(References] A 19.9-L tank is filled with H, to a pressure of 200. atm. How many balloons (each 2.00 L) can be inflated to a pressure of 1.00 atm from the tank? Assume the ideal gas behavior, that there is no temperature change, and that the tank cannot be emptied below 1.00 atm pressure. balloon(s) Submir
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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[References]
A 19.9-L tank is filled with H2 to a pressure of 200. atm. How many balloons (each 2.00 L) can be inflated to a pressure of 1.00 atm from the tank? Assume the ideal gas behavior, that there is no
temperature change, and that the tank cannot be emptied below 1.00 atm pressure.
balloon(s)
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The pressure of a fixed amount of gas changes inversely with its volume (if the temperature is constant). This statement is known as Boyle’s law (based on the experiment conducted by Robert Boyle). For a fixed amount of gas at constant temperature, let the initial volume be V1 and the pressure be p1. Let V2 and p2 be the corresponding final quantities after expansion (or contraction) of the gas. Then the Boyle’s law can be written as:
Given data:
Here p1= 200 atm V1= 19.9 L
And p2= 1.00 atm V2 =2.00 L
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