A $10\mathrm{.}0L$ tank at $29\mathrm{.}1C$ is filled with $4\mathrm{.}16g$ of dinitrogen monoxide gas and $11\mathrm{.}2g$ of sulfur hexafluoride 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$[[$dinitrogen monoxide,mole fraction:,$],[$partial pressure:,atm$],[$sulfur hexafluoride,mole fraction:,$],[$potal pressure in tank:$,$atm$]]$