Consider the formation of sulfur trioxide from sulfur dioxide and oxygen 2SO2 (g) + O2 (g) → 2 SO3 (g) a. If 40.0L of sulfur dioxide at STP is mixed with 40.0L of oxygen also at STP, the new container holds the mixture at STP. What is the volume of the mixture?
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.
Consider the formation of sulfur trioxide from sulfur dioxide and oxygen
2SO2 (g) + O2 (g) → 2 SO3 (g)
a.
If 40.0L of sulfur dioxide at STP is mixed with 40.0L of oxygen also at STP, the new container
holds the mixture at STP. What is the volume of the mixture?
b. The volume is proportional to the number of moles. Calculate the volume of SO3 produced at STP.
c. Calculate the volume of the reactant leftover at STP.
d. Calculate the total volume at the end at STP. [Hint: It will be less than starting volume.]
e. Like parts a and b, starting with 50.0L of sulfur dioxide, but only 10.0L of oxygen calculate the
total volume at the end (STP). [Hint: Think Limiting Reactant]
f.
Like part a or c, starting with 60.0L of sulfur dioxide and 40.0L of oxygen, calculate the total
volume at the end (STP). [Hint: Think Limiting Reactant]
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