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Peroxodisulfate ion, S2O82–, decomposes in aqueous solution as follows: 2S2O82–(aq) + 2H2O(l) = 4SO42–(aq) + O2(g)...

Peroxodisulfate ion, S2O82–, decomposes in aqueous solution as follows:

2S2O82–(aq) + 2H2O(l) = 4SO42–(aq) + O2(g) + 4H+(aq)

When the solution is buffered at pH = 1.00, the rate obeys the following rate law:

Rate = – = k[S2O82–] /delta t = k[ S2O82-]

Under this condition, it was found that it took 330 s for the concentration of S2O82- to decrease from 0.100 M to 0.072 M. (a) Calculate the rate constant k and indicate the appropriate unit for k. (b) What is the half-life for this reaction in minutes? (c) How long in minutes for 75% of the original amount of S2O82– to decompose? (Answer:

(a) k = 1.0 x 10–3 s–1; (b) 690 s; (c) 23 minutes)

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