A 10.0 L tank at \( 21.6^{\circ} \mathrm{C} \) is filled with 4.83 g of carbon dioxide gas and 10.6 g of chlorine pentafluoride 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.
\begin{tabular}{|l|ll|}
\hline carbon dioxide & mole fraction: & \( \square \) \\
\hline partial pressure: & \( \square \mathrm{atm} \) \\
\hline chlorine pentafluoride & mole fraction: \\
& partial pressure: & \( \square \mathrm{atm} \) \\
\hline Total pressure in tank: & \( \square \mathrm{atm} \) \\
\hline
\end{tabular}