Reaction 1: Peroxydisulfate & Iodide Anion

[brake4country]

Homework Statement

Peroxydisulfate ion reacts with the iodide anion according to reaction 1:

S²O₈^2- + 3 I^-⇔ 2 SO₄^2- + I_3^-

The amount of I_3^- formed can be determined by adding a known amount of S_sO₃^2- and allowing it to react according to reaction 2:

2 S₂O₃^2- + I₃^- ⇔ S₄O₆^2- + 3I^-

If starch is added, any excess I₃^- will react to form a blue-black I₂ complex. The formation of this complex indicates the completion of reaction 2. The rate of reaction 1 can be determined by the following equation where t is the elapsed time from the addition of the last component to the formation of the blue-black starch, I₂ complex.

rate = 1/2 [S₂O₃^2-]/t

(1) what would happen to the time and the rate in equation 1, if more S₂O₃^2- were added, and all other conditions remained the same?

Homework Equations

The Attempt at a Solution

The thiosulfate ion only applies to reaction 1, therefore, I assumed that the time would be constant and the rate would increase; however, I need help understanding my initial rationale. Thanks!

 

[Greg Bernhardt]

I'm sorry you are not generating any responses at the moment. Is there any additional information you can share with us? Any new findings?