Unit VI: Study Guide
Chapters 10, 11.4-11.6, and 13
To Know:
-Definitions of all vocabulary words in bold and all sentences in italics.
-Common compounds (and characteristics) of gases in table 10.1 on page 394.
-Conversion factors for various pressure units (bottom of page 396).
-Boyle’s law (10.2 on page 399)
-Charles’ law (10.3 on page 400)
-Avogadro’s law (10.4 on page 401)
-Combined gas law (10.8 on page 405)
-The ideal-gas equation (10.5 on page 402)
-Density equation (10.10 on page 407)
-The molar volume of an ideal gas at STP
-Dalton’s law (10.12 on page 410 or 10.15 on page 411)
-Kinetic molecular theory (not verbatim but generally) on page 414
-Root-mean-square equation (10.22 on page 417)
-Graham’s law (10.23 on page 418)
-The trends for effusion and diffusion
-Differences between real and ideal gases.
-Phase changes and names (figure 11.17 on page 449)
-Signs of enthalpies of various phase changes
-Relationship of vapor pressure to boiling point
-Energetics of solution formation (figure 13.4 on page 531)
-The process in forming a supersaturated solution
-Factors affecting solution formaton (solute-solvent interactions, pressure and
temperature)
-Units of concentration: Mass % (13.5 on page 542), ppm (13.6 on page 542), ppb, mole
fraction (13.7 on page 543), Molarity (13.8 pn page 543), and molality (13.9 on page
543).
-Raoult’s law (13.10 on page 547)
-Bp elevation and FP depression (13.11 on page 549 and 13.12 on page 550)
-Osmotic pressure equation (13.13 on page 553)
To Do:
-Convert between units of pressure (mm Hg, atm, torr, Pa or kPa).
-Calculate the effect of changes in variables on gases using the appropriate gas law.
-Use the ideal-gas equation to solve gas problems.
-Calculate the density or molar mass of a gas using equation 10.10.
-Perform stoichiometric calculations using gases.
-Use Dalton’s law to calculate partial or total pressures of a gas.
-Calculate mole fraction.
-Calculate partial pressures of gases collected over water.
-Calculate the rms speed of a molecule using equation 10.22.
-Use Graham’s law to calculate the rates of effusion or molar masses of a given gas.
-Predict the relative rates of effusion or diffusion for two gases.
-Use van der Waals equation to perform gas law calculations for real gases.
-Calculate enthalpies for changes in temperature or phase.
-Interpret a heating curve or phase diagram.
-Locate the triple point, critical point, normal melting/boiling point, regions of solid,
liquid, and gas states, and melting/boiling point at different pressures on a phase diagram.
-Predict the relative solubility of a solute in a given solvent.
-Perform calculations with and convert between units of concentration.
-Perform stoichiometric calculations using solutions.
-Calculate the lowering of vapor pressure by the addition of a nonvolatile solute using
Roault’s law.
-Calculate boiling point elevation and freezing point depression.
-Calculate the osmotic pressure of a solution using equation 13.13.