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1 Ex exam 1    9/19

We now have an official Exam Procedure page. Check it out and know what to expect on Tuesday.

Coverage for Exam 1: Exam 1 covers all the material that was covered on LE's 00-08 and HW01 and HW02. Most of the exam is over Chapter 1 (Gases) from the gchem site. There will be about 3 questions that are "fundamentals" which means you would be balancing and equation and calculating stoichiometric quantities. Know that this exam is really about gases.

Length / Time for Exam 1: The exam will be between 15 and 20 multiple choice questions. The questions will have a range of point values from 5 points to 7 points. If very short (easy) questions are included, their point values will be 3 points. Point values are included with all questions. The exam is given during class time (9:30-10:45, 11-12:15) which is 75 minutes total which includes the handout time.

Not on Exam 1: Nomenclature. We have decided to push the testing of nomenclature to exam 2. Yes, you should be learning nomenclature each an every day - just no nomenclature questions on exam 1. Focus on gases.

Main Equations/Formulas for Exam 1

Ideal Gas Law: \[PV = nRT\]

Dalton's Law of Partial Pressures: \[P_{\rm total}= P_{\rm A} + P_{\rm B} + P_{\rm C} + \cdots \]

Kinetic Energy of an Ideal Gas: \[E_{\rm k} = {3\over 2} RT\]

Root Mean Squared Speed of particles: \[v_{\rm rms} = \sqrt{3RT\over M}\]

Van der Waal's Equation of State
\[\left(P+a{n^2 \over V^2}\right)(V-nb)=nRT\]

Learning Outcomes for Gases

Students will be able to...

  1. Describe pressure from a macroscopic and microscopic perspective.
  2. Relate Boyles, Charles', and Avogadro's gas laws to observations of gas behavior.
  3. Calculate the values for state functions (n, V, T, P) using the ideal gas equation.
  4. Define the conditions of STP and SATP.
  5. Relate the number density and mass density for a given gas, including quantitative calculations such as mass, molecular weight, and density.
  6. Relate partial pressures and the total pressure as described by Dalton’s Law of Partial Pressure.
  7. Apply the concept of the gas laws to gas phase reactions.
  8. Perform stoichiometric calculations using gas properties, masses, moles, limiting reagents, and percent yield.
  9. Relate kinetic energy to the temperature of a gas.
  10. Relate temperature, molar mass, and gas velocity.
  11. Describe the effect of molar mass and temperature on the Maxwell-Boltzmann gas velocity distribution.
  12. Apply kinetic molecular theory to a variety of gas phenomena including diffusion and effusion.
  13. Calculate relative effusion and diffusion rates using Graham’s Law.
  14. Explain the quantitative relationship between state functions (n, T, V, and P) as described by kinetic molecular theory.
  15. Describe macroscopic gas behavior using a small particle model of a gas.
  16. State when the ideal gas model fails to predict the behavior of gases observed in nature and in the laboratory.
  17. Explain what the breakdown of the ideal gas law reveals about the assumptions of kinetic molecular theory.
  18. Explain the general principles of the hard sphere model and van der Waal's model of gas.