2. In order to study the photochemical decay of aqueous bromine in bright sunlig

Question

2. 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 60 245 174 123 08 062 04 ppm Br 1.74 1.23 0.88 0.62 0.44 (a) Use the differential method to determine the reaction order with respect to 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) 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 do you suggest if you were to obtain more data?

Explanation / Answer

a) the graph of ln [A] vs time is straight line indicating first order reaction

the slope=-k

k=0.3433 s-1

b) 25 gallons means 94.63L

1ppm is 1 mg/L. so, in 94.63L you need 94.63mg to maintain 1ppm

rate law= k*[A]

=0.3433* 94.63

= 32.486 mg/s

In 1 sec we need 32.486mg, then in 1hr = 3600*32.486=116949.6mg

convert this into pounds= 116949.9* 2.2046e-6 = 0.257 pounds

so the rate should be 0.257 pounds/hour

c) i dont know this

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