The reaction of nitrogen dioxide with carbon monoxide is second order in NO2 and

Question

The reaction of nitrogen dioxide with carbon monoxide is second order in NO2 and zero order in CO. Complete the rate law for this reaction in the box below. Use the form k[A]^m[B]^n... , where ?1? is understood for m, n ... (don?t enter 1) and concentrations taken to the zero power do not appear. Rate= In an experiment to determine the rate law, the rate constant was determined to be 0.730 M^-1s^-1. Using this value for the rate constant, the rate of the reaction when [NO2] = 1.26 M and [CO] = 0.452 M would be Ms^-1.

Explanation / Answer

Given

second order in N02 and zero order in CO

so the rate law is

rate = K [N02]^2 [C0]^0

so

rate = K [N02]^2

so the rate law is finally given as

rate = K [N02]^2

b)

given

K = 0.73

[N02] = 1.26

so

rate = 0.73 x [1.26]^2

rate = 1.158948

so the rate is 1.158948

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