PERFORMANCE OBJECTIVES / Chem. B1A - Dr. Daniel 

Chapter 5 – Gases

 At the end of this unit you should be able to:

1.         Describe the nature of gases in terms of their particles, particle motion, and the properties of gases in general.

 

 2.        Define pressure.  Convert from one of the following pressure measurement to the others, Pascals, atmospheres, torr, and mm Hg.

 

 3.        Describe how mercury barometers measure pressure.

 

 4.        Explain how the concept of absolute temperature (Kelvin) arises from an examination of the volume versus temperature relationship of an ideal gas.

 

 5.        State mathematically and in words the relationship between P, V, T, and n with regard to gases.  Be able to sketch a typical plot of how two of the properties would vary while holding the other two properties constant.

 

 6.        Given the initial and final values of P, V, n, or T, for a gas behaving ideally, calculate the change in one property.   (i.e., use the combined gas law)

 

 7.        Use the ideal gas law to determine either P, V, n, or T.  Use this information to calculate the number of gas particles, mass, or the gas constant, when given the other quantities for any gas. 

 

 8.        State what standard temperature and pressure are for a gas.  What is the molar volume of a gas at STP? 

 

 9.        Apply Dalton's Law of partial pressures in given instances, (this includes vapor pressure of water).

 

 10.      State the major postulates of the Kinetic-Molecular Theory and use them to explain how two properties (P, V, n, or T) vary while the two remaining properties are held constant.  Use the KMT to explain Graham’s Law of Effusion and Dalton's Law of partial pressure.

 

 11.      State Graham's Law of Effusion, and apply it to calculate relative rates of effusion.  Define diffusion and discuss how it is related to effusion.  Given relative rates of effusion for a know and unknown gas, calculate the unknown molar mass.

 

 13.      Given appropriate information, determine the molar mass or density of a gas.  Use this information to determine the identity of a compound.

 

 14.      Perform stoichiometric calculation using gas properties, (P, V, n, T).

 

 15.      Explain under what conditions a real gases does not behave ideally.  Explain how the terms a and b correct for non-ideal behavior in van der Waal's equation.

 

 16.      Describe the factors which differentiate real from ideal gases.