Topic: How to calculate Kp  (Read 19592 times)

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#### sparkly

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##### How to calculate Kp
« 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
« Last Edit: March 23, 2009, 01:02:09 PM by Borek »

#### sjb

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##### Re: How to calculate Kp
« Reply #1 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?

#### Las

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##### Re: How to calculate Kp
« Reply #2 on: March 24, 2009, 07:52:12 AM »
are you sure there's enough information here to do this question?

#### sjb

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##### Re: How to calculate Kp
« Reply #3 on: March 24, 2009, 07:57:14 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)  2 NOBr(g) ?

Repeat for the other reactions, and see where that gets you.

#### Las

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##### Re: How to calculate Kp
« Reply #4 on: March 24, 2009, 08:09:22 AM »
LOL..I got it:) that's one funny question All you have to know is how to write the expressions for Kp