EXPERIMENT 4 : Kinetics- Determination of Order of Reaction PDF

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PAGE 6Experiment 4: Kinetics- Determination of Order of ReactionDatasheetTable: Volume of KMnO 4 Used and Concentration of H 2 O 2Reaction Time (min) 3 6 9 12 15 18Volume of KMnO 4 (Vfinal)(mL) 17 25 31 36 39 42.Volume of KMnO 4 (Vinitial)(mL) 0 17 25 31 36 39.Volume of KMnO 4 needed (Vfinal - Vinit...

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Experiment 4: Kinetics- Determination of Order of Reaction Datasheet Table: Volume of KMnO4 Used and Concentration of H2O2

Reaction Time (min)

3

6

9

12

15

18

Volume of KMnO4 (Vfinal)(mL)

17.5

25.5

31.5

36.0

39.4

42.2

Volume of KMnO4 (Vinitial)(mL)

0

17.5

25.5

31.5

36.0

39.4

17.5

8.0

6.0

4.5

3.4

2.8

4.4

2.0

1.5

1.1

Volume of KMnO4 needed (Vfinal - Vinitial) (mL)

Concentration of H2O2 (mol dm-3) remained unreacted at time t (using

-2

×10

-2

×10

-2

×10

-2

×10

0.9 -2

×10

0.7 ×10-2

Eq. 1) (Titration Calculations, 2020) (Northaqifah Hasna, 2020)

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Question 1) Plot a graph of concentration of H2O2 versus time.

Graph of Concentration of H2O2 versus Time Concentration of H202 (×10-2), mol dm-3

5 4.5

4.4

4 3.5 3 2.5

2

2

1.5

First half-life

1.5

1.1

0.9

1

0.7

Second half-life

0.5 Third half-life

0 3

6

9

12

15

18

21

24

Time taken, min

2) Determine from the graph, the first, second and third half-life of this reaction. From the graph, the first half-life is 3 minutes, the second half-life is 6 minutes and the third half-life is 12 minutes

3) How does the concentration affect the rate of dissociation of hydrogen peroxide? High concentration of the reactants will increase the rate dissociation of hydrogen peroxide. At higher concentration, there are more particles at the same amount of space. Thus, the particles are more likely to collide with each other and more frequent therefore, it will more likely to react. In the other hand, this will help the rate of dissociation of hydrogen peroxide become faster. Moreover, the low concentration of the reactant resulting vice versa. (Nurul Amni, 2020)

4) Determine the order of the above reaction. Second-order reaction

5) Write the rate equation for the above reaction. Rate = k[H2O2]2

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