A mixture of He, Ne, and Ar have a total pressure of 558 mmHg. If the partial pressure of He is 341 mmHg and the partial pressure of Ne is 112 mm Hg, what is the partial pressure of Ar? a) b) Calculate the partial pressure of O2 (g) that a diver breathes with a heliox mixture containing 2% O2 (g) at a depth of 90 m where the total pressure if 10.0 atm.
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.
![s Handout - Intro
6. Dalton's Law of Partial Pressure
a) A mixture of He, Ne, and Ar have a total pressure of 558 mmHg. If the partial pressure of
He is 341 mmHg and the partial pressure of Ne is 112 mm Hg, what is the partial pressure
of Ar?
Equation
PV-P.V,
Meaning
There is an inverse
relationship between pressure
and volume of a gas.
The volume of a gas is directly
proportional to the
temperature.
Relates P, V and T
V V
T T
PV P.V
T,
PV-uRT
b) Calculate the partial pressure of O2 (g) that a diver breathes with a heliox mixture
P-pressure (atm)
V- volume (L)
containing 2% O2 (g) at a depth of 90 m where the total pressure if 10.0 atm.
1- amount (mol)
R-0.0821 4tm L
T-temperature (K)
The total pressure of a
gas mixture is the sum of
the partial pressures of
cach gas.
тol K
- P - P +...
c) A diver breathing heliox with an oxygen composition of 5% wants to adjust the total
pressure so that the partial pressure of Oz (g) 0.21 atm, whal must the tolal pressure be?
gas problems:
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