What is the volume, in liters, of 62.3 g of nitrogen gas (N_2) at standard temperature and pressure (STP)?

• A. 49.7 L
• B. 22.4 L
• C. 31.2 L
• D. 62.3 L

Answer: (A)

Verified step by step guidance

1. Identify the molar mass of nitrogen gas (N\_2). Since nitrogen has an atomic mass of approximately 14.0 g/mol, calculate the molar mass of N\_2 by multiplying by 2: \(M = 2 \times 14.0\ \text{g/mol}\).
2. Convert the given mass of nitrogen gas (62.3 g) to moles using the molar mass: \(n = \frac{\text{mass}}{M} = \frac{62.3\ \text{g}}{M}\).
3. Recall that at standard temperature and pressure (STP), 1 mole of any ideal gas occupies 22.4 liters.
4. Calculate the volume of nitrogen gas by multiplying the number of moles by the molar volume at STP: \(V = n \times 22.4\ \text{L/mol}\).
5. Substitute the value of moles from step 2 into the volume equation to find the volume in liters.