Unit 7: Stoichiometry Review
1. What is molar mass and how is it calculated?
2. What is a mole-mole ratio? Give an example.
3. What is the molar mass of sodium chlorate, NaClO3?
4. Find the molar mass of silver sulfide, Ag2S.
5. How many grams are found in 3.5 moles of Na3N?
6. A sample contains 15.2 liters of neon gas. How many moles are in the sample?
7. How many grams are represented by 0.76 moles of Ag2S?
8. What is the molar volume of a 1.7 mole sample of Ar at STP?
Al2O3 + 3 H2  2 Al + 3 H2O
9. How many moles of hydrogen gas are needed to produce 3.4 moles of aluminum?
10. How many liters of hydrogen gas are needed to produce 15.05 grams of water?
11. Calculate the mass of Al2O3 that is needed to react completely with hydrogen gas to produce 15.23 grams of
aluminum metal.
12. How many grams of water are produced if 22.6 grams of Al2O3 are consumed?
Unit 7: Stoichiometry Review
1. What is molar mass and how is it calculated?
2. What is a mole-mole ratio? Give an example.
3. What is the molar mass of sodium chlorate, NaClO3?
4. Find the molar mass of silver sulfide, Ag2S.
5. How many grams are found in 3.5 moles of Na3N?
6. A sample contains 15.2 liters of neon gas. How many moles are in the sample?
7. How many grams are represented by 0.76 moles of Ag2S?
8. What is the molar volume of a 1.7 mole sample of Ar at STP?
Al2O3 + 3 H2  2 Al + 3 H2O
9. How many moles of hydrogen gas are needed to produce 3.4 moles of aluminum?
10. How many liters of hydrogen gas are needed to produce 15.05 grams of water?
11. Calculate the mass of Al2O3 that is needed to react completely with hydrogen gas to produce 15.23 grams of
aluminum metal.
12. How many grams of water are produced if 22.6 grams of Al2O3 are consumed?