KMT, Graham’s Law & Real Gases. Kinetic Molecular Theory. 1. Volume of individual particles is zero. 2. Collisions of particles with container walls cause pressure exerted by gas. Kinetic Molecular Theory. 3. Particles exert no forces on each other.
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1. Volume of individual particles is zero.
2. Collisions of particles with container walls cause pressure exerted by gas.
3. Particles exert no forces on each other.
4. Average kinetic energy Kelvin temperature of a gas.
Kelvin temperature is an index of the random motions of gas particles (higher T means greater motion.)
(The derivation of this equation can be found in many college physics texts)
Diffusion: describes the mixing of gases. The rate of diffusion is the rate of gas mixing.
Effusion: describes the passage of gas into an evacuated chamber.
Must correct ideal gas behavior when at high pressures and low temperatures
-volume of molecules becomes significant
-attractive forces become important
The rate of effusion of a particular gas was measured and found to be 24.0 mL/min. Under the same conditions, the rate of effusion of pure methane gas is 47.8 mL/min. What is the molar mass of the unknown gas?
Van der Waal’s constants, a and b, are dependent on the type of gas molecule (see table 5.3)
Which gas will diffuse faster, ammonia (NH3) or carbon dioxide (CO2)? What are their relative rates of diffusion?
Freon-12 is used as a refrigerant in central home air-conditioners. The rate of effusion of Freon-12 to Freon-11 (molar mass = 137.4 g/mol) is 1.07:1. The formula of Freon-12 is one of the following: CF4, CF3Cl, CF2Cl2, CFCl3 or CCl4