Chapter 11: Gases

DEFINE:

• Pressure – using molecular level and macro level examples
• Partial pressure
• Mole fraction
• Effusion and diffusion and state how they are different

DO:

• Qualitatively discuss the various simple gas law relationships in everyday life
• State the standard temperature and pressure (STP) used for gases (and how is this different from the standard state in thermodynamics)
• State the molar volume at STP
• State the three key assumptions of the kinetic theory of gases
• Use the kinetic theory of gases to explain the simple gas laws
• Explain the differences between ideal and non ideal gases by property and recognize situations where the ideal gas law may not be a valid approximation (Van der Waal’s Equation)

CALCULATE:

• Interconvert between the various units of pressure
• Use the ideal gas law to derive the relationship between

            Pressure and volume (Boyle’s Law)

            Volume and temperature (Charles Law)          

            Volume and moles (Avogadro’s Law)

• Use the ideal gas law for calculations involving T, P, V , n and molar mass
• The density of a gas from molar volume and molar mass at STP
• The density of a gas at a given temperature and pressure (via the ideal gas law)
• Use Dalton’s Law of Partial Pressures to calculate partial pressures of gases in a mixture (including the correction of gas pressure collected over water for the partial pressure of water vapor) or total pressure of a gas given the partial pressures
• Show the relationship between Dalton’s Law of Partial Pressures and mole fraction and use it in gas mixture calculations
• Use molar masses to calculate relative rates of effusion of gases (Graham’s Law) and vice versa
• Perform stoichiometric calculations for reactions with gaseous reactants or products

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