Ash C.

asked • 02/18/22

How do I write the equilibrium constant expressions for these quantities?

A. N2O4(g) <=> 2NO2(g)

B. CO(g) + 3H2(g) <=> CH4(g) + H2O(g)

C. 4NH3(g) +5O2(g) <=> 4NO(g) +6H2O(g)

D. CH4(g) + 2H2S(g) <=> CS2(g) + 4H2(g)

1 Expert Answer

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Andrew Y. answered • 02/18/22

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BS in Chemistry
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The general setup will be: Equilibrium Constant (K) = [Products]n / [Reactants]m,

Where n and m equal the coefficient in front.

part B for example would be: K = ([CH4] * [H2O]) / ([CO] * [H2]3)

Follow the same setup for the rest of the problems.

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J.R. S.

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I would just add that since all of the reactions given involve gases, you might consider using Kp where instead of concentrations, you use partial pressures. The expression will look the same but with pressures in place of concentrations and ( ) instead of [ ]. So, for B, it would be Kp = (CH4)(H2O) / (CO)(H2)^3
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02/18/22

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