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An environmental chemist sampling industrial exhaust gases
Chapter 6, Problem 42P(choose chapter or problem)
An environmental chemist sampling industrial exhaust gases from a coal-buming plant collects a CO2-SO2-H2O mixture in a 21-L steel tank until the pressure reaches 850. torr at 45°C.
(a) How many moles of gas are collected?
(b) If the SO2 concentration in the mixture is 7.95 × 103 parts per million by volume (ppmv), what is its partial pressure? [Hint: ppmv = (volume of component/volume of mixture) × 106.]
Questions & Answers
QUESTION: Problem 42P
An environmental chemist sampling industrial exhaust gases from a coal-buming plant collects a CO2-SO2-H2O mixture in a 21-L steel tank until the pressure reaches 850. torr at 45°C.
(a) How many moles of gas are collected?
(b) If the SO2 concentration in the mixture is 7.95 × 103 parts per million by volume (ppmv), what is its partial pressure? [Hint: ppmv = (volume of component/volume of mixture) × 106.]
ANSWER:
Solution 42P
Step 1
(a) Here we have to find out how many moles of gas are collected.
Given:
In this question it has been given that,
The volume of steel tank = 21 L
Pressure = 850 torr = 0.098 atm
Temperature = 45 oC = 273 + 45 = 318 K
The moles of gas collected can be calculated by using ideal gas equation as follows,
n =
Where P = pressure
V = Volume
T = temperature
n = number of moes
R = gas constant i.e 0.0821 L atm mol-1 k-1
Now substituting the values, the number of moles can be calculated as,
n =
= = 0.89961 or 0.90 mol gas
Thus 0.90 mol of gas has been collected.