Test 3 Review pt. 2

Test 3 Review pt. 2 - Dr McCord CHAPTER 5 Exam 3 Review...

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Chapter 5 – Which Sections for the Exam? Chapter 5: All sections except sections 5.11 and 5.12 were covered. Section 12 is an interesting section on atmospheric chemistry but we will not cover it. Also sections 6-9 have lots of technical proofs that will NOT be on the exam. Let me point you to the KEY parts of those sections. Note the 2 boxed formulas, one for kinetic energy and the other for rms particle velocity. Also, LOOK at the plot of a Maxwell-Boltzmann distribution and how the curve shifts with temperature (Figure 5.16). Know your definitions of effusion and diffusion plus the boxed equations relating velocity (rate) and mass and temperature (all of this is ON this review sheet too). Fundamentals Know how to calculate molar mass. Know your nomenclature (still). Be able to calculate amounts of reactants or products when given amounts of reactant or products – this is called stoichiometry – KNOW IT. See chapters 1-3 Know how to determine the limiting reactant and how much product it leads to. Be able to incorporate percent yield into a problem if necessary. All that is new is moles to P or V instead of grams. How to measure pressure Know the basics of how a manometer works and how a barometer works. Know how to calculate the pressure due to a standing column of liquid: P = dgh or P = ± gh d and ± (rho) are density. Watch your units here. Pressure will be in Pascals if you use kg/m 3 for density, and m for height. If the column is mercury, just get the height in mm and you’ve now got torr. Gas Laws Know the NAMES and the law associated with each name (scientist). Boyle’s Law: Pressure is inversely proportional to volume (assuming constant temperature and amount of gas, moles). Any units will work here. = constant Charles’ Law: Volume is directly proportional to absolute temperature (assuming constant pressure and amount of gas, moles). Any units for volume but remember, T must be Kelvin. = constant Avogadro’s Law: Volume is directly proportional to amount of gas in moles. (assuming constant temperature and pressure). = constant Combined Gas Law: Most books and people refer to this as Boyle’s Law + Charles’ Law which is (assuming constant n ) However, our book throw’s in Avogadro’s Law also giving: = constant which is fine, except that this is really just the Ideal Gas Law in disguise. The constant that is defined by this version of the combined gas law is the Universal
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This note was uploaded on 09/24/2010 for the course CH 301 taught by Professor Fakhreddine/lyon during the Spring '07 term at University of Texas.

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Test 3 Review pt. 2 - Dr McCord CHAPTER 5 Exam 3 Review...

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