K=...? (pg 73 course reader pre-equilibrium ex)

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Zoe Robertson 2H
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Joined: Fri Jun 17, 2016 11:28 am

K=...? (pg 73 course reader pre-equilibrium ex)

Postby Zoe Robertson 2H » Wed Feb 22, 2017 11:23 pm

For the pre-equilibrium example on page 73, the fast step is: NO + NO <==> N2O2. Then K is written as: K=[N2O2]/[NO]^2
I'm confused why N2O2 is in the numerator, because of the formula K1=k1/k1*. Isn't the reverse equilibrium reaction k1*?
I thought it would be flipped. Thanks!

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Joined: Wed Sep 21, 2016 3:00 pm

Re: K=...? (pg 73 course reader pre-equilibrium ex)

Postby Michelle_Li_1H » Wed Feb 22, 2017 11:42 pm

That K would be the equilibrium constant, which would equal to the concentration of the products over the concentration of the reactants.

The purpose is to find an equation that relates the intermediate or in this case [N2O2] with [NO]^2. We would do so by treating the first step as if it were at equilibrium, which gives us the equilibrium constant K.

Hope this helps!

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