You have studied the gas-phase oxidation of HBr by O2:
4HBr (g) + O2 (g) 2H2O (g) + 2Br2 (g)
You find the reaction to be first order with respect to HBr and first order with respect to O2. You propose the following mechanism:
HBr (g) + O2 (g) HOOBr (g)
HOOBr (g)+ HBr (g) 2HOBr (g)
HOBr (g) + HBr(g) H2O (g) + Br2 (g)
(a) Confirm that the elementary reactions add to give the overall reaction.
(b) Based on the experimentally determined rate law, which step is rate determining/ (c) what are the intermediates in this mechanism? (d) If you are unable to detect HOBr or HOOBr among the products, does this disprove your mechanism?
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