Dr. Eric R. Johnson CHEM 111 Chapter 5 Objectives (Chang 9)
Be able to do the following:
1. Know that the noble gases (He, Ne, Ar, Kr, Xe, Rn), H2, N2, O2, F2, Cl2, and O3 exist as gases at room temperature
and pressure (25°C, 1 atm pressure).
2. Know the units for gas pressure (mmHg, torr, atm). Know that 1 atm = 760 mmHg. Know how to convert between
mmHg or torr and atm.
3. State Boyle's Law, Charles' and Gay-Lussac's Law; and the relationship between pressure and temperature using
both words and mathematical formulas.
4. Give the mathematical expression for the combined gas law. Given appropriate information about the initial and
final states, be able to use the combined gas law to calculate initial or final pressure, temperature or volume.
5. State Avogadro's Law. Describe the relationship between moles and volumes of gases.
6. Know that STP for gases refers to 273.15 K and 1.00 atm pressure (standard temperature and pressure). Know that
the volume of one mole of a gas at STP is 22.41 L.
7. State the ideal gas equation, and tell what unit is appropriate for each variable. Given values for R along with any
three of pressure, volume, moles, and temperature; be able to calculate the value for the fourth.
8. Know how to use the ideal gas equation and the molar mass of a gas to determine gas density.
9. Know how to use the ideal gas equation and the mass of a gas sample to determine the molar mass for the gas.
10. Know how to use the ideal gas equation to determine the number of moles of a gas. Know how to use this mole
data to solve stoichiometry problems.
11. Apply Dalton's Law of Partial Pressures to calculate the total pressure of a mixture of gases or the partial pressure
of a gas in a mixture of gases where the total pressure is known..
12. Know that the mole fraction (X) indicates concentration (XA = moles A / total moles).
13. Calculate the partial pressure of a gas from the total pressure and the mole fraction of the gas (PA = XA Ptotal)
14. Know that the pressure of a gas sample collected over water is the sum of the partial pressure of the gas and the
partial pressure of the water vapor.
15. Understand how the four postulates of the kinetic molecular theory of gases account for the behavior of gases.
16. Describe the relationship between molar mass of a gas and its rate of diffusion.
17. Know that real gases deviate from ideal behavior when one or more of the postulates of the kinetic molecular
theory of gases are no longer true.
18. Know that gases exhibit less ideal behavior at high pressures and low temperatures.
Assigned problems to work (These problems will not be collected): 5.1, 5.3, 5.13, 5.18, 5.20, 5.22, 5.24, 5.27, 5.28,
5.30, 5.32, 5.34, 5.36, 5.38, 5.40, 5.42, 5.44, 5.46, 5.48, 5.50, 5.52, 5.54, 5.58, 5.60, 5.62, 5.64, 5.66, 5.68, 5.72, 5.86,
5.94, 5.100, 5.114