What is the molar mass of molecular fluorine, F_2?

• A. 18.00 g/mol
• B. 9.00 g/mol
• C. 19.00 g/mol
• D. 38.00 g/mol

Answer: (A)

Verified step by step guidance

1. Identify the element involved: molecular fluorine, which is represented as \(\mathrm{F}_2\), meaning it consists of two fluorine atoms bonded together.
2. Find the atomic mass of a single fluorine atom from the periodic table. The atomic mass of fluorine (F) is approximately 19.00 g/mol.
3. Since molecular fluorine consists of two fluorine atoms, calculate the molar mass by multiplying the atomic mass of fluorine by 2: \(\text{Molar mass of } \mathrm{F}_2 = 2 \times 19.00 \ \mathrm{g/mol}\).
4. Write the formula explicitly: \(\mathrm{Molar\ mass\ of\ } \mathrm{F}_2 = 2 \times \mathrm{Atomic\ mass\ of\ F}\).
5. Perform the multiplication to find the molar mass of \(\mathrm{F}_2\) (do not calculate the final number here, just set up the expression).