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by: Carmela Kilback


Carmela Kilback
GPA 3.92

A. Carroll

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A. Carroll
Class Notes
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This 2 page Class Notes was uploaded by Carmela Kilback on Wednesday September 9, 2015. The Class Notes belongs to CHEM 142 at University of Washington taught by A. Carroll in Fall. Since its upload, it has received 46 views. For similar materials see /class/192553/chem-142-university-of-washington in Chemistry at University of Washington.




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Date Created: 09/09/15
Chem 142B Aut10 List of Topics to Review for Exam 2 We have started applying the concepts we learned in Chapters 14 to new reactions and experimental conditions It is assumed for Exam 2 and future exams that you know ALL of the material on the Exam 1 topic list regardless of whether or not it showed up on Exam 1 You can expect to see comprehensive problems on future exams so please be sure that you keep those previous chapters in mind as you study work through problems and take the exam Types of Chemical Reactions and Solution Stoichiometry Chapter 4 sections 11 D Balancing oxidationreduction equations 0 Half reaction method andor oxidation state method you can use whichever you feel most comfortable with o Balancing reactions in acidic or basic solutions Gases Chapter 5 sections 110 B De nition and common units ofpressure the ones we 39Ve focused on in most ofour calculations D Instruments for measuring pressure how do you use the measurements from a manometerto determine the pressure of a gas or the atmosphere D Qualitative and quantitative evaluations of the laws from Boyle Charles and Avogadro as well as the ideal gas law 0 Variations of the form of the ideal gas law if you have or are looking for density or molar mass 0 Calculations involving change of conditions 0 Combining the gas laws with reaction stoichiometry use the gas laws to get the moles of reactants andor products and use the mole ratios from balanced reactions to find the amounts of reactantsproducts used up or produced D STP standard volume ony applies if you have 1 mole of substance at STP D Mole fractions and Dalton39s law ofpartial pressures 0 Also using partial pressures when considering a reaction for which a gaseous product is collected over water you ll have to be given the vapor pressure of water at a specified temperature D Kinetic Molecular Theory KMT o The four postulates of the KMT theory 0 Purpose of the KMT how does it support the experimentally determined ideal gas law 0 How to calculate kinetic energy KE of a molecule and KEavngr a mole of gas molecules watch your units 0 How to calculate the root mean square velocity most probably velocity and the average velocity watch your units 0 How do velocities kinetic energy force of impact etc change with mass of the particles number of particles temperature etc understand which variables affect these observed properties and understand how changes in the variables will translate to changes in the observed properties ie if temperature doubles what happens to D Effusion and Diffusion 0 Difference between effusion and diffusion 0 Relationship between rate of effusiondiffusion and molar mass of a gas 0 How to calculate the relative ratesvelocities of effusiondiffusion of two gases Collisions with container walls and other molecules 0 Factors that affect the number of collisions per second 0 See the last few slides of the lecture notes for the summary of what you are expected to know from these sections D Real vs ideal gases qualitative differentiation see the last slide of the Chapter 5 notes and the first three paragraphs of section 510 Chemical Equilibrium Chapter 6 sections 18 B Definitions ofequilibrium equilibrium position and equilibrium constant D How to write an equilibrium expression using concentrations or pressures be sure to understand why pure liquids and solids are not included know the relationship between K and Kp D How to rearrange the equilibrium expression and recalculate the quilibrium constant when the reaction is reversed multiplied by a factor etc D How to determine the apparent units ofthe equilibrium constant and why they are referred to as a pparentquot units D Determine the extent ofreaction and how to calculate the reaction quotient Q 0 Compare Q with K to determine in which direction the reaction will proceed D How to calculate the equilibrium constantgiven the chemicalreaction and the equilibrium concentrations or pressures D How to nd the equilibrium concentrations or pressures of reactants or products given the value of the equilibrium constant and the initial concentrations D How to nd initial concentrations or pressures ofreactants or products given the value ofthe equilibrium constant and additional necessary information U Know your algebralhow to work with the quadratic formula how to solve for x and then use x to calculate equilibrium or initial concentrations know howwhen to make assumptions that will simplify these calculations and when they fail 5 rule etc D Le Chate lier39s Principle qualitatively how does a system respond to a change in conditions 0 Effect of a change in concentration 0 Effect of a change in volume partial pressure 0 Effect of a change in temperature


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