### Kinetics of the Reaction Between Hydrogen Peroxide and Iodide Ion#### Experimental DataKinetic data were obtained on the aqueous reaction of hydrogen peroxide with iodide ion and H⁺:\[ H_2O_2 (aq) + 3 I^{-} (aq) + 2 H^{+} (aq) \rightarrow I_3^{-} (aq) + 2 H_2O (l) \]The following table summarizes the experimental data observed:| Exp. | \([H_2O_2]\), M | \([I^-]\), M | \([H^+]\), M | Initial Rate, M/s ||------|-------------------|------------|--------------|-------------------------|| 1 | 0.010 | 0.010 | 0.00050 | 1.15 × 10⁻⁶ || 2 | 0.020 | 0.010 | 0.00050 | 4.60 × 10⁻⁶ || 3 | 0.010 | 0.020 | 0.00050 | 1.15 × 10⁻⁶ || 4 | 0.010 | 0.010 | 0.00100 | 2.30 × 10⁻⁶ |#### Determine the Rate Law for the ReactionUsing the experimental data provided, determine the rate law for the reaction. None of the given answers are correct.### Possible Rate Law Options- \( R = 2.3 \, M^{-2} \, s^{-1} \, [\text{H}_2\text{O}_2]_2 \, [\text{H}^+] \)- \( R = 1.15 \times 10^{-2} \, M^{-1} \, s^{-1} \, [\text{H}_2\text{O}_2]_2 \)- \( R = 0.0115 \, M^{-1} \, s^{-1} \, [\text{H}_2\text{O}_2] \, [\text{I}^-] \)### Explanation of Graphs and DiagramsThere are no additional graphs or diagrams

Answered: Image /qna-images/answer/eea2a4b5-97b4-48cb-92ae-8f4852a75a42.jpg

Kinetic data were obtained on the aqueous reaction of hydrogen peroxide with iodide ion and H+. H2O2(aq) + 3 l-(aq) + 2 H+(aq) → 13-(aq) + 2 H2O(1) Exp. 1 [H₂O₂], M 0.010 [1], M [H-], M 0.00050 Initial Rate, M/s 1.15 x 10-6 0.010 2 0.020 0.010 0.00050 4.60 x 10-6 3 0.010 0.020 0.00050 1.15 x 10-6 4 0.010 0.010 0.00100 2.30 x 10-6 Determine the rate law for the reaction: none of the answers are correct R = 2.3 M-2 S-1 [H2O2]2 [H+] R = 1.15 x 10-2 M-1 S-1 [H2O2]2 R = 0.0115 M-1 S-1 [H2O2] [-]

Kinetic data were obtained on the aqueous reaction of hydrogen peroxide with iodide ion and H+. H2O2(aq) + 3 l-(aq) + 2 H+(aq) → 13-(aq) + 2 H2O(1) Exp. 1 [H₂O₂], M 0.010 [1], M [H-], M 0.00050 Initial Rate, M/s 1.15 x 10-6 0.010 2 0.020 0.010 0.00050 4.60 x 10-6 3 0.010 0.020 0.00050 1.15 x 10-6 4 0.010 0.010 0.00100 2.30 x 10-6 Determine the rate law for the reaction: none of the answers are correct R = 2.3 M-2 S-1 [H2O2]2 [H+] R = 1.15 x 10-2 M-1 S-1 [H2O2]2 R = 0.0115 M-1 S-1 [H2O2] [-]

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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