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The rate law for the reaction, 2NO(g) + O2(g) -- 2NO2(g), is found to be: rate of reaction=k[NO]2[O2]2 (PLEASE note that the 2's after the concentrations are powers, so we have NO to the power of 2 and O2 to the power of 2). The first, fast step is
2NO(g) -- N2O2 (g) (note: this arrow is also in reverse)
Which best represents the rate equation for the rate-determining step of this reaction?
Chose from these answer choices:
A) rate of reaction = k1 [NO]
B) rate of reaction = k2 [N2O2]
C) rate of reaction = k3 [N2O2][O2]
D) rate of reaction = k3 [NO2][O2]
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