K11. Given the initial rate data below, what is the rate law for the reaction: 4 Fe²+ + O2 +4 H4 Fe³+ + 2 H₂O? Experiment [Fe2+lo [02]o [H*Jo 1 2 3 4 a) Rate = K[Fe²+] [O₂] [H] c) Rate = k[Fe²+] [0₂]² [H*] e) Rate = k[Fe²+1² [0₂] [H*]² 1 x 10³ 1 x 10³ 0.1 2 x 10³ 2 x 10-3³ 0.1 2 x 103 1 x 10-³ 0.2 2 x 10-3 2 x 103 0.2 Initial Rate A[02]/Ato 5 x 104 8 x 10-3 8 x 10-3 1.6 x 10-2 b) Rate = k[Fe²+1³ [0₂] [H] d) Rate = k[Fe²+] [0₂]²
K11. Given the initial rate data below, what is the rate law for the reaction: 4 Fe²+ + O2 +4 H4 Fe³+ + 2 H₂O? Experiment [Fe2+lo [02]o [H*Jo 1 2 3 4 a) Rate = K[Fe²+] [O₂] [H] c) Rate = k[Fe²+] [0₂]² [H*] e) Rate = k[Fe²+1² [0₂] [H*]² 1 x 10³ 1 x 10³ 0.1 2 x 10³ 2 x 10-3³ 0.1 2 x 103 1 x 10-³ 0.2 2 x 10-3 2 x 103 0.2 Initial Rate A[02]/Ato 5 x 104 8 x 10-3 8 x 10-3 1.6 x 10-2 b) Rate = k[Fe²+1³ [0₂] [H] d) Rate = k[Fe²+] [0₂]²
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![K11. Given the initial rate data below, what is the rate law for the reaction:
4 Fe²+ + O₂ + 4H-4 Fe³+ + 2 H₂O?
Experiment [Fe2+lo [02]o [H*Jo
1
2
3
4
a) Rate = K[Fe²+] [0₂] [H*]
c) Rate = k[Fe²+] [0₂]² [H+]
e) Rate = k[Fe²+1² [0₂] [H*]²
1 x 10³ 1 x 10-³ 0.1
2 x 10³ 2 x 10-³ 0.1
2 x 103 1 x 10-³ 0.2
2 x 103 2 x 10-³ 0.2
Initial Rate
A[02]/A to
5 x 104
8 x 10-3
8 x 10-3
1.6 x 10-2
b) Rate = k[Fe²+1³ [0₂] [H]
d) Rate = k[Fe²+] [0₂]²](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9077c120-5b3f-4825-86ae-193451a028c6%2F9be25473-a367-496b-9361-22794d09fd67%2Fj6diek_processed.jpeg&w=3840&q=75)
Transcribed Image Text:K11. Given the initial rate data below, what is the rate law for the reaction:
4 Fe²+ + O₂ + 4H-4 Fe³+ + 2 H₂O?
Experiment [Fe2+lo [02]o [H*Jo
1
2
3
4
a) Rate = K[Fe²+] [0₂] [H*]
c) Rate = k[Fe²+] [0₂]² [H+]
e) Rate = k[Fe²+1² [0₂] [H*]²
1 x 10³ 1 x 10-³ 0.1
2 x 10³ 2 x 10-³ 0.1
2 x 103 1 x 10-³ 0.2
2 x 103 2 x 10-³ 0.2
Initial Rate
A[02]/A to
5 x 104
8 x 10-3
8 x 10-3
1.6 x 10-2
b) Rate = k[Fe²+1³ [0₂] [H]
d) Rate = k[Fe²+] [0₂]²
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