CHEMISTRY PROBLEM HELP? 10 POINTS ASAP?
Heating Zinc sulfide in the presence of oxygen yields the following: ZnS+O2 -> ZnO+SO2
If 1.72 mol of ZnS is heated in the presence of 3.04 mol of O2 which reactant will be used up?
Balance equation
Heating Zinc sulfide in the presence of oxygen yields the following: ZnS+O2 -> ZnO+SO2
If 1.72 mol of ZnS is heated in the presence of 3.04 mol of O2 which reactant will be used up?
Balance equation
Comments
You must start with a balanced equation:
2 ZnS + 3 O2 -> 2 ZnO + 2 SO2
Determine the limiting reactant:
Calculate the mole of O2 needed for the complete consumption of 1.72 mole ZnS.
Use the mole ratio from the balanced equation and do ratio and proportion to get the mole of O2 .
.
Upon calculation, 1.72 mole ZnS would react completely with 2.58 mole O2.
Since the required 2.58 mole of O2 by 1.72 mole ZnS is less than the mole of O2 available (which is 3.04 mole), then the O2 is in excess.
So limiting reactant is ZnS.
the answer would be 37Chromium Nitrate