Question

The following is a proposed mechanism for the gas phase decomposition of nitryl chloride. step 1 fast: NO2CNO2+CI step 2 slow: NO2CI+CI NO2 + Cl2 (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Which species acts as a catalyst? Enter formula. If none, leave box blank: (3) Which species acts as a reaction intermediate? Enter formula. If none, leave box blank: (4) Complete the rate law for the overall reaction that is consistent with this mechanism. Use the form k[A][B]", where 'T' is understood (so don't write it if it's a '1') for m, n etc. Rate =

Answer 1

step 1 :   fast   NO2Cl---------> NO2 + Cl

step 2 : slow     NO2Cl + Cl -----------> NO2 + Cl2

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1.                  2NO2Cl ---------------------> 2NO2 + Cl2   overall reaction

2. no catalyst

3. intermediate Cl

4. The rate of reaction depends upon the slow step is called rate determining step

Rate law

Rate = K[NO2Cl]^1[Cl]^1    >>>>>>answer