Asked by Wright, Easton

S8 (s) + 24 F2 (g) → 8 SF6 (g)

Typical Stoichiometry Problem :

Starting with 100 g of Sulfur…

How much MASS of Sulfur hexafluoride ( SF6 ) would be produced?
Answered by DrBob222
S8 (s) + 24 F2 (g) → 8 SF6 (g)
moles S = grams/molar mass = 100/8*32 = 0.39
moles SF6 produced = 0.39 mols S8 x (8 moles SF6/1 mol S8) = 3.125
grams SF6 = moles SF6 x molar mass SF6 = ?
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