Conservation of Mass
Chapter 10
 State the “Law of Conservation of Mass”.
 What are the steps to balance a chemical equation?
 Identify parts of a chemical reaction (such as reactants, products).
 How are coefficients and subscripts different?
 Practice:
o
o
o
o
o
HgO → Hg + O2
Fe + O2 → Fe2O3
C3H8 + O2 → CO2 + H2O
CH3CH2OH + O2 → CO2 + H2O
Al + CuSO4 → Cu + Al2(SO4)3
Chapter 11
 How is a mole similar to a dozen?
 Why do chemists use the mole? (hint: talk about conversion)
 How is 1 mole of cars similar to 1 mole of CO2 molecules?
 How many grams of carbon are there in one mole? in 0.5 mole?
 Explain how a mole of any two differing objects are similar but yet different.
 How many atoms of carbon are there in one mole? in 0.5 mole?
 What contains more molecules, 10 moles of H2O or 10 moles of C6H12O6?
Explain your answer.
 What contains more atoms, 2g of Hydrogen or 6g of Carbon?
 Where do you find the molar mass of any substance? How many moles is it
worth?
 Arrange the following in order of smallest to largest:
(88gCO2) (6.02 x 1023 molecules of H2O) (1.5 moles CH4) (6.02 x 1024 molecules of
NaCl)
Chapter 12
 In balanced chemical equations, coefficients are also called _________?
 What are mole ratios used for?
 What is the first step in stoichiometry problems?
 Practice:
N2 + O2 → NO
 How many moles of NO are produced from 2.00 moles of nitrogen?
 How many grams of NO are produced from 0.5 moles of nitrogen?
 How many grams of NO are produced from 56 grams of nitrogen?
Solutions
Chapter 16
 What are parts to a solution?
 What are two types of mixtures?
 Like dissolves like rule.
 What is concentration? How do we measure concentration? Write the equations
Thermodynamics
Chapter 17
Movement of heat
 What is temperature?
 What is heat?
 Explain how heat moves.
 Compare & Contrast the terms: system, surrounding, and universe.
o In the following picture, a scientist is studying the solution in the flask.
The solution is very hot. Describe (using terms: system, surrounding and
universe) how heat flows.
Endo-vs-Exothermic
 Define the following thermodynamic processes, exothermic, and endothermic.
 Identify which process is responsible for forming bonds. Which is responsible for
breaking them?
 Identify the following reactions as exothermic or endothermic. Explain two ways
you can tell.
o NH3(g)  NH3(l) +heat
ΔHrxn= -1983kJ
o C2H5OH(l) + heat  C2H5OH(g)
ΔHrxn= 205kJ
 Draw the graphs of each thermodynamic process.
o Identify the following in the graph: energy axis, reactants, and products.
o Draw an arrow connecting the reactants and products that show enthalpy
(ΔH).
Phase changes
 Identify the phase changes that require (absorb) energy.
o What thermodynamic process is this?
 Identify the phase changes that release (lose) energy.
o What thermodynamic process is this?
 Explain how bond (intermolecular forces) strength is related to absorbing or
releasing energy.
Math Calculation
 Identify the equation that relates heat with temperature change. Identify all
variables.
 Identify the equation that is used to find phase change. Identify all variables.
 How does the value of heat differ between endothermic and exothermic
reactions?
 Identify the S.I. unit for heat.
 What does specific heat (c) describe? What are the units of specific heat?
 Know how to draw a heating curve of water and use it to calculate problems.
Reaction Rate Review
Chapter 17
What is it?
 Define reaction rate.
 Identify the three requirements of the collision theory.
 Know the rate laws.
Factors
 Identify and explain the factors affecting reaction rates.
o Note: with gas reactants, increasing pressure is the same as increasing
concentrating.
 Does changing pressure have any affect on a reaction that does not have
gas molecules?
 What is a catalyst? Explain what it does to reaction rates.
Role of activation energy
 Know how to draw and identify parts of an EXOTHERMIC and
ENDOTHERMIC graph such as:
o Reactants, products, activated complex/transition state, activation energy, and
energy of reaction.
 Describe an activated complex/transition state.
 What is activation energy?
Equilibrium Review
Chapter 18
 Explain what equilibrium is.
o Why is reversibility an important concept in equilibrium?
o Compare forward and reverse reactions (be able to identify reactants and
products).
o How does rate apply in chemical equilibrium?
 Know Le Châtelier’s Principle.
o Know the type stresses that are placed on chemical reactions.
o Be able to identify the reaction shift when stress is applied.
 Be able to write and solve equilibrium constants for chemical reactions at
equilibrium.
o Remember that solids and liquids are constant in reactions.
Study over the weekend! The more study time you put in the better the grade. Come to
tutorial or after school for help. Good luck and relax. You can do it!