850.0 gra of flourine gas F2 is removed from a 200.0 L-tank ay 40.0 C° and 32.0 atm without changing the volume of temperature .Calculate the new pressure in the tank
Given the volume of the tank, V = 200.0 L
Temperature, T = 40.0 DegC = 40+273 = 313 K
Initial pressure, Pi = 32.0 atm
Initial moles of F2 gas, n1 can be calculated from ideal gas equation.
PV = n1RT
=> n1 = PV / RT
=> n1 = 32.0 atm x 200.0 L / (0.0821 L.atm.mol-1.K-1 x 313 K) = 249.05 mol
moles of F2 gas removed = mass / molar mass = 850.0 g / 38.0 g/mol = 21.8 mol
Hence final moles of F2 gas, n2 = 249.05 mol - 21.8 mol = 227.25 mol
Since V and T are constant,
P / n = constant
=> P1 / n1 = P2 / n2
=> 32.0 atm / 249.05 mol = P2 / 227.25 mol
=> P2 = 29.2 atm (answer)
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