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? ChartShows the initial reaction rate measurement for the acidic conditions performed in acidic condition (H+). Equation2Fe2+(aq)+Cl2(aq)----> 2Fe3+(aq)+2Cl-(aq) Experiments[Fe2+][Cl2][H+]RateExperiment 10.0014 M0.0045 M0.10 M1.03x10-5 M/sExperiment 20.0040 M0.0045 M0.10 M1.98x10-5 M/sExperiment 30.0014 M0.0090 M0.10 M2.02x10-5 M/sExperiment 40.0040 M0.0090 M0.10 M3.90x10-5 M/sExperiment 50.0014 M0.0045 M0.05 M1.97x10-5 M/sExperiment 60.0014 M0.0045 M0.01 M9.98x10-5 M/s

Rate law for the given equation is: Order of the reaction = m+n+p 1) To get m value, consider…

Answered: Determine the rate law, rate…

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter11: Dynamic Electrochemistry

Section: Chapter Questions

Problem 10P

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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^-5M/s
Experiment 2	0.0040 M	0.0045 M	0.10 M	1.98x10^-5M/s
Experiment 3	0.0014 M	0.0090 M	0.10 M	2.02x10^-5M/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^-5M/s
Experiment 6	0.0014 M	0.0045 M	0.01 M	9.98x10^-5M/s

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