A 9.00 L tank at \( 15 .{ }^{\circ} \mathrm{C} \) is filled with 12.0 g of carbon dioxide gas and 8.06 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: & \( \square \) \\
\hline partial pressure: & \( \square \mathrm{atm} \) \\
\hline \multicolumn{2}{|c|}{ Total pressure in tank: } & \( \square \mathrm{atm} \) \\
\hline
\end{tabular}