Laboratory Assignment for Module 3: Reaction Rates
(eScience Lab 4 [16])

Table 1. 10 mL Undiluted IKI and 5 mL 3% H₂O₂

Table 2. 10 mL 0.5–1.0% IKI and 5 mL 3% H₂O₂

Table 3. 10 mL 0.5–1.0% IKI and 5 mL 2.25% H₂O₂

III. CALCULATIONS (20 POINTS)

Table 1: 10 mL Undiluted IKI and 5 mL 3% H₂O₂

 Slope:

Inverse Slope:

Table 2: 10 mL 0.5–1.0% IKI and 5 mL 3% H₂O₂

Slope:

Inverse Slope:

Table 3:10 mL 0.5–1.0% IKI and 5 mL 2.25% H₂O₂

Slope:

Inverse Slope:

Order of H₂O₂:

Order of IKI:

Rate law constant:

*Show Calculations and Include Graphs

IV.  RESULTS (15 POINTS)

Overall rate law:

1.      How many grams of IKI (iodine-potassium iodide; molar mass = 166.0 g/mol) would it take to obtain a 100.0 mL solution of 0.300 M IKI? How many grams of IKI would it take to create a 100.0 mL solution of 0.600 M IKI? (6 points)

2.      What is the molarity of 100.0 mL of a 3.0% H₂O₂ (mass/volume) solution? What is the molarity of 100.0 mL  of a 2.25% H₂O₂ (mass/volume) solution?  (6 points)

3.      When finding the order of H₂O₂, why was Trial 1 and Trial 3 used? (6 points)

4.      When  finding the order of IKI, why was Trial 1 and Trial 2 used? (6 points)

5.      How does temperature affect the reaction rate? Explain in terms of the collision theory.
(6 points)