A 400 L container at temperature of 4 celsius initially contains 0.25 mol He gas. Molecular hydrogen, which is a gas at 4 celsius is added until total pressure is 9.38*10^-2 atm. What is the partial pressure of the molecular hydrogen in the container?© BrainMass Inc. brainmass.com March 4, 2021, 6:02 pm ad1c9bdddf
* denotes multiplication
^ denotes power
Volume=V= 400 L
No of moles=n= 0.25 mol
Temperature= T= 4 C= 277.15 K =273.15+4
Ideal gas Law is PV=nRT
R= Gas constant= 0.082058 L.atm.mol ^-1K ^-1
P=Pressure= 0.0142140 atm =(0.25*0.082058*277.15)/400
Thus the calculation of pressure of Helium is correct
In a mixture of two ...
The solution calculates partial pressure.