The air all around us is a mixture of gasses containing nitrogen, oxygen, carbon dioxide, argon

and water vapor. If the partial pressure of nitrogen is 1.3 atm, the partial pressure of oxygen is

1824 mmHg, the partial pressure of carbon dioxide is 247 torr, the partial pressure of argon is

0.015 atm, and the partial pressure of water vapor is 53.69 kPa. What is the total pressure in

units of atmospheres (atm) ?

Total pressure = 4.57 atm

Explanation:

Given dа ta:

Partial pressure of nitrogen = 1.3 atm

Partial pressure of oxygen = 1824 mmHg

Partial pressure of carbon dioxide = 247 torr

Partial pressure of argon = 0.015 atm

Partial pressure of water vapor = 53.69 kpa

Total pressure = ?

Solution:

First of all we convert the units other into atm.

Partial pressure of oxygen = 1824 mmHg / 760 = 2.4 atm

Partial pressure of carbon dioxide = 247 torr / 760 = 0.325 atm

Partial pressure of water vapor = 53.69 kpa / 101 = 0.53 atm

Total pressure = Partial pressure of N + Partial pressure of O + Partial pressure of CO₂ + Partial pressure of Ar + Partial pressure of water vapor

Total pressure = 1.3 atm + 2.4 atm + 0.325 atm + 0.015 atm + 0.53 atm

Total pressure = 4.57 atm