Iodide ion is oxidized to hypoiodite ion, IO-, by hypochlorite ion, ClO-, in basic solution. The equation is I-(aq) + ClO-(aq) +OH-(aq) → IO-(aq) + Cl-(aq) The following intitial rate experiments were run and, for each, the initial rate of formation of IO- was determined. Initial Rate (mol/(L•s)) Exp. 1 0.010 M 0.020 M 0.010 M 12.2x10-2 Exp. 2 0.020 M 0.010 M 0.010 M 12.2x10-2 Exp. 3 0.010 M 0.010 M 0.010 M 6.1x10-2 Exp. 4 0.010 M 0.010 M 0.020 M 3.0x10-2 What is the rate law for the reaction?
Iodide ion is oxidized to hypoiodite ion, IO-, by hypochlorite ion, ClO-, in basic solution. The equation is I-(aq) + ClO-(aq) +OH-(aq) → IO-(aq) + Cl-(aq) The following intitial rate experiments were run and, for each, the initial rate of formation of IO- was determined. Initial Rate (mol/(L•s)) Exp. 1 0.010 M 0.020 M 0.010 M 12.2x10-2 Exp. 2 0.020 M 0.010 M 0.010 M 12.2x10-2 Exp. 3 0.010 M 0.010 M 0.010 M 6.1x10-2 Exp. 4 0.010 M 0.010 M 0.020 M 3.0x10-2 What is the rate law for the reaction?
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Chapter13: Rates Of Reaction
Section: Chapter Questions
Problem 13.56QP: Iodide ion is oxidized to hypoiodite ion, IO, by hypochlorite ion, ClO, in basic solution. The...
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Iodide ion is oxidized to hypoiodite ion, IO-, by hypochlorite ion, ClO-, in basic solution. The equation is
I-(aq) + ClO-(aq) +OH-(aq) → IO-(aq) + Cl-(aq)
The following intitial rate experiments were run and, for each, the initial rate of formation of IO- was determined.
Initial Rate (mol/(L•s)) |
||||
Exp. 1 | 0.010 M | 0.020 M | 0.010 M | 12.2x10-2 |
Exp. 2 | 0.020 M | 0.010 M | 0.010 M | 12.2x10-2 |
Exp. 3 | 0.010 M | 0.010 M | 0.010 M | 6.1x10-2 |
Exp. 4 | 0.010 M | 0.010 M | 0.020 M | 3.0x10-2 |
What is the rate law for the reaction?
Input the answer in the form rate = k[A]2[B]
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