Answer:
of zinc sulfide:
0.382 moles ZnS * 97.45 g/mol = 37.4 g ZnS
To find the mass of the excess reactant (sulfur) that will remain after the reaction is complete, we need to subtract the mass of the product (zinc sulfide) from the mass of the excess reactant:
30.0 g sulfur - 37.4 g ZnS = -7.4 g excess sulfur
Since the mass of the excess reactant is negative, this means that the reaction will consume all of the sulfur and there will be none left over.
To summarize:
A. Zinc is the limiting reactant.
B. 37.4 g of ZnS will be formed.
C. There will be no excess sulfur left over after the reaction is complete.
Step-by-step explanation: