A 9.00 L tank at \( 6.22^{\circ} \mathrm{C} \) is filled with 3.76 g of carbon dioxide gas and 10.4 g of dinitrogen monoxide 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 dinitrogen monoxide & mole fraction: & \( \square \) \\
\hline partial pressure: & \( \square \mathrm{atm} \) \\
\hline \multicolumn{2}{|c|}{ Total pressure in tank: } & \( \square \mathrm{atm} \) \\
\hline
\end{tabular}