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* 10^(-4)Ms^(-1)`

Step-by-step 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)* [1.14* 10^(-3)M]^1* [2.64* 10^(-3)M]^1=2.36* 10^(-4)Ms^(-1)`

The rate of the reaction is
`2.36* 10^(-4)Ms^(-1)`