Gases and the Kinetic Molecular Theory

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Presentation transcript:

Gases and the Kinetic Molecular Theory

Speeds of gas molecules. For a single molecule. Kinetic energy is: KE = ½ mv2 m = mass; v = velocity For a collection of gas molecules, the average kinetic energy is: R = ideal gas constant = 8.314 J/Kmol T = temperature in Kelvin

How fast do gas molecules move? Called the root mean square speed of the gas. in kg/mol Equation gives speed in meters/second. What is the rms speed of O2 molecules at room temperature?

Boltzmann Distributions

Boltzmann Distributions and Molar Mass

Boltzmann Distributions and Temperature

Gas Diffusion

Gas Effusion

Graham’s Law of Gas Effusion: used for determining molar mass of a gas

Example: A sample of ethane, C2H6, effuses through a small hole at a rate of 3.6 x 10-6 mol/hr. An unknown gas, under the same conditions, effuses at a rate of 1.3 x 10-6 mol/hr. Calculate the molar mass of the unknown gas.