The Oxidation of Iodide Ions by Hydrogen Peroxide

September 15, 2009

1. Objectives:

We Will Write a Custom Essay Specifically
For You For Only $13.90/page!


order now

* To determine the rate law.

* To determine the activation energy.

2. Experimental Methods:

2.1 General Procedure: The procedure was followed by the lab manual, Principles of Chemistry, CHEM 1211L & CHEM 1212L Laboratory Experiments, A Project Oriented Approach, 4th Edition, 2009-Fall, p.137-150.

3. Experimental Results:

3.1 Data Table

CLASS DATA

Raw Data – Concentration Data

Reaction Time

Avg time

(s)

Reaction

mL H2O2

ml I-

Run A

Run B

Run C

1

5

5

839

1300

1245

1128

2

7.5

5

379

594

796

590

3

10

5

632

447

764

614

4

12.5

5

363

540

426

443

5

5

7.5

843

800

822

6

5

10

710

570

519

600

7

5

12.5

611

463

537

Table 1: Class Data

3.1 Data Table (Cont.)

Raw Data

Rate vs Temperature

Stock Concentrations

Temp

time

23

443

[S2O3]

4.00E-04

60

136

[H2O2]

0.04

5

1277

[I-]

0.04

4

2372

Table 2: Raw Data & Stock Concentrations

Reaction

[H2O2]

(10-3 M)

Rate

(10-8 M/s)

ln([H2O2]

ln(Rate)

1

4.0

7.1

-5.5

-16.5

2

6.0

9.7

-5.1

-16.1

3

8.0

13.3

-4.8

-15.8

4

10.0

14.9

-4.6

-15.7

Table 3: H2O2 Runs

Order

1

ORDER FOR IODIDE

Reaction

[I-]

(10-3 M)

Rate

(10-8 M/s)

ln([I-]

ln(Rate)

1

4.0

7.1

-5.5

-16.5

5

6.0

9.7

-5.1

-16.1

6

8.0

13.3

-4.8

-15.8

7

10.0

14.9

-4.6

-15.7

Order

1

TEMPERATURE DEPENDENCE

T(K)

Rate

(10-8 M/s)

k

1000/T

ln(k)

296

18.1

564334.1

3.4

13.2

333

58.8

1838235.3

3.0

14.4

278

6.3

195771.3

3.6

12.2

277

3.4

105396.3

3.6

11.6

[H2O2]

0.008

[I]

0.004

R = k[H2O2][I-]

3.2 Graphs