If you started with 35.0 grams of h2s and 40.0 grams of o2, how many grams of s8 would be produced, assuming 95 % yield? 8h2s(g)+4o2(g)→s8(l)+8h2o(g)

Molar mass

H2S = 34.0 g/mol
O2 = 31.99 g/mol
S8 = 256.52 g/mol

Identifying excess reagent and the limiting of the reaction :

8 H2S(g) + 4 O2(g) = S8(I) +  8 H2O(g)

8 x 34 g H2S >  256. 52 g S8
35.0 g > ??

35.0 x 256.52 / 8 x 34 =

8978.2 / 272 => 33.00 g of S8  

H2S is  the  limiting reactant


4 x 31.99 g O2 256.52 g S8
40.0 g O2 ??

40.0 x 256.52 / 4 x 31.99 =

10260.8 / 127.96 = 80.16 g of S8  

O2 is the excess reagent is the excess reagent



H2S is the limiting reactant, one that is fully consumed, it is he who determines the mass of S8 produced 

33.0 g 100%
?? g 95 %

95 x 33.00 / 100 => 31.35 g

hope this helps!

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