Outline of Material for Exam 2
Chem 101, Summer 2006
Karyn Mlodnosky
1. Chemical Reactions (Ch. 6)
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Identify chemical changes versus physical changes
Balance chemical equations
Classify reactions as combination, decomposition, replacement (single or
double), combustion and/or redox
Given reactants, be able to write products with correct chemical formulas (for
simple reactions that follow the patterns of the 4 main reaction types)
Identify what is oxidized and what is reduced in redox reactions
Identify reactions as exothermic or endothermic
Interpret energy diagrams for chemical reactions (be able to label reactants,
products, transition state, activation energy and heat of reaction)
Identify factors that increase or decrease reaction rate
Know LeChâtelier’s Principle and identify factors that shift the equilibrium of a
reversible reaction towards products or towards reactants
Know (Table 4.8), Table 6.2, Table 6.3, Table 6.4, Table 6.6 and Table 6.7
2. Chemical Quantities (Ch. 7)
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Know Avogadro’s number and use it to convert between number of particles and
number of moles
Determine the molar mass of an atom or compound
Use molar mass to convert between grams and moles
Calculate percent composition by mass of a compound
Determine empirical formula from percent composition or masses
Use mole ratios from balanced chemical equations to relate moles of reactants
and products
Use mole ratios and molar masses to calculate grams of product or reactant
Given actual yield (in moles or grams) calculate percent yield of a reaction
Determine limiting reactant given moles or grams of reactants used
Be able to write an equilibrium expression for a reversible reaction
Given the equilibrium constant (Keq) determine if the equilibrium favors
products or reactants
3. Gases and Gas Laws (Ch. 8)
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List the 5 main points of the Kinetic Molecular Theory of Gases (p. 245)
Know units for the four variables that describe a gas (P, V, T and n)
Use Boyle’s Law (P and V), Charles’ Law (T and V) and Gay-Lussac’s Law (T and
P) to calculate one variable based on changes in the other variable
Use the combined gas law to find new P, V or T based on changes in the other
two variables
(Can derive any of the first 3 laws from the combined gas law)
Use Avogadro’s Law (V and n) and the molar volume of a gas at STP to calculate
V or n based on changes in the other variable
Use the ideal gas law to calculate P, V, T or n given values for the other three
variables
Calculate total P from partial P’s for a mixture of gases (or calculate a partial P
given the total P and other partial P’s); relate moles of gas to partial pressure
Note: you are responsible for knowing the formula for each law, and how to use
it, but not for the names of the laws
Know Table 8.1, Figure 8.2, Figure 8.3, Figure 8.4, Figure 8.5 and Table 8.6
4. Solutions (Ch. 9; section 9.4 will not be on the exam)
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Identify solvent and solute in a solution
Understand how solutions form (like dissolves like; solvation of ions in water)
Know terms homogeneous and heterogeneous
Classify solute as strong electrolyte, weak electrolyte or nonelectrolyte
Write equations for dissociation of strong and weak electrolytes
Use solubility to classify solutions as saturated or unsaturated
Calculate amount of solute of solvent in a saturated solution (given solubility)
Understand effects of temperature and pressure on solubility
Know solubility rules and use them to predict solubility of salts in water
Calculate solution concentrations using mass % (m/m), volume % (v/v) and
mass/volume % (m/v) and be able to use them as conversion factors
Calculate the molarity (M) of a solution and be able to use molarity as a
conversion factor (to determine moles of solute or volume of a solution)
Classify a mixture as a solution, colloid or suspension and know how to separate
them from each other
Understand osmosis and osmotic pressure
Classify solutions as isotonic, hypotonic or hypertonic and describe what
happens to a red blood cell placed in any of these solutions
Understand dialysis and use of semipermeable membranes
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Know Table 9.7, Table 9.12 and Figure 9.7