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