*Unit 4 - Stoichiometry / Read / Complete / Assessment Scores
Standard 4.1 / Section 10.1 / p.323 1-8, 10, 13-14
WS: Atoms and Moles
Section 10.2 / p.328 15-21, p.332 22,26,27
Lab: Grams, Atoms, and Moles
WS: Grams, Atoms, and Moles
Section 10.3 / p.335 29-45, 47, 50
Read / Complete / Assessment Scores
Standard 4.2 / Section 10.4 / p.344 54-61, p.350 62-69, 73
Lab: Determining Empirical Formula
Read / Complete / Assessment Scores
Standard 4.3 / Section 11.2 / p.375 11-17, 21
WS: Stoichiometry Practice Problems
Section 11.3 / p.383 23-25, 27
Lab: Limiting Reactant
Section 11.4 / p.387 28-35
Lab: Percent Yield
WS: Limiting Reactant and Percent Yield Problems
*Unit 5– Solutions and Gases / Read / Complete / Assessment Scores
Standard 5.1 / Section 14.2 / WS: Solution Vocabulary
p.481 9-12, 16-22, p.488 33, 34
WS: Solution Problems
Lab: Vinegar Analysis
WS: Titration Problems
Read / Complete / Assessment Scores
Standard 5.2 / Section 13.2 / p.453 20-30, p.459 35, 36
Lab: Ideal Gas Law
WS: Ideal Gas Law problems
Section 13.1 / p.443 1-3, p.446 4-13, 16
Lab: Gas Relationships
WS: Changing Conditions
Read / Complete / Assessment Scores
Standard 5.3 / Section 13.3 / p.461 38-46, 48,
Lab: Eggshell Analysis
WS: Gas Stoichiometry
You must be able to do the following to achieve mastery:
Standard 4.1
- Know the difference between the 3 types of representative particles (atoms, molecules, formula units)
- Convert between representative particles and moles
Example: How many molecules of water are there in 6.5 moles of water?
- Convert between representative particles and grams
Example: Determine the mass, in grams, of 5.8 x 1022 atoms of sulfur.
- Convert between moles and grams
Example: Convert 200 grams of aluminum to moles.
- Determine the molar mass of a compound
Example: What is the molar mass of Sr(NO3)2?
- Determine the number of individual atoms in a specific mass of a compound
Example: How many chlorine atoms are present in 55 grams of AlCl3?
Standard 4.2
- Determine percent composition from a chemical formula
Example: Determine the percent by mass of each element in C6H12O6.
- Determine an empirical formula from percent composition
Example: A compound is found to contain 34.9 g of silver, 4.5 g of nitrogen, and 15.6 g of oxygen. Determine the empirical formula of the compound.
- Determine the molecular formula from an empirical formula and molar mass
Example: What is the molecular formula for a compound with a molar mass of 58.14 g and an empirical formula of C2H5?
Standard 4.3
- Solve basic stoichiometry problems
Example: How many grams of oxygen are produced when 2.50 g of hydrogen peroxide, H2O2, decomposes? 2H2O2 → 2H2O+ O2
- Determine the amount of product produced when multiple reactant amounts are given
Example: How many grams of Br2 are produced when 25.0 g of F2 react with 150 g of KBr?F2 + 2 KBr → Br2 + 2 KF
- Determine which reactant is the limiting reactant
Example: Which reactant is the limiting reactant in the previous problem?
- Determine the mass of an excess reactant that remains when a reaction is complete
Example: How many grams of F2 remain when the reaction above is complete?
- Determine the percent yield in a chemical reaction
Example: What is the percent yield if 35.5 g of Fe reacts with excess O2 to produce 48.6 g of Fe2O3? 4 Fe + 3 O2→ 2 Fe2O3
- Understand the factors that cause percent yield to be less than 100%.