A tank at is filled with of dinitrogen difluoride gas and of carbon dioxide 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. Be sure your answers have the correct number of significant digits. dinitrogen difluoride molar fraction: partial pressure: carbon dioxide mole fraction: partial pressure: Total pressure in tank:

For N₂F₂:

Molar fraction = 0.84

Partial pressure = 1.12 atm

For SF₄:

Molar fraction = 0.16

Partial pressure = 0.208 atm

Explanation:

It seems your question is missing the values required to solve the problem. However, an internet search showed me the following values for your question. If the values in your problem are different, your answer will be different as well, however the solving method will remain the same:

" A 5.00L tank at 0.7°C is filled with 16.5g of dinitrogen difluoride gas and 5.00g of sulfur tetrafluoride gas. You can assume both gases behave as ideal gases under these conditions. "

First we calculate the moles of each gas, using their molar mass:

16.5 g N₂F₂ ÷ 66 g/mol = 0.25 mol N₂F₂5.00 g SF₄ ÷ 108 g/mol = 0.0463 mol SF₄

Total mol number = 0.25 + 0.0463 = 0.2963 mol

Mole Fraction N₂F₂ = 0.25/0.2963 = 0.84Mole Fraction SF₄ = 0.0463/0.2963 = 0.16

Now we use PV=nRT to calculate the partial pressure of each gas:

P = ?

V = 5.00 L

T = 0.7 °C ⇒ 0.7 + 273.16 = 273.86 K

For N₂F₂:

P * 5.00 L = 0.25 mol * 0.082 atm·L·mol⁻¹·K⁻¹ * 273.86 KP = 1.12 atm

For SF₄:

P * 5.00 L = 0.0463 mol * 0.082 atm·L·mol⁻¹·K⁻¹ * 273.86 KP = 0.208 atm

Yapo 13 fool coming at you for it

The answer should be vaporization