Final answer:
To find the volume occupied by 12 g of N₂ at room temperature and pressure, we calculate the number of moles and use the Ideal Gas Law. The calculations give us a volume of approximately 10.58 L, which does not exactly match the provided options, indicating a need for review or clarification of exam conditions.
Step-by-step explanation:
To determine what volume 12 g of nitrogen gas (N₂) will take up at room temperature and pressure, we can use the Ideal Gas Law, which is PV = nRT. Room temperature is assumed to be 25°C, which is 298K when converted to Kelvin (25 + 273). Using the molar mass of N₂ (28.01 g/mol), we first need to calculate the number of moles of N₂ that corresponds to the given mass.
n = mass / molar mass = 12 g / 28.01 g/mol = 0.42856 mol (approx).
Now we apply the Ideal Gas Law:
V = nRT / P
Assuming standard pressure (1 atm) and using the gas constant R (0.0821 L.atm.mol⁻¹.K⁻¹), we have:
V = (0.42856 mol) (0.0821 L.atm.mol⁻¹.K⁻¹) (298 K) / (1 atm)
This gives us:
V = 10.57809 L (approx)
However, the options provided do not include this answer, which suggests a possible need to review calculations or provided data. If the exam conditions stipulate rounding or a different standard temperature and pressure, this should be taken into account accordingly.