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For the following reaction, Kc = 0.513 at 500 K. N2O4(g)⇌2NO2(g) Part A If a reaction...

For the following reaction, Kc = 0.513 at 500 K.
N2O4(g)⇌2NO2(g)

Part A

If a reaction vessel initially contains an N2O4 concentration of 5.50×10−2 MM at 500 K, what are the equilibrium concentrations of N2O4 and NO2 at 500 K?

[N2O4], [NO2] =

nothing
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Homework Answers

Answer #1

Let x be the change in concentration to reach equilibrium.

Hence, At equilibrium:

[N2O4] = initial concentration - change in concentration = 5.5 x 10-2 - X

[NO2] = initial concentration + change in concentration = 0 + 2X

Hence, equilibrium constant expression will be given by:

Solving for x we get:

Therefore, Equilibrium concentrations will be:

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