(1) Find the limiting reactant

MM of I_{2} = 253.8 g/mol

MM of F_{2} = 38.0 g/mol

$\mathbf{mol}\mathbf{}{\mathbf{IF}}_{\mathbf{5}}\mathbf{}\mathbf{=}\mathbf{}\mathbf{10}\mathbf{.}\mathbf{2}\overline{)\mathbf{}\mathbf{g}\mathbf{}{\mathbf{I}}_{\mathbf{2}}}\mathbf{}\left(\frac{1\overline{)\mathrm{mol}{I}_{2}}}{253.8\overline{)g}}\right)\left(\frac{2\mathrm{mol}{\mathrm{IF}}_{5}}{1\overline{)\mathrm{mol}{I}_{2}}}\right)$

mol IF_{5} = 0.0804 mol IF_{5}

$\mathbf{mol}\mathbf{}{\mathbf{IF}}_{\mathbf{5}}\mathbf{}\mathbf{=}\mathbf{}\mathbf{10}\mathbf{.}\mathbf{2}\overline{)\mathbf{}\mathbf{g}\mathbf{}{\mathbf{F}}_{\mathbf{2}}}\mathbf{}\mathbf{\left(}\frac{\mathbf{1}\mathbf{}\overline{)\mathbf{mol}\mathbf{}{\mathbf{F}}_{\mathbf{2}}}}{\mathbf{38}\mathbf{}\overline{)\mathbf{g}}}\mathbf{\right)}\mathbf{\left(}\frac{\mathbf{2}\mathbf{}\mathbf{mol}\mathbf{}{\mathbf{IF}}_{\mathbf{5}}}{\mathbf{5}\mathbf{}\overline{)\mathbf{mol}\mathbf{}{\mathbf{F}}_{\mathbf{2}}}}\mathbf{\right)}$

mol IF_{5} = 0.1074 mol IF_{5}

Gaseous iodine pentafluoride, IF_{5}, can be prepared by the reaction of solid iodine and gaseous fluorine:

I_{2} (s) + 5 F_{2}(g) → 2 IF_{5} (g)

A 5.10-L flask containing 10.2 g I_{2} is charged with 10.2 g F_{2}, and the reaction proceeds until one of the reagents is completely consumed. After the reaction is complete, the temperature in the flask is 125^{o}C.

What is the partial pressure of IF_{5} in the flask?

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