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# Oct_03 - Kinetic Molecular Theory Assumptions for an Ideal...

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Kinetic Molecular Theory Assumptions for an Ideal Gas: (1) Gases are very small particles, so they occupy negligible volume. (2) Random collisions with the walls create the pressure exerted by the gas. (3) The particles do not interact with each other. (4) The average kinetic energy of the particles is proportional to the absolute temperature (K).

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Pressure depends on: collision frequency of the gas molecules with the walls the momentum of the gas particles PV = 1 3 n N A m u 2 Molecular View of Pressure Analyzing these two factors, you can show ū = average gas velocity m = mass of gas particle n = moles of gas particles
Kinetic Energy PV = 2 3 1 2 n N A m u 2 = 2 3 KE Using our experimental results for 1 mole of an ideal gas PV = RT = 2 3 KE or KE = 3 2 RT Rewriting the previous equation

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Using the previous equation, you can show that for an ideal gas: u 2 = 3 RT M or u 2 = 3 RT M = u rms Conclusions: (1) lighter gases move faster at a given temperature (2) all gases move faster at higher temperatures u rms 1 M u rms T Relative Speeds of Gases
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Oct_03 - Kinetic Molecular Theory Assumptions for an Ideal...

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