Physics question....

Question

A tank contains 0.460kg of nitrogen gas at a pressure of 50.0 atm. What mass of oxygen would an identical tank contain, also at 50.0 atm and at the same temperature? The molar mass of Nitrogen is 28g/mol and that of oxygen is 32g/mol.

Answer 1

The relevant equation is the gas law

P*V=n*R*T

For the nitrogen, n = 0.46/28 = 0.0164 mole

at the same temperature, volume and pressure, the no of moles of gas in the tank is the same, so there are 0.0164 moles of oxygen in the tank

mass of oxygen is then 0.0164*32 = 0.526 g

EDIT:  Misread the mass of gas as g not kg.  Multiply the answer by 1000.

Answer 2

Neither Ideal or Combined Gas Law calculations are required for this.

32g/mol / 28g/mol = 1.143.

O2 is therefore 1.143 times the mass of Nitrogen.

460g x 1.143 = 526g = 0.526kg Oxygen.