What is the density of fluorine gas (F_2) at standard temperature and pressure (STP)?

• A. 3.00 g/L
• B. 22.4 g/L
• C. 1.70 g/L
• D. 0.89 g/L

Answer: (C)

Verified step by step guidance

1. Recall that at standard temperature and pressure (STP), one mole of any ideal gas occupies 22.4 liters of volume.
2. Determine the molar mass of fluorine gas (F_2) by adding the atomic masses of two fluorine atoms. The atomic mass of fluorine (F) is approximately 19.00 g/mol, so the molar mass of F_2 is calculated as \$2 \times 19.00$ g/mol.
3. Use the formula for density of a gas at STP: \(\text{Density} = \frac{\text{Molar mass}}{\text{Molar volume}}\) where the molar volume at STP is 22.4 L/mol.
4. Substitute the molar mass of F_2 and the molar volume (22.4 L) into the density formula to set up the calculation: \(\text{Density} = \frac{2 \times 19.00 \text{ g/mol}}{22.4 \text{ L/mol}}\).
5. Perform the division to find the density in g/L, which will give you the density of fluorine gas at STP.