Answer:
1190.2 Torr
Explanation:
Data Given:
Volume of a nitrogen gas ( V )= 4.0 L
temperature of a gas ( T ) = 24 °C
Convert °C to K
T = °C + 273
T = 24 + 273 = 297 K
mass of nitrogen gas (m) = 7.2 g
Pressure of a gas ( P ) =? in Torr
Solution:
Formula to be used
PV= nRT . . . . . . .(1)
As we Know
n= m/M
So, the equation 1 can be written as
PV = (m/M)RT
Rearrange the above formula
P = (m/M)RT / V . . . . . . . . . . (2)
Where
R is ideal gas constant
R = 62.37 L Torr mol⁻¹ K⁻¹
M = molar mass of N₂
molar mass of N₂ = 2(14) = 28 g/mol
m = mass of N₂ gas
Put values in equation 1
P = (m/M)RT / V
P = (7.2 g / 28 g/mol) 62.37 L Torr mol⁻¹ K⁻¹ x 297 K / 4.0 L
P = 0.257 mol x 62.37 L Torr mol⁻¹ K⁻¹ x 297 K /4.0 L
P = 4761 L Torr / 4.0 L
P = 1190.2 Torr
Pressure of gas (N₂) = 1190.2 Torr
