Percent Composition and Finding Formula - Chemistry

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The discussion focuses on determining the formula of a sulfide formed from a reaction between sulfur and iron. Initially, 50.0g of sulfur is combined with 100.0g of iron, but 12.5g of iron remains unreacted after heating. The participants calculate the moles of each element, with iron yielding 1.79 moles and sulfur 1.56 moles. To find the ratio for the sulfide formula, the reacted mass of iron is calculated by subtracting the unreacted mass from the initial mass. The final step involves dividing the moles of each element to establish the simplest whole-number ratio for the formula.
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% Composition and Finding Formula - Chemistry

50.0g of Sulphur is mixed with 100.0g of iron and heated strongly. When the reaction is complete 12.5g of iron remains. What is the formula of the sulphide formed?

What i have done so far is i got the 2 mols of each element.

Fe=1.79
S=1.56

i divided biggest/smallest and i get 1.41
now i need to know how to put it in ratio form and what to do to find the formula for Sulphide
 
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it said 12.5g of Fe was unreacted!
 
Kushal said:
it said 12.5g of Fe was unreacted!

hmm so i should go 100-12.5 then find the mol then find the ratio?
 
yeah... this is it...

you divide the mass reacted by the respective atomic mass. then you find the ratio.
 
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