G.53. Suppose you are studying the kinetics of the iodine-catalyzed decomposition of hydrogen peroxide.2 H₂O2 → 2 H₂O + O₂If you determine the initial rate is 7.50 × 10-4 M/s when [H₂O₂] = 0.452 M and [KI] = 0.285 M, what isthe rate constant? Assume that the order of both reactants is 1.Type answer:

The general rate equation is as follows: Rate = k [Reactants](order)

Suppose you are studying the kinetics of the iodine-catalyzed decomposition of hydrogen peroxide. 2 H₂O₂ → 2 H₂O + 0₂ If you determine the initial rate is 7.50 × 10-4 M/s when [H2₂O₂] = 0.452 M and [KI] = 0.285 M, what is the rate constant? Assume that the order of both reactants is 1.

Suppose you are studying the kinetics of the iodine-catalyzed decomposition of hydrogen peroxide. 2 H₂O₂ → 2 H₂O + 0₂ If you determine the initial rate is 7.50 × 10-4 M/s when [H2₂O₂] = 0.452 M and [KI] = 0.285 M, what is the rate constant? Assume that the order of both reactants is 1.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter13: Chemical Kinetics

Section: Chapter Questions

Problem 13.26QE

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