A suggested mechanism for the gas phase decomposition of nitrous oxide is: step

Question

A suggested mechanism for the gas phase decomposition of nitrous oxide is: step I slow: N_2O rightarrow_N2 + O step 2 fast: N_2O + O rightarrow N_2 + O_2 What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. 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]^n hellip, where T is understood (so don't write it) for m, n etc.) Rate = .

Explanation / Answer

step 1: N2O ==> N2 + O

step 2: N2O+ O ==> N2 + O2

1)

overall reaction can be obtained by adding both steps:

2N2O +(blank box) ==> 2N2 + O2

2) here, i would like to differentiate between catalyst and intermediate:

A catalyst is a species that is present at the beginning of a reaction and reappears at the end. It does not appear in the final equation.

An intermediate is not present at the beginning. It forms during the reaction and disappears before the end.

so no catalyst is there in this reaction.

3)

O forms during the reaction and is used up before the end. So O is the intermediate

4)

rate is determined by the slowest step.

So rate for this reaction would be:

rate= k[N2O]

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