1. Ideal Gas Law:

* The ideal gas law is a good approximation for gases under normal conditions. It states: PV = nRT

* P = Pressure (in Pascals)

* V = Volume (in cubic meters)

* n = Number of moles

* R = Ideal gas constant (8.314 J/mol·K)

* T = Temperature (in Kelvin)

2. Convert Units:

* Volume: 150 liters = 0.15 cubic meters (1 liter = 0.001 cubic meters)

* Assume Standard Temperature and Pressure (STP):

* Temperature (T) = 273.15 K (0°C)

* Pressure (P) = 101325 Pa (1 atm)

3. Solve for Moles (n):

* Rearrange the ideal gas law equation: n = (PV) / (RT)

* Substitute the values: n = (101325 Pa * 0.15 m³) / (8.314 J/mol·K * 273.15 K)

* Calculate: n ≈ 6.68 moles of nitrogen gas

4. Calculate Mass:

* Molar mass of N₂: 28.01 g/mol

* Mass = moles * molar mass: Mass ≈ 6.68 mol * 28.01 g/mol ≈ 187.05 g

Therefore, the mass of 150 liters of nitrogen gas at STP is approximately 187.05 grams.