Final answer:
Using Avogadro's law and the molar masses of the gases provided, N₂ is calculated to have a mass closest to 4g in a 2L container at STP, making N₂ the correct answer.
Step-by-step explanation:
The question asks which gas will have a mass of about 4g when 2L is contained at 0°C and 1 atm. According to Avogadro's Law, equal volumes of gases at the same temperature and pressure contain the same number of molecules, having the same number of moles. At standard temperature and pressure (STP), which is 0°C (273.15 K) and 1 atm, one mole of any ideal gas occupies 22.4 liters. Therefore, 2 liters of gas at STP is approximately 1/11.2 moles (2L / 22.4L/mol).
By using the molar masses of the gas options provided:
- SO₂: 64g/mol
- N₂: 28g/mol
- CO₂: 44g/mol
- C₄H₈: 56g/mol
- NH₃: 17g/mol
We can calculate the mass:
For N₂, the calculation would be (28g/mol) * (1/11.2 moles) ≈ approx. 2.5g, which is the closest to 4g. Therefore, option B) N₂ is the correct answer.