Determine the rate law, rate constant(k) of the reaction with the given information. What's the balanced reaction using the half-reaction method. Also for experiment 1 what will be the concentration of [Fe2+] after 10 seconds? Chart Shows the initial reaction rate measurement for the acidic conditions performed in acidic condition (H+). Equation 2Fe2+(aq)+Cl2(aq)----> 2Fe3+(aq)+2Cl-(aq)
Determine the rate law, rate constant(k) of the reaction with the given information. What's the balanced reaction using the half-reaction method. Also for experiment 1 what will be the concentration of [Fe2+] after 10 seconds? Chart Shows the initial reaction rate measurement for the acidic conditions performed in acidic condition (H+). Equation 2Fe2+(aq)+Cl2(aq)----> 2Fe3+(aq)+2Cl-(aq)
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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Determine the rate law, rate constant(k) of the reaction with the given information. What's the balanced reaction using the half-reaction method. Also for experiment 1 what will be the concentration of [Fe2+] after 10 seconds?
Chart
Shows the initial reaction rate measurement for the acidic conditions performed in acidic condition (H+).
Equation
2Fe2+(aq)+Cl2(aq)----> 2Fe3+(aq)+2Cl-(aq)
| Experiments | [Fe2+] | [Cl2] | [H+] | Rate |
| Experiment 1 | 0.0014 M | 0.0045 M | 0.10 M | 1.03x10-5 M/s |
| Experiment 2 | 0.0040 M | 0.0045 M | 0.10 M | 1.98x10-5 M/s |
| Experiment 3 | 0.0014 M | 0.0090 M | 0.10 M | 2.02x10-5 M/s |
| Experiment 4 | 0.0040 M | 0.0090 M | 0.10 M | 3.90x10-5 M/s |
| Experiment 5 | 0.0014 M | 0.0045 M | 0.05 M | 1.97x10-5 M/s |
| Experiment 6 | 0.0014 M | 0.0045 M | 0.01 M | 9.98x10-5 M/s |
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