Answer Happy

SECTION B QUESTION 1 1.1 Consider the following gas - phase oxidation of hydrogen bromide (HBr) by oxygen (O₂): 4HBr(g) + O₂(g) → 2H₂O(g) + 2Br₂(g) The rate Law for this reaction is first order with respect HBr and first order with respect to O₂. The reaction proceeds as follows: Step 1: HBr(g) + O₂(g) → HOOBr(g) Step 2: HOOBr(g) + HBr(g) → 2HOBr(g) Step 3: HOBr(g) + HBr(g) → H₂O(g) + Brz₂(g) 1.1.1 Show how the three steps can be added to give the overall equation. 1.1.2 Write the rate law for each elementary step in the mechanism. 1.1.3 Write the rate law for the overall reaction. 1.1.4 Based on the rate law for the overall reaction, which step is rate determining? 1.1.5 Identify any intermediate/s in the mechanism. 6 (1) (1) (2) [27]