Question

The proposed mechanism for the reaction ClO-(aq) + I-(aq) --> IO-(aq) + Cl-(aq) is

1. ClO-(aq) + H2O(l) <=> HClO(aq) + OH-(aq) FAST

2. I-(aq) + HClO(aq) <=> HIO(aq) + Cl-(aq) FAST

3. OH-(aq) + HIO(aq) => H2O(l) + IO-(aq) SLOW

Which of the following would be a rate law for the reaction? Note that the concentration of solvent, H2O, is constant.

Identify intermediates

answer: rate = k[ClO^-][I^-]/[Cl^-]

Answer 1

intermediats = HClO , OH-