Question

A $ 9.00 \mathrm{~L} \operatorname{tank} $ at $ 1.7^{\circ} \mathrm{C} $ is filled with 3.54 g of dinitrogen difluoride gas and 15.0 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 dinitrogen difluoride & mole fraction: & (I] \\ & partial pressure: & $ \square \mathrm{atm} $ \\ \hline chlorine pentafluoride & mole fraction: & $ \square $ \\ & partial pressure: & $ \square \mathrm{atm} $ \\ \hline \multicolumn{2}{|c|}{ Total pressure in tank: } & $ \square \mathrm{atm} $ \\ \hline \end{tabular}

          A \( 9.00 \mathrm{~L} \operatorname{tank} \) at \( 1.7^{\circ} \mathrm{C} \) is filled with 3.54 g of dinitrogen difluoride gas and 15.0 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 dinitrogen difluoride & mole fraction: & (I] \\
& partial pressure: & \( \square \mathrm{atm} \) \\
\hline chlorine pentafluoride & mole fraction: & \( \square \) \\
& partial pressure: & \( \square \mathrm{atm} \) \\
\hline \multicolumn{2}{|c|}{ Total pressure in tank: } & \( \square \mathrm{atm} \) \\
\hline
\end{tabular}

$A 9.00 Ltank at 1.7^∘C is filled with 3.54 g of dinitrogen difluoride gas and 15.0 g of chlorine pentafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. dinitrogen difluoride mole fraction: (I] partial pressure: □atm chlorine pentafluoride mole fraction: □ partial pressure: □atm 2|c| Total pressure in tank: □atm$

Added by Stephen C.

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