A sample of gas is collected in a balloon that can easily expand and contract. It should be noted that the pressure and the number of moles of gas both remain constant. The following data is collected from the balloon: Temperature (°C) -34.6 Volume (L) 20.0 22 -10.8 25 25 27 48.8 Construct a plot of temperature vs. volume. Keep the units for temperature in °C; do not convert the temperatures to Kelvin. Make a line of best fit for the data points, and then extrapolate the line back to where the volume is 0. Answer the following questions about your graph: 1. At what temperature (in °C) does the sample have a volume of zero litres? Use the equation of the line of best fit to determine this temperature. 2. What is the significance of this temperature? 3. Can a sample of a gas ever have an actual volume of zero litres? Why or why not? 4. Now use the equation of the line to determine what the volume of the gas would have to be in order for the gas to have a temperature of -350°C. Does this answer make sense? Why or why not?
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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