Learning Outcomes for UNIT 1

Each student should have a good grasp of the following learning outcomes for unit 1. Unit 1 is assessed on Exam 1 which is on Tuesday 9/13/11 from 7-9 PM. Read the bulleted points and self assess yourself on how well you know the topic.

Students will be able to...

• Perform stoichiometric calculations using masses, moles, limiting reagents, and percent yields.
• Apply the concept of the gas laws to gas phase reactions and perform stoichiometric calculations using gas properties, masses, moles, limiting reagents and percent yields.
• Explain and apply Boyles, Charles’, and Avogadro’s gas Laws to observations of gas behavior.
• Perform calculations using the ideal gas equation.
• Describe the concept of pressure from a macroscopic and microscopic perspective.
• Explain the relationship between the number density and mass density for a given gas.
• Perform calculations to determine the mole fractions of gases within and gas mixture and relate mole fraction to the partial pressure of a gas within a gas mixture.
• Describe the relationship between partial pressures and the total pressure as described in Dalton’s Law of Partial Pressure.
• Explain the relationship between kinetic energy and temperature of a gas.
• Explain the relationship between temperature and the velocity of a gas.
• Explain the relationship between molar mass and the velocity of a gas.
• Apply the ideas of kinetic molecular theory to a variety of gas phenomena.
• Describe the distribution of velocities for the particles in a gas sample and what factors affect this distribution.
• Explain how T, V, and n affect the pressure as described by kinetic molecular theory.
• Explain the general principles of the hard sphere model of a gas.
• Explain what the breakdown of the ideal gas law tells us about the assumptions of kinetic molecular theory.
• Explain when and why the ideal gas model fails to predict the behavior of gases observed in nature and in the laboratory.