What is the mass of 2 litres of nitrogen at 22.4 atmosphere pressure and 273k?

Question

Answer

Use ideal gas equation.PV=nRT
mass will be 14n amu

Answer

Calculating the mass of nitrogen at given conditions:

- Given data:
- Volume (V) = 2 liters
- Pressure (P) = 22.4 atm
- Temperature (T) = 273 K
- Molar mass of nitrogen (N2) = 28.02 g/mol

- Step 1: Convert pressure to atm to Pa:
- 1 atm = 101325 Pa
- Pressure (P) = 22.4 atm = 22.4 * 101325 Pa = 2259360 Pa

- Step 2: Use ideal gas law to calculate moles of nitrogen:
- Ideal Gas Law: PV = nRT
- n = PV / RT
- n = (2259360 Pa * 2 L) / (8.314 J/(mol*K) * 273 K)
- n ≈ 204.85 mol

- Step 3: Calculate the mass of nitrogen:
- Mass = moles * molar mass
- Mass = 204.85 mol * 28.02 g/mol
- Mass ≈ 5741.14 g

Therefore, the mass of 2 liters of nitrogen at 22.4 atm pressure and 273 K is approximately 5741.14 grams.

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