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

Answer 1

Answer: The rate of the reaction is $2.36\times 10^{-4}Ms^{-1}$

Explanation:

Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

$OCl^-+I^-\rightarrow OI^-+Cl^-$

$Rate=k[OCl^-]^m[I^-]^n$

where m = n = 1

$Rate=78.6M^{-1}s^{-1}\times [1.14\times 10^{-3}M]^1\times [2.64\times 10^{-3}M]^1=2.36\times 10^{-4}Ms^{-1}$

The rate of the reaction is $2.36\times 10^{-4}Ms^{-1}$