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**Problem**: Gaseous iodine pentafluoride, IF5, can be prepared by the reaction of solid iodine and gaseous fluorine:I2 (s) + 5 F2(g) → 2 IF5 (g)A 5.10-L flask containing 10.2 g I2 is charged with 10.2 g F2, and the reaction proceeds until one of the reagents is completely consumed. After the reaction is complete, the temperature in the flask is 125oC.What is the partial pressure of IF5 in the flask?

###### FREE Expert Solution

###### FREE Expert Solution

(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}

###### Problem Details

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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