Stoichiometry Study Guide
Honors Chemistry Name: _____________________
Study Guide – Unit 8: Stoichiometry
Vocabulary – Give definitions and examples where applicable
1. Product
2. Reactant / Reagent
3. Theoretical Yield
4. Actual Yield
5. Percent Yield
6. Excess Reagent
7. Limiting Reagent
8. Law of Conservation of Matter
Short Answer – explain the following:
9. What is conserved in every balanced equation (multiple answers)?
10. What determines the mole ratio in a balanced equation?
11. What is the proper method to determine limiting reagents?
12. What is the relationship between the masses of products and reactants?
Practice problems:
13. Using the following equation: Fe2O3 + 3CO 3CO2 + 2Fe
a) How many grams CO are needed to react with excess Fe2O3 to produce 591g Fe?
b) What is the proper way to name Fe2O3?
14. Using the following equation: N2 + 3H2 2NH3 a) What is the limiting reagent when 100g of nitrogen reacts with 32.1g hydrogen? a b) How much excess reagent exists?
15. Using the following SKELETON equation: P4 + H2 PH3
a) Balance the above equation… what is the mole ratio?
b) What is the limiting reagent when 6.2 g P4 reacts with 4 g of H2?
c) How much PH3 could be formed from this reaction?
16. Using the following SKELETON equation: NH3 + O2 NO2 + H2O
a) Balance the above equation … what is the molecule ratio?
b) What is the ratio of moles of Oxygen used to moles of NO2 produced?
c) How many molecules of H2O are produced when 18.3 moles of NH3 are used (assume excess O2)?
17. Draw a particle picture to represent the equation in #16 (above) when given 4 molecules of NH3 and 8 molecules of O2 react to form NO2 and H2O
Study Guide – Unit 8: Stoichiometry
Vocabulary – Give definitions and examples where applicable
1. Product
2. Reactant / Reagent
3. Theoretical Yield
4. Actual Yield
5. Percent Yield
6. Excess Reagent
7. Limiting Reagent
8. Law of Conservation of Matter
Short Answer – explain the following:
9. What is conserved in every balanced equation (multiple answers)?
10. What determines the mole ratio in a balanced equation?
11. What is the proper method to determine limiting reagents?
12. What is the relationship between the masses of products and reactants?
Practice problems:
13. Using the following equation: Fe2O3 + 3CO 3CO2 + 2Fe
a) How many grams CO are needed to react with excess Fe2O3 to produce 591g Fe?
b) What is the proper way to name Fe2O3?
14. Using the following equation: N2 + 3H2 2NH3 a) What is the limiting reagent when 100g of nitrogen reacts with 32.1g hydrogen? a b) How much excess reagent exists?
15. Using the following SKELETON equation: P4 + H2 PH3
a) Balance the above equation… what is the mole ratio?
b) What is the limiting reagent when 6.2 g P4 reacts with 4 g of H2?
c) How much PH3 could be formed from this reaction?
16. Using the following SKELETON equation: NH3 + O2 NO2 + H2O
a) Balance the above equation … what is the molecule ratio?
b) What is the ratio of moles of Oxygen used to moles of NO2 produced?
c) How many molecules of H2O are produced when 18.3 moles of NH3 are used (assume excess O2)?
17. Draw a particle picture to represent the equation in #16 (above) when given 4 molecules of NH3 and 8 molecules of O2 react to form NO2 and H2O