a) 22.4

**Answer 1**

XeF6 is Xenon hexafluoride….

6 atoms F per 1 molecule XeF6.. right?

6 moles F per 1 mole XeF6

so that…

3.2 moles XeF6 x (6 mole F / 1 mole XeF6) = 19.2 moles F

Answer is “D”

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your problem is with “moles”.. If you read this answer of mine and want some help with moles, ask in the “additional info” box.

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now.. in case you’re wondering, if you do as Norrie did…

you did this…

(g F / mole) / (g XeF6 / mole) x moles XeF6

= (g F / g XeF6) x moles XeF6

= g F x (moles XeF6 / g XeF6)

= g F x 1 / mw XeF6

= g F / mw XeF6…

not moles F

**Answer 2**

Well, the answer is D. No need to add up atomic wts, as done in a previous answer. Look at it this way. One mole of XeF6 contains 1 moles of Xe and 6 moles of F. So, 3.2 moles of XeF6 will have 3.2 moles of Xe and 19.2 moles of F. So the answer is D.

**Answer 3**

I make it ‘e).’ none of the above.

XeF6 mol mass = 131 + (6 x 19) = 131 + 114 = 245g/mol.

Moles of Fluorine (114g/mol / 245g/mol) x 3.2moles.

= 1.5 moles of F.