1) Assuming ideal behaviour, calculate the pressure in atmospheres of 2.19 kilograms of hydrogen chloride gas (HCl(g) - yes, hydrochloric acid is also called hydrogen chloride, and it's a gas at room temperature. It's "liquid" when you use it in the lab because you use it dissolved in water!) in a 25.0 L container at 18°C.
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.
In the previous two questions, the actual pressure is less than the ideal pressure. Which false assumption in the kinetic molecular theory of gases has more effect on this error?
(Note - the actual pressure isn't always less than the ideal pressure - it depends on the conditions. In this set of examples, however, the conditions give Preal<Pideal.)
2) Given the Van der Waals constants for hydrogen chloride, below, calculate the pressure in atmospheres of 2.19 kilograms of hydrogen chloride gas in a 25.0 L container at 18°C.
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