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Chapter 7, Problem 7.8P

In order to study the photochemical decay of aqueous bromine in bright sunlight, a small quantity of liquid bromine was dissolved in water contained in a glass battery jar and placed in direct sunlight. The following data were obtained at 25°C:

Chapter 7, Problem 7.8P, In order to study the photochemical decay of aqueous bromine in bright sunlight, a small quantity of , example  1

  1. (a) Determine whether the reaction rate is zero, first, or second order in bromine, and calculate the reaction-rate constant in units of your choice.
  2. (b) Assuming identical exposure conditions, calculate the required hourly rate of injection of bromine (in pounds per hour) into a sunlit body of water, 25,000 gal in volume, in order to maintain a sterilizing level of bromine of 1.0 ppm. [Ans.: 0.43 lb/h]

Chapter 7, Problem 7.8P, In order to study the photochemical decay of aqueous bromine in bright sunlight, a small quantity of , example  2

  1. (c) Apply one or more of the six ideas in Preface Table P-4, page xxviii, to this problem. (Note: ppm = parts of bromine per million parts of brominated water by weight. In dilute aqueous solutions, 1 ppm = 1 milligram per liter.) (From California Professional Engineers’ Exam.)
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Chapter 7 Solutions

Elements of Chemical Reaction Engineering (5th Edition) (Prentice Hall International Series in the Physical and Chemical Engineering Sciences)

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