Respuesta :
When gaseous F₂ and solid I₂ are heated to high temperatures, the I₂ sublimes and gaseous iodine heptafluoride forms. If 350. torr of F₂ and 2.50 g of solid I₂ are put into a 2.50-L container at 250. K and the container is heated to 550. K. The partial pressure of I₂ gas  is 178 torr.
[tex]$7 \mathrm{~F}_{2}+\mathrm{I}_{2} \rightarrow 2 \mathrm{IF}_{7}$[/tex]
1) [tex]$\mathrm{PV}=\mathrm{nRT}$[/tex]
2) [tex]$n=m / M$[/tex]
[tex]$\mathrm{n}\left(\mathrm{I}_{2}\right)=(3.30 \mathrm{~g}) /((2) \times(126.90 \mathrm{~g} / \mathrm{mol}))=0.013$[/tex] moles
3) [tex]$F_{2}$[/tex] is limiting reactant
4) 7 moles [tex]$\mathrm{F}_{2}-2$[/tex] moles [tex]$\mathrm{IF}_{7}$[/tex]
[tex]$0.045$[/tex] moles [tex]$\mathrm{F}_{2}-\mathrm{x}$[/tex] moles [tex]$\mathrm{IF}_{7}$[/tex]
[tex]$x=0.013$[/tex]moles
5)[tex]$\mathrm{PV}=\mathrm{nRT}$[/tex]
[tex]$\mathrm{P}=\mathrm{nRT} / \mathrm{V}=(0.013 \mathrm{moles}) \times\left(62.36 \mathrm{~L} \cdot \mathrm{Torr}^{-1} \cdot \mathrm{K}^{-1} \cdot \mathrm{mol}^{-1}\right) \times(550 \mathrm{~K}) /(2.50 \mathrm{~L})=178 \mathrm{Torr}$[/tex]
Each gas that makes up a mixture of gases has a partial pressure, which is the notional pressure of that gas as if it alone filled the original combination's complete volume at the same temperature.
At sea level, where atmospheric pressure is known to be 760 mm Hg, the partial pressures of the various gases can be estimated to have partial pressures of approximately 593 mm Hg for nitrogen, 160 mm Hg for oxygen, and 7.6 mm Hg for argon.
To calculate the partial pressure of a gas: Divide the dissolved gas moles by the moles of the mixture to find the mole fraction. Multiply the total pressure by the mole fraction to find the partial pressure of the chosen gas
Learn more about partial pressure https://brainly.com/question/13199169
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