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:
Time (min) | 10 | 20 | 30 | 40 | 50 | 60 |
ppm Br2 | 2.45 | 1.74 | 1.23 | 0.88 | 0.62 | 0.44 |
(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, calculale the required hourly rate of injection of bromine (in pounds) into a sunlit body of water, 25,000 gal in volume, in order to maintain a sterilizing level of bromine of 1.0 ppm.
(c) What experimental conditions would you suggest if you were to obtain more data?
(Note: ppm = parts of bromine per million parts of brominated water by weight. In dilute aqueous solutions, 1 ppm = I milligram per liter.) (From California Professional Engineers Exam.)
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