Solve the following problems assuming a constant pressure. 1. A sample of nitrogen occupies a volume of 250 mL at 25° C. What volume will it occupy at 95° C? 2. Oxygen gas is at a temperature of 40° C when it occuples a volume of 2.3 liters. To what temperature should it be raised to occupy a volume of 6.5 liters? 3. Hydrogen gas was cooled from 150° C to 50° C. Its new volume is 75 mL. What was its original volume? 4. Chlorine gas occupies a volume of 25 mL at 30 K. What volume will it occupy at 600 K? 5. A sample of neon gas at 50° C and a volume of 2.5 liters is cooled to 25° C. What is the new volume? 6. Fluorine gas at 300 K occupies a volume of 500 mL. To what temperature should it be lowered to bring the volume to 300 mL?
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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