The gas phase reaction of carbon monoxide with nitrogen dioxide is believed to o

Question

The gas phase reaction of carbon monoxide with nitrogen dioxide is believed to occur by the following mechanism: slow: 2 NO_2 rightarrow NO_3 + NO fast: NO_3 + CO rightarrow NO_2 + CO_2 What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. + rightarrow + Which species acts as a catalyst? Enter formula. If none leave box blank: Which species acts as a reaction intermediate? Enter formula. If none, leave box blank: Complete the rate law for the overall reaction that is consistent with this mechanism. (Use the form k[A]^m[B]^h.... where '1' is understood (so don't write it) for in. n etc.) Rate =

Explanation / Answer

(1) Over all reaction:

NO2 + CO --------------> NO + CO2

(2) No catalyst used

(3)

NO3 acts as reaction intermediate

(4)

Rate of reaction depends on slow step only.

So, rate law expression can be written as,

rate = k1[NO2]2

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