Given 3.2 moles of xenon hexafluoride (XeF_6), how many moles of fluorine atoms are present?

• A. 3.2 moles
• B. 0.53 moles
• C. 19.2 moles
• D. 6.0 moles

Answer: (C)

Verified step by step guidance

1. Identify the chemical formula of the compound given: xenon hexafluoride is \(\mathrm{XeF_6}\), which means each molecule contains 6 fluorine atoms.
2. Understand that the number of moles of fluorine atoms is related to the number of moles of \(\mathrm{XeF_6}\) molecules multiplied by the number of fluorine atoms per molecule.
3. Set up the calculation using the formula: \(\text{moles of fluorine atoms} = \text{moles of } \mathrm{XeF_6} \times 6\).
4. Substitute the given value of moles of \(\mathrm{XeF_6}\) into the formula: \$3.2 \text{ moles} \times 6$.
5. Perform the multiplication to find the total moles of fluorine atoms present in the sample.