*Mole Fraction (X)** relates the moles of solute and solvent within a solution:*

$\overline{){\mathbf{m}}{\mathbf{o}}{\mathbf{l}}{\mathbf{e}}{\mathbf{}}{\mathbf{f}}{\mathbf{r}}{\mathbf{a}}{\mathbf{c}}{\mathbf{t}}{\mathbf{i}}{\mathbf{o}}{\mathbf{n}}{\mathbf{}}{\mathbf{\left(}}{\mathbf{X}}{\mathbf{\right)}}{\mathbf{=}}\frac{\mathbf{m}\mathbf{o}\mathbf{l}\mathbf{e}\mathbf{}\mathbf{o}\mathbf{f}\mathbf{}\mathbf{s}\mathbf{o}\mathbf{l}\mathbf{u}\mathbf{t}\mathbf{e}}{\mathbf{m}\mathbf{o}\mathbf{l}\mathbf{e}\mathbf{}\mathbf{o}\mathbf{f}\mathbf{}\mathbf{s}\mathbf{o}\mathbf{l}\mathbf{u}\mathbf{t}\mathbf{i}\mathbf{o}\mathbf{n}}}$

**Step 1: Moles of solute and solvent.**

A solution is prepared by dissolving 20.2 mL of methanol (CH_{3}OH) in 100.0 mL of water at 25 ^{o}C. The densities of methanol and water at this temperature are 0.782 g/mL and 1.00 g/mL, respectively. For this solution, calculate each of the following.

Mole percent of methanol

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