A+B+C ⇒ D Exp. Initial B Initial A (mol/dm³) Init. Rate of Formation of D (mol/dm³ min-¹) (mol/dm³) 1 0.10 0.10 3.0 x 10-4 2 0.30 0.30 9.0 x 10-4 3 0.10 0.30 3.0 x 10-4 4 0.20 0.40 6.0 x 10-4 5 0.10 0.10 1.2 x 10-3 The student concluded that the rate equation should be: rate= K[A][B][C]² ii) Using the data for experiment 4, calculate the value of the rate constant, k, using the correct rate equation, making sure that you include the correct units. Initial C (mol/dm³) 0.10 0.10 0.10 0.10 0.20

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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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A+B+CD
Exp.
Initial A
(mol/dm³)
Initial B
(mol/dm³)
Init. Rate of Formation
of D (mol/dm³ min-¹)
1
0.10
0.10
3.0 x 10-4
2
0.30
0.30
9.0 x 10-4
3
0.10
0.30
3.0 x 10-4
4
0.20
0.40
6.0 x 10-4
5
0.10
0.10
1.2 x 10-3
The student concluded that the rate equation should be:
rate = K[A] [B][C]²
ii) Using the data for experiment 4, calculate the value of the rate constant, k, using the correct rate
equation, making sure that you include the correct units.
Initial C
(mol/dm³)
0.10
0.10
0.10
0.10
0.20
Transcribed Image Text:A+B+CD Exp. Initial A (mol/dm³) Initial B (mol/dm³) Init. Rate of Formation of D (mol/dm³ min-¹) 1 0.10 0.10 3.0 x 10-4 2 0.30 0.30 9.0 x 10-4 3 0.10 0.30 3.0 x 10-4 4 0.20 0.40 6.0 x 10-4 5 0.10 0.10 1.2 x 10-3 The student concluded that the rate equation should be: rate = K[A] [B][C]² ii) Using the data for experiment 4, calculate the value of the rate constant, k, using the correct rate equation, making sure that you include the correct units. Initial C (mol/dm³) 0.10 0.10 0.10 0.10 0.20
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