The iodide ion, I- , is oxidized to the hypoiodite ion, IO- , by the hypochlorit

Question

The iodide ion, I-
, is oxidized to the hypoiodite ion, IO-
, by the hypochlorite ion,
ClO-
, in basic solution. The equation is ions.

+ ()
()

+ ()
()
The following initial rate experiments were run, and for each, the initial rate of
formation of IO-
was determined. Find the rate law and the value of the rate
constant.
Initial Concentrations
(mol/L)
Initial Rate
(mol/(L s)
I
- ClO-
OH-
[I-] [ClO-] [OH-] Initial rate
Exp. 1 0.010 0.020 0.010 12.2 x 10-2
Exp. 2 0.020 0.010 0.010 12.2 x 10-2
Exp. 3 0.010 0.010 0.010 6.1 x 10-2
Exp. 4 0.010 0.010 0.020 3.0 x 10-2

Explanation / Answer

rate = k (I-)((ClO-)

first order with respect to I-

first order with respect to ClO-

rate is independent on OH-

k = rate / (I-)((ClO-)

k = 12.2 x 10-2 / (0.01)(0.02)

k= 305 M-1 time-1

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