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# Scan_Doc0121 - 5.7 Effusion and Diffusion 213 Stated in...

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In Graham's law the units for molar mass can be glmol or kglmol, since the units Vii; cancel in the ratio , r.-:- vM 1 EXAMPLE 5.20 '" 0.04 0) :; ~ (3 E; b 0.02 ~ co ;: 0) 2 ~ 0.03 0.01 o o UF 6 at 273 K H2 at 273 K 1000 2000 3000 Speed Figure 5.23 Relative molecular speed distribution of H2 and UF e . 5.7 Effusion and Diffusion 213 Stated in another way, the relative rates of effusion of two gases at the same tempera- ture and pressure are given by the inverse ratio of the square roots of the masses of the gas particles: Rate of effusion for gas 1 Rate of effusion for gas 2 where M J and M2 represent the molar masses of the gases. This equation is called Graham's law of effusion. Calculate the ratio of the effusion rates of hydrogen gas (H 2 ) and uranium hexafluoride (UF6)' a gas used in the enrichment process to produce fuel for nuclear reactors (see Fig. 5.23). Solution First we need to compute the molar masses: Molar mass of H2 = 2.016 glmol, and molar mass of UF 6 = 352.02 g/mol. Using Graham's
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## This note was uploaded on 12/13/2010 for the course CHEM 2301 taught by Professor Bill during the Spring '10 term at South Texas College.

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