Calculating partial pressure in a gas mixture

Question

A 9.00L

 tank at 23.5°C

 is filled with 3.33g

 of dinitrogen difluoride gas and 9.45g

 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.

dinitrogen difluoride	mole fraction:
partial pressure:	atm
dinitrogen monoxide	mole fraction:
partial pressure:	atm
Total pressure in tank:	atm

Answer 1

(3.33 g N2F2)(1 mole N2F2 / 66.01 g N2F2) = 0.05 moles N2F2

(9.45g N2O) (1 mole N2O / 44.01 g N2O) = 0.21 moles N2)

Mole Fraction of N2F2 = [(0.05 moles N2F2 ) / (0.05 moles + 0.21 moles)] = .192

Mole Fraction of N2O = [(0.21 moles N2O) / (0.05 moles + 0.21 moles)] = .808

Partial Pressure N2F2 = (nRT)/V = [(0.05 moles)(0.0821)(296.5K)] / 9.0L = 0.135 atm

Partial Pressure N2O = (nRT)/V = [(0.21 moles)(0.0821)(296.5K)] / 9.0L = 0.568 atm

Total Pressure in Tank = 0.135 atm + 0.568 atm = 0.703atm