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What is the partial pressure of CO2 in bar in atmosphere if its concentration is 385 parts per million by volume and the total atmospheric pressure is 14 pis?
Wiki User
∙ 12y ago
Assuming ideal gas behaviour for CO2 and air, the mole fraction of CO2 in air would
be 0.000385 since the data of 385 ppm are given by volume.
Then the partial pressure of CO2 in the atmospheric air is given by the product of
CO2 mole fraction and the atmosphere's total pressure.
So, p.p.CO2 = 0.000385 x 14 psi = 0.00539 psi.
Relation of psi to bar, 14.696 psi = 1.01325 bar.
Finally, p.p.CO2 = 0.00539 psi x [1.01325 bar/14.696 bar] = 3.72 x 10-4 bar
Wiki User
∙ 12y ago
To find the partial pressure of CO2 in the atmosphere, first convert the concentration to a decimal fraction: 385 ppm = 0.000385. Then, calculate the partial pressure by multiplying the concentration by the total pressure: 0.000385 * 14 psi = 0.00539 psi. Converting this value to bars gives approximately 0.00037 bar.
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