Elemental sulfur occurs as octatomie molecules, #S_8#. What mass of fluorine gas is needed to react completely with 28.6 g of sulfur to form sulfar hexafluoride?

Question

Elemental sulfur occurs as octatomie molecules, #S_8#.  What mass of fluorine gas is needed to react completely with 28.6 g of sulfur to form sulfar hexafluoride?

Serenity Allen · Accepted Answer

Approx. #100*g#.

(i) A stoichiometric equation is required. #S(s) + 3F_2(g) rarr SF_6(g)#. And (ii) the molar equivalence of sulfur and fluorine #=# #(28.6*g)/(32.06*g*mol^-1)# #=# #0.892*mol#. And thus #0.892xx3xx38.00*g*mol^-1# #~=# #100*g# fluorine gas are required. Just a note on the molecularity of sulfur, of course I could have treated it as #S_8# as you did. The arithmetic is a bit easier if I give the equation as written above: 3 equiv of fluorine gas react with 1 equiv of sulfur. Note that fluorine, like all the other elemental gases (SAVE FOR THE NOBLE GASES), is binuclear, i.e. a diatomic molecule.

Olivia Anton · Answer

undefined To determine the mass of fluorine gas needed to react completely with 28.6 g of sulfur to form sulfur hexafluoride (SF6), we first need to balance the chemical equation for the reaction between sulfur and fluorine:

S8 + 24F2 → 8SF6

From the balanced equation, we can see that 24 moles of fluorine (F2) react with 1 mole of sulfur (S8) to produce 8 moles of sulfur hexafluoride (SF6).

Now, let's calculate the molar mass of sulfur (S8) and sulfur hexafluoride (SF6):

Molar mass of S8 = 8 × atomic mass of sulfur = 8 × 32.06 g/mol = 256.48 g/mol
Molar mass of SF6 = atomic mass of sulfur + 6 × atomic mass of fluorine = 32.06 g/mol + 6 × 19.00 g/mol = 146.06 g/mol

Now, let's calculate the number of moles of sulfur (S8) in 28.6 g:

Number of moles of S8 = mass / molar mass = 28.6 g / 256.48 g/mo