The compound sodium thiosulfate pentahydrate, Na2S2O3·5 H2O, is important commercially to the photography

The compound sodium thiosulfate pentahydrate, Na2S2O3·5 H2O, is important commercially to the photography business as "hypo," because it has the ability to dissolve unreacted silver salts from photographic film during development. Sodium thiosulfate pentahydrate can be produced by boiling elemental sulfur in an aqueous solution of sodium sulfite.

S8(s) + Na2SO3(aq) + H2O(l) Na2S2O3·5 H2O(s) (unbalanced)

What is the theoretical yield of sodium thiosulfate pentahydrate when 3.22 g of sulfur is boiled with 15.2 g of sodium sulfite?

Sodium thiosulfate pentahydrate is very soluble in water. What is the percent yield of the synthesis if a student doing this experiment is able to isolate (collect) only 11.7 g of the product?

Please help me

S8(s) + 8 Na2SO3(aq) → 8 Na2S2O3(aq)
(The water doesn't participate in the chemical reaction.)

(3.22 g S8) / (256.5240 g S8/mol) = 0.012552 mol S8
(15.2 g Na2SO3) / (126.0433 g Na2SO3/mol) = 0.12059 mol Na2SO3

0.012552 mole of S8 would react completely with 0.012552 x (8/1) = 0.10042 mole of Na2SO3 but there is more Na2SO3 present than that, so Na2SO3 is in excess and S8 is the limiting reactant.

(0.012552 mol S8) x (8/1) x (248.1854 g Na2S2O3·5 H2O/mol) =
24.9 g Na2S2O3·5 H2O

(The only time the five waters of hydration enter into this problem is when calculating the molar mass of Na2S2O3·5 H2O in the previous step.)

(11.7 g) / (24.9 g) = 0.470 = 47.0% yield