25. Which of the following is FALSE about the observed properties of gases? A) Gases will expand because they have no definite shape or volume B) As the temperature increases, the pressure will increase (especially in a closed container) C) Gases have very high densities D) Gases are completely miscible 26. According to Charles' Law, at 25 degrees Celcius a volume of water will be 100 mL. If you raise the temperature to 37 degrees Celcius, the new volume of water will be? a) 104 ml b) 96 mL c) 148 ml. d) 67.6 mL 27. According to Reference Table G, what is the maximum amount of KNO, that can be dissolved in 100 g of water at 60 degrees Celcius? a) 50 g b) 110 g c) |as d) '85 g 28. What do we call two liquids that are mutually soluble in each other? a) Efflorescent b) Miscible c) Deliquescent d) Immicible
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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