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KMT and Graham’s Law

KMT and Graham’s Law. Molecular Speed Of A Gas. Depends on the mass of the gas molecules and the temperature they are at R is in different units and has a different value ( R=8.3145) M is molar mass in kg/mole. Example. Find the speed of hydrogen gas at 25 o C.

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KMT and Graham’s Law

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  1. KMT and Graham’s Law

  2. Molecular Speed Of A Gas • Depends on the mass of the gas molecules and the temperature they are at R is in different units and has a different value ( R=8.3145) M is molar mass in kg/mole

  3. Example • Find the speed of hydrogen gas at 25o C. • Find the speed of oxygen gas at 25o C.

  4. Effusion • Gas escapes through tiny holes when a pressure difference is present

  5. Diffusion • Gases will mix uniformly

  6. Graham’s Law • Rate of both effusion and diffusion is inversely related to the square root of their weights • Shows the relationship between rate and molecular weight

  7. Example • If an unknown gas effuses at a rate that is only .468 times that of oxygen at the same temperature, what is its molecular weight?

  8. Ideal vs. Real Gas Behavior • Ideal gases follow all of the gas laws outlined • No gas is totally ideal, but at low pressures and/or high temperatures most come close • Gases will deviate significantly from ideal at high pressures and/or low temperatures - particles become closer together and intermolecular forces between significant

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