Two gases of A and B having molar masses 60g and 45g respectively are enclosed in a vessel. The mass of A is 0.50g and that of B is 0.20g. The total pressure of the mixture is 750mm. Calculate the partial pressure of A and B gases respectively.
345.8mm, 260.7mm
589.2mm, 342.7mm
236.5mm, 432.5mm
487.5mm, 262.5mm
We have:
Molar mass of A = 60g and molar mass of B = 45g
Given mass of A = 0.50g and given mass of B = 0.20g
Now, the total pressure of the mixture
= 750mm
Now, moles of A = 0.50/60 = 0.0084 moles
And, moles of B = 0.20/45 = 0.0045 moles
Again, mole fraction of A = 0.0084/0.0129 = 0.65
And, mole fraction of B = 0.0045/0.0129 = 0.35
Thus, partial pressure of A ( ) = 750 x 0.65 = 487.5mm
Again, partial pressure of B( ) = 262.5mm
Therefore, Option(4) is correct