The air that we breathe is composed of 78% nitrogen (N2), 21% oxygen (O2), and the other 1% includes water vapor, carbon dioxide, and pollutants. If a tire is inflated to a pressure of 33 pounds per square inch (psi) with regular air, what is the partial pressure of nitrogen and of oxygen within the tire?
Partial pressure = mole fraction x total pressure.
For nitrogen, Partial pressure = 0.78 x 33psi = 25.74psi
For oxygen, Partial pressure = 0.21 x 33psi = 6.93psi
The air that we breathe is composed of 78% nitrogen (N2), 21% oxygen (O2), and the...
We can determine the molecular mass of air by considering nitrogen (N2), oxygen (O2) and argon (Ar) make up 78%, 21% and 1% of the atmosphere. The atomic masses of nitrogen, oxygen and argon are 14, 16, 40 grams/mole. Compute the molecular mass of air.
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}We mix 0.25 g of oxygen gas (O2) and 1.5 g nitrogen gas (N2) in a 2 L container at 20oC. Assuming both gases behave ideally, (a)what is the partial pressure of oxygen? (b)what is the partial pressure of nitrogen? (c)what is the total pressure in the container? Molar masses are 32 g/mol for oxygen and 28 g/mol for nitrogen.
Air is a gas mixture, and consists of approximately 78% nitrogen and 21% oxygen. Calculate the mass concentrations of the gas species at standard ambient temperature and pressure.
Almost all gaseous systems that we use are gas mixtures, air is the most obvious example. Air is composed of 78% nitrogen, 20% oxygen, 1 % argon, 1% water vapor, 0.3% carbon dioxide. Chemists often express the composition of a gas not with percent, but with a fraction. The mole fraction of nitrogen,ΧN2 , in air is defined as ΧN2= nN2 ⁄ nTotal = 0.78 The pressure of a gas mixture is the sum of the partial pressures of each...
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An air sample in the lungs contains oxygen at 98 mmHg, nitrogen at 568 mmHg, carbon dioxide at 32 mmHg, and water vapor at 51 mmHg. What is the total pressure, in atmospheres, exerted by the gas mixture?