Question

The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following way:

OCl−+I−→OI−+Cl−.

This rapid reaction gives the following rate data:

[OCl−](M) [I]−(M) Rate (M/s)
1.5×10^−3 1.5×10^−3 1.36×10^−4
3.0×10^−3 1.5×10^−3 2.72×10^−4
1.5×10^−3 3.0×10^−3 2.72×10^−4

a. Write the rate law for this reaction.
b. Calculate the rate constant with proper units.
c. Calculate the rate when [OCl-]= 1.8×10^3 M and [I-]= 6.0×10^4 M .

Answer 1

The rate law for the given reaction is Rate = k [OCl−] [I−]. The rate constant can be calculated using the rate data. The rate can also be calculated using the rate law equation given the concentrations of OCl- and I-.

Step-by-step explanation:

The given chemical reaction between OCl− and I− can be represented by the rate law: Rate = k [OCl−] [I−]. The rate constant (k) can be calculated by substituting the values from the rate data into the rate law equation. When [OCl-] = 1.8×10^3 M and [I-] = 6.0×10^4 M, the rate can be calculated using the rate law equation as well.