Q. What is the molar mass of fluorine, \( \mathrm{F}_2 \)?

Q: What is the molar mass of fluorine gas, \mathrm{F_2} ?

\alpha = 2 \times 19.00 = 38.00\ \mathrm{g/mol} .

Q: Why is the answer not 19.00\ \mathrm{g/mol}?

19.00\ \mathrm{g/mol} is for atomic fluorine, \mathrm{F} , not diatomic \mathrm{F_2} .

Q: What is the atomic molar mass of fluorine, \mathrm{F} ?

From the periodic table, \mathrm{F} \approx 19.00\ \mathrm{g/mol} .

Q: How do you compute molar mass for a diatomic molecule like \mathrm{F_2} ?

Add masses of both atoms: M(\mathrm{F_2}) = 2 \times M(\mathrm{F}) .

Q: Which option is correct: 9.00, 18.00, 19.00, or 38.00\ \mathrm{g/mol}?

38.00\ \mathrm{g/mol} is correct.

Q: What units should molar mass have?

Molar mass is in \mathrm{g/mol} , since it’s mass per mole.

Q: What would \mathrm{F} (one atom) have as molar mass?

M(\mathrm{F}) = 19.00\ \mathrm{g/mol} .

Answer

Fluorine gas is diatomic: \( \mathrm{F_2} \). The atomic molar mass of fluorine is about \(19.00\ \mathrm{g/mol}\). So the molar mass of \( \mathrm{F_2} \) is \(2 \times 19.00 = 38.00\ \mathrm{g/mol}\).

\[ \mathrm{M(F_2)} = 2 \times 19.00\ \mathrm{g/mol} = 38.00\ \mathrm{g/mol} \]

Detailed Explanation

Step 1: Understand the species

The question asks for the molar mass of fluorine gas, which is given as \( \mathrm{F_2} \). That means each molecule contains two fluorine atoms.

Step 2: Use atomic molar mass of fluorine

The atomic molar mass of fluorine \( \mathrm{F} \) is approximately \( 19.00 \, \mathrm{g/mol} \).

Step 3: Add the mass of two fluorine atoms

Since \( \mathrm{F_2} \) contains 2 atoms, the molar mass is:

\[
\text{Molar mass of } \mathrm{F_2} = 2 \times (19.00 \, \mathrm{g/mol})
\]

Step 4: Perform the calculation

\[
\text{Molar mass of } \mathrm{F_2} = 38.00 \, \mathrm{g/mol}
\]

Final Answer

\( 38.00 \, \mathrm{g/mol} \)

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General Chemistry FAQs

What is the molar mass of fluorine gas, \( \mathrm{F_2} \)?

\( \alpha = 2 \times 19.00 = 38.00\ \mathrm{g/mol} \).

Why is the answer not \(19.00\ \mathrm{g/mol}\)?

\(19.00\ \mathrm{g/mol}\) is for atomic fluorine, \( \mathrm{F} \), not diatomic \( \mathrm{F_2} \).

What is the atomic molar mass of fluorine, \( \mathrm{F} \)?

From the periodic table, \( \mathrm{F} \approx 19.00\ \mathrm{g/mol} \).

How do you compute molar mass for a diatomic molecule like \( \mathrm{F_2} \)?

Add masses of both atoms: \( M(\mathrm{F_2}) = 2 \times M(\mathrm{F}) \).

Which option is correct: \(9.00\), \(18.00\), \(19.00\), or \(38.00\ \mathrm{g/mol}\)?

\(38.00\ \mathrm{g/mol}\) is correct.

What units should molar mass have?

Molar mass is in \( \mathrm{g/mol} \), since it’s mass per mole.

What would \( \mathrm{F} \) (one atom) have as molar mass?

\( M(\mathrm{F}) = 19.00\ \mathrm{g/mol} \).

The molar mass of F₂ is 38 g/mol.
Choose 38.00 g/mol.

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