Iodide ion is oxidized to hypoiodite ion, IO^-, by hypochlorite ion, ClO^-, in basic solution as: I^-(aq) + ClO^-(aq) --(OH^-)-- IO^-(aq) + Cl^-(aq). The following initial-rate experiments were run..

Question

Iodide ion is oxidized to hypoiodite ion, IO^-, by hypochlorite ion, ClO^-, in basic solution as: I^-(aq) + ClO^-(aq) --(OH^-)--> IO^-(aq) + Cl^-(aq). The following initial-rate experiments were run... The correct rate law for the reaction is

Prashant Kotian · Accepted Answer

Correct answer: D. Comparing Exp 3 and 4: [OH^-] doubles, rate halves => order w.r.t OH^- is -1. Exp 1 and 3: [ClO^-] doubles, rate doubles => order 1. Exp 2 and 3: [I^-] doubles, rate doubles => order 1. Rate = K[I^-][ClO^-][OH^-]^-1. Therefore, correct answer is D.

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