Question

A 8.00 L tank at 1.88 °C is filled with 2.53 g of dinitrogen difluoride gas and 5.50 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. Be sure your answers have the correct number of significant digits. mole fraction: dinitrogen difluoride partial pressure: atmx ? mole fraction: chlorine pentafluoride partial pressure: | atm Total pressure in tank: | atm

Answer 1

N2F2(dinitrogen difluoride)

Moles of N2F2= 2.53/66.0 => 0.0383 mol

Moles of ClF5 = 5.50/130.4 => 0.0422 mol

Mole fraction of N2F2 = 0.0383/(0.0383+0.0422) => 0.476

Partial pressure of N2F2

P = nRT/V

= 0.0383×0.0821×274.88/8.00 => 0.108 atm

Mole fraction of ClF5 = 1-0.476 => 0.524

Partial pressure of ClF5

P = 0.0422×0.0821×274.88/8

=> 0.119 atm

Total pressure = 0.119+0.108 = 0.227 atm

Dinitrogen difluoride

Mole fraction = 0.476

Partial pressure = 0.108 atm

Chlorine Penta fluoride

Mole fraction = 0.524

Partial pressure = 0.119 atm

Total pressure = 0.227 atm