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Three of the primary components of air are
carbon dioxide, nitrogen, and oxygen. In a
sample containing a mixture of only these
gases at exactly one atmosphere pressure, the
partial pressures of carbon dioxide and nitrogen
are given as PCO2 = 0.285 torr and
PN2 = 569.523 torr. What is the partial pressure
of oxygen?
Answer in units of torr.

Respuesta :

Hunaid

Answer:

PO2 = 166.19 torr

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The partial pressure of oxygen gas in the given misture of the gas at 1 atm is 190.2 torr.

What is Dalton's law?

Dalton's law of gas states that total pressure of any mixture of gas is equal to the sum of the partial pressures of each gases present in that mixture.

According to the question,

Total pressure of gas = 1 atm = 760 torrs

Partial pressure of carbon dioxide = 0.285 torrs

Partial pressure of nitrogen = 569.523 torrs

Partial pressure of oxygen = ?

According to Dalton's law:
Total pressure = Partial pressure of carbon dioxide + Partial pressure of nitrogen + Partial pressure of oxygen

Partial pressure of oxygen = 760 - (0.285 + 569.523) = 190.2 torr

Hence required partial pressure is 190.2 torr.

To know more about Dalton's law, visit the below link:
https://brainly.com/question/13082853

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