Which of the following is the mass in grams of 4.25 × 10^3 mol of N_2?

• A. 4.25 × 10^3 g
• B. 8.50 × 10^4 g
• C. 2.98 × 10^4 g
• D. 1.19 × 10^5 g

Answer: (D)

Verified step by step guidance

1. Identify the given quantity: 4.25 \times 10^{3} moles of N_2 (nitrogen gas).
2. Recall that to convert moles to grams, you need to use the molar mass of the substance. The molar mass of N_2 is calculated by summing the atomic masses of two nitrogen atoms.
3. Find the atomic mass of nitrogen (N) from the periodic table, which is approximately 14.0 g/mol. Therefore, the molar mass of N_2 is 2 \times 14.0 = 28.0 g/mol.
4. Use the formula to convert moles to grams: \(\text{mass (g)} = \text{moles} \times \text{molar mass (g/mol)}\).
5. Substitute the values: mass = (4.25 \times 10^{3} mol) \times (28.0 g/mol). This will give you the mass in grams of 4.25 \times 10^{3} moles of N_2.