A $5\mathrm{.}00L$ tank at $8\mathrm{.}65C$ is filled with $10\mathrm{.}6g$ of sulfur hexafluoride gas and $7\mathrm{.}83g$ of boron trifluoride gas. You can assume both gases behave as ideal gases under these conditions.

Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to $3$ significant digits.

$\backslash$table$[[$sulfur hexafluoride,mole fraction:,$],[$partial pressure:,atm$],[,$mole fraction:,$],[$boron trifluoride,partial pressure:,atm$],[$Total pressure in tank:$,$atm$]$

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