Major Points and Concepts
Objectives:
- mole-mole relationships
- determining mole ratios
- using mole rations in equations
- mass calculations
- using mass-mole conversions with mole ratios
- stoichiometric calculations: comparing two ratios
- identifying limited reactants
- percent yield
- -theoretical number- amount of product predicted from the amounts of reactants used
- -actual number- amount of product actually obtained
- -percent yield- comparison using theoretical and actual yields
- -equation: (actual yield/theoretical yield) x 100 = percent yield
Example Calculations
determining mole ratios/using mole ratios in equations
-mole ratios are the factors in going from one compound to the other
example: determine the number of moles of O2 required to react with 4.30 mol C3H8.
-mole ratios are the factors in going from one compound to the other
example: determine the number of moles of O2 required to react with 4.30 mol C3H8.
mass calculations/using mass-mole conversions with mole ratios:
what are the grams of carbon dioxide required to react exactly with 50.4g of propane?
what are the grams of carbon dioxide required to react exactly with 50.4g of propane?
percent yield equations:
What is the percent yield for a reaction if you predicted the formation of 21. grams of C6H12 and actually recovered only 3.8 grams?
What is the percent yield for a reaction if you predicted the formation of 21. grams of C6H12 and actually recovered only 3.8 grams?
limited reactant problem:
2.00g of NaCl reacts with 5.00g of AgNO3 to form NaNO3 and AgCl. What is the limited reagent?
2.00g of NaCl reacts with 5.00g of AgNO3 to form NaNO3 and AgCl. What is the limited reagent?