2nd Edition

ISBN: 9780321809261

Author: John E. McMurry, Robert C. Fay

Publisher: Prentice Hall

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Chapter 12, Problem 12.119CHP

Consider the following concentration–time data for the reaction of iodide ion and hypochlorite ion (OCl⁻). The products are chloride ion and hypoiodite ion (OI⁻).

Chapter 12, Problem 12.119CHP, Consider the following concentrationtime data for the reaction of iodide ion and hypochlorite ion

(a) Write a balanced equation for the reaction.
(b) Determine the rate law, and calculate the value of the rate constant.
(c) Does the reaction occur by a single-step mechanism? Explain.
(d) Propose a mechanism that is consistent with the rate law, and express the rate constant in terms of the rate constants for the elementary steps in your mechanism. (Hint: Transfer of an H⁺ ion between H₂O and OCl− is a rapid reversible reaction.)

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Chapter 12, Problem 12.118CHP

Chapter 12, Problem 12.120CHP

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Chapter 12 Solutions

General Chemistry: Atoms First

Ch. 12.1 - The oxidation of iodide ion by arsenic acid,...Ch. 12.1 - Prob. 12.2P Ch. 12.2 - Consider the last two reactions in Table 12.2....Ch. 12.3 - The oxidation of iodide ion by hydrogen peroxide...Ch. 12.3 - Prob. 12.5P Ch. 12.3 - Prob. 12.6CP Ch. 12.4 - Prob. 12.7P Ch. 12.4 - Prob. 12.8P Ch. 12.5 - Prob. 12.9P Ch. 12.5 - Prob. 12.10CP

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Solution Summary: The author explains that a balanced equation obeys the law of conservation of mass, which states that the number of atoms remains constant throughout the reaction.

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