🤓 Based on our data, we think this question is relevant for Professor Nettles' class at MSSTATE.

Recall that ** Graham's Law of Effusion** allows us to compare the rate of effusion of two gases. Graham's Law states that the rate of effusion of a gas is inversely proportional to its molar mass.

$\mathbf{rate}\mathbf{=}\frac{\mathbf{1}}{\sqrt{\mathbf{MM}}}$

This means that when comparing two gases:

$\overline{)\frac{\mathbf{rate}\mathbf{}\mathbf{1}}{\mathbf{rate}\mathbf{}\mathbf{2}}{\mathbf{=}}\sqrt{\frac{{\mathbf{MM}}_{\mathbf{2}}}{{\mathbf{MM}}_{\mathbf{1}}}}}$

We separate U-235 from U-238 by fluorinating a sample of uranium to form UF_{6} (which is a gas) and then taking advantage of the different rates of effusion and diffusion for compounds containing the two isotopes.

Calculate the ratio of effusion rates for ^{238} UF_{6} and ^{235} UF_{6}. The atomic mass of U-235 is 235.054 amu and that of U-238 is 238.051 amu.

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Based on our data, we think this problem is relevant for Professor Nettles' class at MSSTATE.