Molar volume is the volume occupied by 1 mol of any (ideal) gas at standard temperature and pressure (STP: 1 atmospheric pressure, 0 °C). Show that it is 22.4 litres.

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What is the mass of 2 litres of nitrogen at 22.4 atmospheric pressure and 273 K

The correct option is C 28 gConsider STP conditions:1) 1 mol = 22.4 L of gas; 1 mol of Nitrogen gas = 14 g2) Therefore, 22.4 L Nitrogen gas = 14 g → 2 L Nitrogen = 1.25 g3) This is at a standard pressure of 1 atm. So, 22.4 atm pressure corresponds to 22.4 × 1.25 = 28 g

What is the mass of $2$ litres of nitrogen at $22.4$ atmospheric pressure and $273 K$

The correct option is C $28 g$
Consider STP conditions:
1) 1 mol = 22.4 L of gas; 1 mol of Nitrogen gas = 14 g
2) Therefore, 22.4 L Nitrogen gas = 14 g → 2 L Nitrogen = 1.25 g
3) This is at a standard pressure of 1 atm. So, 22.4 atm pressure corresponds to 22.4 × 1.25 = 28 g