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The standard free energy of formation of nitric oxide, NO, at 800. K (roughly the temperature...

The standard free energy of formation of nitric oxide, NO, at 800. K (roughly the temperature in an automobile engine during ignition) is 72.0 kJ/mol. Δf H (N2) and Δf H (O2) =0.

Calculate the equilibrium constant for the reaction: N2(g) + O2(g) => 2NO(g) at 800. K. (R = 8.31 J/(K · mol)) 2NO(g)

a. 7.0 x 10^–10

b. 7.0 x 10^–9

c. 4 x 10^-10

d. 4 x 10^5

e. 6.8 x 10^–6

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Answer #1

Standard free energy formation of NO =

=

For 2 moles standard free energy of formation of NO = 144*103 J

Relation between standard free energy and equilibrium constant

, where R= 8.314 J/K.mol and T = 800 K

K = 4*10-10

So answer is (c)

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