The reaction, 2NO(g) + O2(g) → 2NO2(g) proceeds via the following steps:
NO + NO \[\xrightarrow{{{{\text{K}}_{\text{a}}}}}\] N2O2
N2O2 \[\xrightarrow{{{{\text{K}}_{{\text{a'}}}}}}\] NO + NO
N2O2 + O2 \[\xrightarrow[{\left( {{\text{slow}}} \right)}]{{{{\text{k}}_{\text{b}}}}}\] NO2 + NO2
The rate of this reaction is equal to
A. 2kb[NO][O2]
B. (2Kakb[NO]2[O2])/(Ka + kb[O2])
C. 2kb [NO]2[O2]
D. Ka[NO]2[O2]
Answer: Option C
This Question Belongs to Engineering Chemistry >> Chemical Kinetics
Related Questions on Chemical Kinetics
The half-life of a first order reaction varies with temperature according to
A. In t1/2 ∝ 1/T
B. In t1/2 ∝ T
C. t1/2 ∝ 1/T2
D. t1/2 ∝ T2
A. 0.1386 min-1
B. 0.0693 min-1
C. 0.1386 mol L-1min-1
D. 0.0693 mol L-1min-1
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