Question

Question #a40ec

Answer 1

`"41.2 g"`

Explanation:

The balanced chemical equation that describes your reaction looks like this

`"S"_ (8(s)) + 24"F"_ (2(g)) -> 8"SF"_ (6(g))`

Notice that the reaction consumes `24` moles of fluorine gas for every `1` mole of octatomic sulfur that takes part in the reaction.

This means that in order for your sample of sulfur, which consists of

`11.6 color(red)(cancel(color(black)("g"))) * "1 mole S"_8/(256.52color(red)(cancel(color(black)("g")))) = "0.04522 moles S"_8`

to be completely consumed by the reaction, you need to provide

`0.04522 color(red)(cancel(color(black)("moles S"_8))) * "24 moles F"_2/(1color(red)(cancel(color(black)("mole S"_8)))) = "1.085 moles F"_2`

To convert the mass of fluorine gas to moles, use the molar mass of diatomic fluorine

`1.085 color(red)(cancel(color(black)("moles F"_2))) * "37.997 g"/(1color(red)(cancel(color(black)("mole F"_2)))) = color(darkgreen)(ul(color(black)("41.2 g")))`

The answer is rounded to three sig figs, the number of sig figs you have for the mass of sulfur.