The reaction of hypochlorite ion with iodide ion in 1 M aqueous hydroxide soluti

Question

The reaction of hypochlorite ion with iodide ion in 1 M aqueous hydroxide solution

OCl- + I- OI- + Cl-

is first order in OCl- and first order in I-.

Complete the rate law for this reaction in the box below.
Use the form k[A]m[B]n... , where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear.

Rate =   k[OCl]-[I]

In an experiment to determine the rate law, the rate constant was determined to be 78.6 M-1s-1. Using this value for the rate constant, the rate of the reaction when [OCl-] = 1.14×10-3 M and [I-] = 2.64×10-3 M would be  Ms-1.

Explanation / Answer

If 1s order with respect to OCl- ionthen

Rate = k*[OCl-]^1

for I --< assume 0 order

b)

k = 78.6 1/(Ms)

IF rate is 1/(M-s) this must be 2nd order

so

for [I] assume there is also first order

RAte = (78.6)(1.14*10^-3)(2.64*10^-3)

Rate = 0.00023655 M/s

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