1.If 60.5 mol of an ideal gas is at 3.39 atm at 62.70 ∘C, what is the volume of the gas? 2.A sample of an ideal gas has a volume of 2.35 L at 2.80×102 K and 1.09 atm. Calculate the pressure when the volume is 1.82 Land the temperature is 306 K. 3.An open flask sitting in a lab refrigerator looks empty, but it is actually filled with a mixture of gases called air. If the flask volume is 2.50 L, and the air is at standard temperature and pressure, how many gaseous molecules does the flask contain?
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.
1.If 60.5 mol of an ideal gas is at 3.39 atm at 62.70 ∘C, what is the volume of the gas?
2.A sample of an ideal gas has a volume of 2.35 L at 2.80×102 K and 1.09 atm. Calculate the pressure when the volume is 1.82 Land the temperature is 306 K.
3.An open flask sitting in a lab refrigerator looks empty, but it is actually filled with a mixture of gases called air. If the flask volume is 2.50 L, and the air is at standard temperature and pressure, how many gaseous molecules does the flask contain?
4.A 3.65 g sample of an unknown gas at 61 ∘C and 1.00 atm is stored in a 2.05 L flask.What is the density of the gas? What is the molar mass of the gas?
5. An unknown gas at 73.1 ∘C and 1.05 atm has a molar mass of 44.10 g/mol. Assuming ideal behavior, what is the density of the gas?
6. A 0.04336 g sample of gas occupies 10.0 mL at 293.5 K and 1.10 atm. Upon further analysis, the compound is found to be 25.305% C and 74.695% Cl. What is the molecular formula of the compound?
7.Consider this molecular‑level representation of a mixture of gases. (see attached image) If the partial pressure of the diatomic gas is 0.300 atm, what is the total pressure?
8.If 60.5 mol of an ideal gas is at 3.39 atm at 62.70 ∘C, what is the volume of the gas?
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