Hydrogen peroxide, H₂O₂, has a density of 1.45 g/cm³ and decomposesspontaneously but slowly. The decomposition reaction will proceed at afaster rate if iodide ion, a catalyst, is added. The steps for the catalyzedreaction are:H₂O₂(aq) + (aq) → H₂O(l) + Ol-(aq)OOH₂O₂(aq) + Ol(aq) →H₂O(l) + O₂(g) +1-(aq)a. What is the net reaction?b. If 10.00 mL of H₂O₂ undergoes thisreaction, what mass of oxygen is produced?c. If the reaction has an 85.5% yield, whatmass of oxygen is actually produced?

Given: Density of H2O2 solution = 1.45 g/cm3 = 1.45 g/mL Volume of H2O2 decomposed = 10 mL

Hydrogen peroxide, H₂O₂, has a density of 1.45 g/cm³ and decomposes spontaneously but slowly. The decomposition reaction will proceed at a faster rate if iodide ion, a catalyst, is added. The steps for the catalyzed reaction are: H₂O₂(aq) + (aq) → H₂O(l) + Ol-(aq) H₂O₂(aq) + Ol(aq) → H₂O(l) + O₂(g) + (aq) a. What is the net reaction? b. If 10.00 mL of H₂O₂ undergoes this reaction, what mass of oxygen is produced? c. If the reaction has an 85.5% yield, what mass of oxygen is actually produced?

Hydrogen peroxide, H₂O₂, has a density of 1.45 g/cm³ and decomposes spontaneously but slowly. The decomposition reaction will proceed at a faster rate if iodide ion, a catalyst, is added. The steps for the catalyzed reaction are: H₂O₂(aq) + (aq) → H₂O(l) + Ol-(aq) H₂O₂(aq) + Ol(aq) → H₂O(l) + O₂(g) + (aq) a. What is the net reaction? b. If 10.00 mL of H₂O₂ undergoes this reaction, what mass of oxygen is produced? c. If the reaction has an 85.5% yield, what mass of oxygen is actually produced?

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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