The question is incomplete, the complete question is;
Zinc and sulfur react to form zinc sulfide by the equation shown below. How many grams of ZnS can be formed when 12.0 g of Zn reacts with 6.50 g of S? (Atomic mass: Zn = 65.38, S = 32.06).
Answer:
17.5 g of ZNS
Step-by-step explanation:
The equation of the reaction is;
Zn(s) + S(s) ------->ZnS(s)
Number of moles of Zn = 12.0/65.38 = 0.18 moles
Number of moles of S = 6.50/32.06 = 0.20 moles
Hence Zn is the limiting reactant
If 1 mole of Zn yields 1 mole of ZnS
Then 0.18 moles of Zn also yields 0.18 moles of ZnS
Mass of ZnS produced = 0.18 moles * 97.44 g/mol = 17.5 g of ZNS