For the aqueous reaction 2 Cr³⁺ + 3 IO₄^- + 10 OH^-→2 CrO₄^{2 -} + 3 IO₃^- + 5 H₂O, under a given set of conditions, the rate of appearance of CrO₄^{2 -} is 3.0×10^{- 4} mol/L × s. What is the rate of disappearance of IO₄^-?

Question

Quizplus · Accepted Answer

The stoichiometry of the reaction shows that 3 moles of IO₄⁻ are consumed for every 2 moles of CrO₄²⁻ produced. Therefore, the rate of disappearance of IO₄⁻ is (3/2) times the rate of appearance of CrO₄²⁻, which is 4.5×10⁻⁴ mol/L × s.

For the Aqueous Reaction 2 Cr3+ + 3 IO4 -

For the Aqueous Reaction 2 Cr³⁺ + 3 IO₄^-