2. Graphing Pressure versus Volume: Boyle's Law Pressure vs Volume 950 900 850 800 750 700 650 600 550 20.0 22.0 24.0 26.0 28.0 30.0 32.0 34.0 Volume (mL) Questions and Problems Q1 According to your graph, what is the relationship between the pressure and the volume of a gas? ther sodentS Q2 On your graph, what is the volume of the gas at a pressure of 760. mmHg? bath Q3 On your graph, what is the pressure of the gas when the volume is 30.0 mL? Q4 A sample of helium has a volume of 325 mL and a pressure of 655 mmHg. What will be the pressure, in mmHg, if the sample of helium is compressed to 125 mL (T, n constant)? 1358 1358 Q5 A 75.0-mL sample of oxygen has a pressure of 1.50 atm. What will be the new volume, in milliliters, if the pressure of the sample becomes 4.50 atm (T, n constant)? Pressure (mm Hg)
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.
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