6. Consider that the average lung can hold about 6 liters of air and the composition of air is 78% nitrogen and 22% oxygen. If you breathe in 3.2 grams of air at 1.3 atm and 26 °C, do you completely fill your lungs with air?
Ideal and Real Gases
Ideal gases obey conditions of the general gas laws under all states of pressure and temperature. Ideal gases are also named perfect gases. The attributes of ideal gases are as follows,
Gas Laws
Gas laws describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. The very first observations about the physical properties of gases was made by Robert Boyle in 1662. Later discoveries were made by Charles, Gay-Lussac, Avogadro, and others. Eventually, these observations were combined to produce the ideal gas law.
Gaseous State
It is well known that matter exists in different forms in our surroundings. There are five known states of matter, such as solids, gases, liquids, plasma and Bose-Einstein condensate. The last two are known newly in the recent days. Thus, the detailed forms of matter studied are solids, gases and liquids. The best example of a substance that is present in different states is water. It is solid ice, gaseous vapor or steam and liquid water depending on the temperature and pressure conditions. This is due to the difference in the intermolecular forces and distances. The occurrence of three different phases is due to the difference in the two major forces, the force which tends to tightly hold molecules i.e., forces of attraction and the disruptive forces obtained from the thermal energy of molecules.
![the total gas mixture is compressed to a pressure of 5.2 atm before combustion, calculate the total
volume of the gas mixture at this point in time.
6.
Consider that the average lung can hold about 6 liters of air and the composition of air is
78% nitrogen and 22% oxygen. If you breathe in 3.2 grams of air at 1.3 atm and 26 °C, do you
completely fill your lungs with air?
7.
Calculate the partial pressure of nitrogen and oxygen in a mixture of 35.8 grams of
nitrogen gas and 28.3 grams s of oxygen gas
in a 1.65 L container at 42 °C.
8)
atm. The
An unsealed 450.0 mL beaker contains 320mL of a very dense gas at 52 °C and 3.12
gas is much denser than the surrounding air, so it does not disperse into the air.
At constant pressure, what would the temperature have to reach for the gas to fill the
a.
beaker?
b.
At constant temperature, what pressure is required for the gas to fill the beaker?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1838b780-8427-4597-888a-028907f173dc%2F1d194dc2-d331-48e0-a90a-2ff7806a2c0a%2F1xz4yxi_processed.jpeg&w=3840&q=75)
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