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Find the atmospheric concentration in steady-state in both µg/m³ and parts per million if the pollutant of interest is sulfur. Recall that ppm is expressed as:

Find the atmospheric concentration in steady-state in both µg/m³ and parts per million if the pollutant of interest is sulfur. Recall that ppm is expressed as:

Applications and Investigations in Earth Science (9th Edition)
Applications and Investigations in Earth Science (9th Edition)
9th Edition
ISBN:9780134746241
Author:Edward J. Tarbuck, Frederick K. Lutgens, Dennis G. Tasa
Publisher:Edward J. Tarbuck, Frederick K. Lutgens, Dennis G. Tasa
Chapter1: The Study Of Minerals
Section: Chapter Questions
Problem 1LR
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A source is producing 1 gram/day of sulfur at a mountain location where the atmospheric pressure is 0.643 atm. Dry deposition removes 1% of the total mass of sulfur in the air each day, while chemical reactions remove another 3% each day. The pressure follows the relationship p(z) = po e-0.00013z, where z is the elevation in meters and po = 1 atmosphere at sea level. The temperature is 10°C (283 K) at sea level and dT/dz = - ½ . You may assume the source is located in a small airshed with an air volume of 10 Million m³. a. Find the atmospheric concentration in steady-state in both ug/m³ and parts per million if the pollutant of interest is sulfur. Recall that ppm is expressed as: moles of sulfur million moles of air b. All of the sulfur leaking out of the tank is found to be in the form of SO2. With the production of sulfur equal to 1 gram/day, what is the production written in terms of grams SO2/day? What is the concentration expressed as ug of SO2/m³ air and the concentration expressed as ppm for SO2? (You do not need to recalculate from the beginning – just write the answer and explain it).
Transcribed Image Text:A source is producing 1 gram/day of sulfur at a mountain location where the atmospheric pressure is 0.643 atm. Dry deposition removes 1% of the total mass of sulfur in the air each day, while chemical reactions remove another 3% each day. The pressure follows the relationship p(z) = po e-0.00013z, where z is the elevation in meters and po = 1 atmosphere at sea level. The temperature is 10°C (283 K) at sea level and dT/dz = - ½ . You may assume the source is located in a small airshed with an air volume of 10 Million m³. a. Find the atmospheric concentration in steady-state in both ug/m³ and parts per million if the pollutant of interest is sulfur. Recall that ppm is expressed as: moles of sulfur million moles of air b. All of the sulfur leaking out of the tank is found to be in the form of SO2. With the production of sulfur equal to 1 gram/day, what is the production written in terms of grams SO2/day? What is the concentration expressed as ug of SO2/m³ air and the concentration expressed as ppm for SO2? (You do not need to recalculate from the beginning – just write the answer and explain it).
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