The reaction of hypochlorite ion with iodide ion in1Maqueoushydroxide solution.
ID: 535951 • Letter: T
Question
The reaction of hypochlorite ion with iodide ion in1Maqueoushydroxide solution. OCT + I rightarrow is first order in OCT and first order in I. Complete the rate law for this reaction in the box below. Use form k[A]"[B]" where "I" is understood for ma (don't enter I) and concentration stake to the zero power appear. In an experiment to determine the rate law, the rate of the reaction was determined to be 1.37 times 10^3 Ms^-1 when [OCI] = 1.73 times 10^3 M and [T] = 8.36 times 10^2 M from this experiment, the constant is M^-1s^-1.Explanation / Answer
The reaction is
OCl- + I- -------> OI- + Cl-
It is said that the reaction is first order in both the reactants Therefore, the rate law for the reaction can be written as
Rate = k[OCl-]1[I-]1 where k = second order rate constant (the reaction is first order in each reactant; hence must be 2nd order overall). Therefore,
Rate = k[OCl-][I-] (ans)
The values of the rate, [OCl-], [I-] are given. Plug in values and obtain k.
(1.37*10-3 Ms-1) = k*(1.73*10-3 M)*(8.36*10-2 M) (I hope I read the exponents correctly, the figure is quite hazy).
===> (1.37*10-3 Ms-1) = k*(1.44628*10-4 M2)
===> k = (1.37*10-3 Ms-1)/(1.44628*10-4 M2) = 9.472 M-1s-1 9.50 M-1s-1 (ans).
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