Diffusion, Effusion, and Graham’s Law of Diffusion

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Presentation transcript:

Diffusion, Effusion, and Graham’s Law of Diffusion

What is diffusion? The movement of particles from regions of higher concentrations to regions of lower concentration. Eventually, the particles will disperse evenly throughout the space. Low High

What is effusion? The passage of a gas under pressure through a tiny opening.

Graham’s law of diffusion Thomas Graham studied effusion in detail and determined that the rate of effusion is indirectly proportional to the square root of the molar mass of the gas, if pressure and temperature are kept constant. In other words: vA vB = Molar MassB Molar MassA 

 How does that work? Let’s go back to the Kinetic Molecular Theory We saw that the movement of particles is proportional to the amount of kinetic energy. KE= ½ m v 2 So, if the KE is constant, ½ mA vA2 = ½ mB vB2 With a little algebra, we get: vA vB = Molar MassB Molar MassA 

Example Problems At the same temperature, which molecule travels faster, O2 or N2? How much faster? At room temperature, Xe atoms have an average speed of 240 m/s. At the same temperature, what is the speed of H2 molecules? What is the molar mass of a gas if it diffuses 0.907 times the speed of argon gas?

Answers 1) N2 (lower molar mass) (32/28) = 1.07 times faster 2) x/240 =  (131.3/2) x/240 = 8.10 x = 1944 m/s 3) 1/0.907 = (x/39.9) (1/0.907)2 = ((x/39.9))2 1.216 = x/39.9 x = 48.5 g/mol