Sulfur hexafluoride can be synthesized by burning sulfur with fluorine. What is the percent yield of the reaction if 76.8 g of sulfur hexafluoride is recovered from the combustion of 28.7 g of sulfur? S8(s) + 24 F2(g) → 8 SF6 (g)

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Answer 1 · 2017-09-20T16:44:36

Approx. #60%#.........

Well, let's make it a little easier by writing the stoichiometric equation as.....

#1/8S_8(s) + 3F_2(g) rarr SF_6#

We assume, reasonably, that fluorine gas was in excess....

And #"% yield"# #=# #(8xx"Moles of sulfur hexafluoride")/"Moles of sulfur"xx100%#

#"% yield"=(8xx(76.8*g)/(146.06*g*mol^-1))/((28.7*g)/(32.06*g*mol^-1))xx100%=58.7%#

It of course would be the same had I formulated the reaction as....

#S(s) + 3F_2(g) rarrSF_6#

#"% yield"=((76.8*g)/(146.06*g*mol^-1))/((28.7*g)/(32.06*g*mol^-1))xx100%=58.7%#

Do you follow my reasoning?