Sulfur combines with iron to form iron(ii) sulfide. in an experiment, 15.24 g of fe are allowed to react with 17.34 g of sulfur what is the limiting reactant? the reactant in excess? what mass of fes is created?

The balanced equation for the above reaction is as follows;
Fe + S ---> FeS
stoichiometry of Fe to S is 1:1
limiting reactant is the reagent that is fully consumed during the reaction and amount of product formed depends on amount of limiting reactant present.
excess reactant is provided in excess and only a fraction of the amount present initially is used up for the reaction.
Number of Fe moles - 15.24 g / 56 g/mol = 0.27 mol
Number of S moles - 17.34 g / 32 g/mol = 0.54 mol
according to molar ratio of 1:1
number of Fe moles are lower than S moles therefore;
 Fe is the limiting reactant 
0.27 mol of Fe reacts with 0.27 mol of S
S is excess reactant, number of moles in excess = 0.54  - 0.27 = 0.27 mol
molar ratio of Fe to FeS - 1:1
number of FeS moles formed - 0.27 mol 
Mass of FeS formed - 0.27 mol x 88 g/mol = 23.76 g

I’m pretty sure it’s false i’m not sure