A gas mixture containing equal masses of O2 (g) and SO3 (g) is kept in a constant-volume vessel. The partial pressure of O2 (g) in the mixture is 1.00 atm. (No chemical reaction occurs in the vessel). I. The molar mass of the mixture is 45.7 g/mol. II. The total pressure in the vessel is 1.40 atm. III. If the mass of SO3 in the vessel was doubled at the same temperature, its partial pressure would be 0.800 atm. Which of the given statements is/are true for this mixture? Your answer: Only II Only II I and II Il and III O I, II, and III
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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