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Chapter 10, 11, and 12 Test Review Guide
Chapter 10 Review
Section 10.1: writing a word equation or formula (and balancing!)
1. When calcium hydroxide reacts with hydrochloric acid (aqueous hydrogen chloride) in water, dissolved calcium
chloride and water are formed.
2. When lithium hydroxide pellets are added to a solution of sulfuric acid (aqueous dihydrogensulfate), dissolved
lithium sulfate and water are formed.
Balancing equations
Key Terms (be able to explain each one, NOT just give the analogy)
Synthesis:
Combustion:
Decomposition:
Complete ionic equation:
Single Displacement:
Net ionic equation:
Double Displacement:
Predict products, use state symbols, and identify type of reaction (given JUST reactants) (and balance)
4)
____ C5H9O (l) + ____ O2 (g) 
Type: _______________________
5)
____ Pb (s) + ____ H3PO4 (aq)
Type: _______________________
6)
____ Li3N (aq) + ____ NH4NO3 (aq)
Type: _______________________
7)
____ Na2O (s) 
Type: _______________________
8)
____ N2 (g) + ____ O2 (g) 
Type: _______________________
Chapter 11
Define these Key Terms:
Mole Avagadro’s Number Molar Mass –
Empirical formulaMolecular formulaHydrateFill in the appropriate numbers for following conversion factors:
Know how to do the following calculations:
1. Molar Mass Calculations
Ex: calculate the molar mass of NaCl (answer = 58.44 g/mol)
2. Moles to Particles (atoms, molecules, formula units, ions, etc)
Ex: Calculate the number of particles from the following quantity: 11.5 moles of potassium
bromide (answer = 6.92 * 1024 formula units)
3. Moles to Mass
Ex: Determine the mass in grams in 3.35 moles of calcium (answer = 134 g)
4. Mass to Moles to Atoms
Ex: Calculate the number of moles in 6.35 g of lithium (answer = 0.915 moles)
5. Hydrate problems: A mass of 2.50 g of hydrated copper (II) sulfate is placed in a crucible
and heated. On heating, 1.59 g of white anhydrous copper (II) sulfate is left behind.
Determine the ratio of water to copper (II) sulfate. (answer = 5:1)
Chapter 12 Review Guide
Types of Problems
1. Converting between grams of one substance to grams of another (using molar mass)
Calcium carbide, CaC2, reacts with water to form acetylene. How many grams of water are needed to react with 485 g of CaC2?
CaC2 + 2H2O  C2H2 + Ca(OH)2
(ans = 273 g H2O)
2. Limiting reactant problems (aka calculate theoretical yield) “In the reaction CaC2 + 2H2O  C2H2 + Ca(OH)2, 64 g H2O is
reacted with 64 g CaC2. CaC2. Which is the excess reactant, which is limiting? What is the theoretical yield of C 2H2 ?
Limiting Reactant = __________
Excess Reactant = __________
Theoretical Yield = ____________
(ans = 26 g C2H2 prod)
3. Percent Yield Problems (do NOT have to determine Limiting Reactant for these ones!)
5a) If 156 g NaNO3 react and 112 g of NaNO2 are recovered, what is the percentage yield?
2NaNO3  2NaNO2 + O2
Actual yield = ____________________
Theoretical Yield = ________________
Percent Yield = ___________________
(ans = 88.4%)
3b) Reacting 9.91 mol of SiO2 with excess carbon yields 3.00 g of SiC. What is the percentage yield?
SiO2 + 3C  SiC + 2CO
Actual yield = ____________________
Theoretical Yield = ________________
Percent Yield = ___________________
(ans = 75.6%)
Definitions/Key Terms
Describe the following terms, using these questions to guide you:
- What is important to know about the term?
- What kind of calculations or conversion factors are they involved in?
- Do they have units?
stoichiometry:
actual yield:
percent yield:
limiting reactant:
molar mass:
excess reactant:
theoretical yield: