Let us consider the following reaction NO2(g) + CO(g)-> NO(g) + CO2(g) the rate equation of reaction is Rate = K[NO2]2 then the rate determining step is:
Correct answer: B. NO2 + NO2 --> NO3+NO
- A. 2NO2 + CO --> 2NO + CO2
- B. NO2 + NO2 --> NO3+NO
- C. NO2+NO --> NO + CO2
- D. NO2+CO --> NO + CO2
Explanation
The proposed mechanism for this reaction is as follows.Slow :NO2(g) + NO2(g)→NO3(g) + NO(g) (rate determining step)Fast :NO3 (g) + CO(g)→NO2(g) + CO2(g)The first step is the rate determining step as it is the slow step.
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Reaction kinetics relates reaction rate to concentration, temperature, surface area and catalysts. Questions cover rate laws, reaction order, rate constants, activation energy and the activated complex, including how a catalyst lowers the activation energy without changing the overall energy change or equilibrium position.
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