Reaction rates

 

LABORATORY REPORT

Laboratory Assignment: Reaction Rates

 

 

 

1. PURPOSE (10 POINTS)

 

 

 

 

 

 

 

1. TEST DATA (15 POINTS)

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

Water displaced in milliliters	Time in seconds
2 mL
4 mL
6 mL
8 mL
10 mL
12 mL
14 mL
16 mL
18 mL
20 mL
22 mL

 

 

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

Water displaced in milliliters	Time in seconds
2 mL
4 mL
6 mL
8 mL
10 mL
12 mL
14 mL
16 mL
18 mL
20 mL
22 mL

 

 

 

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

Water displaced in milliters	Time in seconds
2 mL
4 mL
6 mL
8 mL
10 mL
12 mL
14 mL
16 mL
18 mL
20 mL
22 mL

 

 

 

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

 

 

 

 

 

 

1. RESULTS (15 POINTS)

 

Overall rate law:

 

 

 

1. CONCLUSION (10 POINTS)

 

 

 

 

 

1. QUESTIONS (30 POINTS)

 

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)