Answer:
The partial pressure of nitrogen in the flask is 1.08 atm and the total pressure in the flask is 1.70 atm.
Explanation:
We must use the Ideal Gas Law to solve this:
Pressure . volume = n . R . T
T = T° in K → T°C + 273
17°C + 273 = 290K
n = moles
In a mixture, n is the total moles (Sum of each mol, from each gas)
Moles = Mass / Molar mass
Moles He = 0.738 g / 4g/m = 0.184 moles
Moles N₂ = 8.98 g / 28g/m = 0.320 moles
0.184 m + 0.320m = 0.504 moles
P . 7.03L = 0.504m . 0.082L.atm/ mol.K . 290K
P = (0.504m . 0.082L.atm/ mol.K . 290K) /7.03L
P = 1.70 atm - This is the total pressure.
To know the partial pressure of N₂ we can apply, the molar fraction:
Moles of N₂ / Total moles = Pressure N₂ / Total pressure
0.320m / 0.504m = Pressure N₂ / 1.70atm
(0.320m / 0.504m) . 1.70atm = Pressure N₂
1.08atm = Pressure N₂
