7. Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution. H+H₂O₂H₂O-OH (rapid equilibrium) H₂O-OH+Br→ HOBr + H₂O (slow) HOBr+ H+ Br Br₂ + H₂O (fast) Which of the following rate laws is consistent with the mechanism? A. Rate-k[H₂O₂][H*[Br] B. Ratek[H₂O-OH][Br] C. Rate-k[H₂O₂][H*][Br] D. Rate-k[HOBr][H][Br][H₂O₂] E. Rate [Br] W 8. In the previous problem, k has been simplified as a single constant. Write the individual constants that make up the overall, simplified k for the reaction.

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