Problem: 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)Based on the rate law, which step is rate determining?

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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)

Based on the rate law, which step is rate determining?

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