Below is a list of topics which may appear on the hourly exam.  Not all topics listed will be on the exam, and some topics which are not on the list but included in the homework may appear.  Updated Feb 26, 2015

The exam will cover the topics, also covered in class and in the homework, from Chapters 11, 12 & 13, 14, & 19 .

Chapter 11:

Students should be able to:

• Describe the properties of gases
• List the assumptions of the kinetic molecular theory of gases
• Describe the difference between diffusion and effusion
• Understand the relationship between effusion and molecule mass
• Define the standard temperature and pressure (STP) and molar volume at STP
• Conduct unit conversions among all pressure units
• Differentiate between ideal and non-ideal gases
• List factors that may cause a gas to deviate from ideal behavior
• Use the relationships among P, V, T, and n in calculations
• Use the gas constant, R, in calculations
• Use the ideal gas law to determine density or molar mass
• Define mole fraction
• State Dalton’s Law of Partial Pressures in words or symbols
• Perform gas mixture calculations using Dalton’s Law of Partial Pressures and mole fractions
• Perform stoichiometric calculations for reactions with gaseous reactants and/or products.

The relationship between molar mass and relative velocity of gaseous molecules will be provided, along with the Ideal gas law. You will not be given equations for Boyles, Charles' law or Avogadro's law.

Chapters 12 & 13

Students should be able to:

• Describe or define the physical properties of liquids (surface tension, viscosity, vapor pressure, boiling point)
• Explain the relationship between intermolecular forces of attraction and the properties of liquids
• Describe the relationship between vapor pressure and temperature (The Classius-Clapeyron equation will be provided)
• Describe the physical properties of solids (melting point, vapor pressure)
• Describe the relationship between the bonding and structure of forms of carbon and its properties.
• Interpret phase diagrams.
• Identify phase changes and their associated enthalpies
• Interpret heating/cooling curves
• Calculate heat(q) changes with temperature and/or phase changes

Chapter 14

Students should be able to:

• Describe types of solutions, including all phases
• Describe saturation states of a solution (saturated, unsaturated, supersaturated) 
• Describe energy changes (thermodynamic) when solutions are formed
• Calculate concentration in a variety of ways (molarity, molality, and %mass vs % by volume)
• Use concentration to perform stoichiometric calculations
• Describe how environmental factors (T and P) affect solubility 
• Explain and calculate different physical properties between solutions and pure solvent (colligative properties)
• vapor pressure lowering
• boiling point elevation elevation
• freezing point depression
• osmotic pressure
• Use the colligative properties to calculate the molar mass of an unknown solute
• Predict the van't Hoff factor for a given solute and solvent
• Explain why the van't Hoff factor may vary from the predicted value
• Determine the percent ionization of an electrolyte from colligative properties

Chapter 19

Students should be able to:

• Distinguish between a spontaneous and a nonspontaneous process
• Define entropy (S)
• Recognize the conditions necessary for standard entropy (S°)
• Identify trends in standard entropy values
• Calculate the standard entropy change (ΔS°) for a given reaction
• Predict the sign of ΔS for a given process and use the sign to indicate whether the system has undergone an increase or decrease in entropy
• State in words or symbols the second law of thermodynamics
• Define Gibbs free energy (G)
• Calculate ΔG from temperature, ΔH,and ΔS
• Use  the sign of ΔG to indicate if a process is spontaneous
• Predict the sign of ΔG given the signs of ΔH and ΔS at high and low temperatures
• Recognize the conditions necessary for standard free energy of formation (G°_f)
• Calculate the standard free energy change (ΔG°) of a given reaction
• Calculate the temperature at which a process becomes spontaneous

Equations:  The relationship between molar mass and relative velocity of gaseous molecules will be provided, along with the Ideal gas law. You will not be given equations for Boyles, Charles' law or Avogadro's law. I will provide any of the formulas for the colligative properties (vapor pressure, melting point change, freezing point change or osmotic pressure).  You will need to know what the symbols (m, M, i, X, etc.) stand for.  All physical constants needed will be provided to you. You should learn the relationship: ΔG = ΔH - TΔS.