A student conducts an experiment where she monitors the pressure and temperature inside a container that is holding a particular alcohol in the gas phase. The container volume and the amount of gas did not change during cooling. The temperature and pressure data appear in the table and graph below. Temperature (K) Pressure (atm) 873 15.55 764 13.61 651 11.60 543 9.67 433 7.71 Relationship Between Temperature and Pressue of an Alcohol in the Gas Phase 18 16 14 12 10 6. 4 100 200 300 400 500 600 700 800 900 1000 Temperature (K) (a) Does the graph demonstrate a direct relationship, an inverse relationship, or no relationship between temperature and pressure when the alcohol is in the gas phase? Explain your choice. (b) Provide a particle-level explanation for the relationship between the two variables. (c) Predict the pressure that would be observed if the container was at a temperature of 1,135 K. Pressure (atm) 2.
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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