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Chem 1332 Test 1 Ch10-11 Equations and Facts Sheet

by: Tyler

Chem 1332 Test 1 Ch10-11 Equations and Facts Sheet CHEM 1332

Marketplace > University of Houston > CHEM 1332 > Chem 1332 Test 1 Ch10 11 Equations and Facts Sheet

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Hand typed from an image of equations sheet into pdf format for ease of studying.
Fundamentals of Chemistry 2
Simon Bott
Test Prep (MCAT, SAT...)
Chem 1332, test, Study Guide, cheat sheet, equations
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This 2 page Test Prep (MCAT, SAT...) was uploaded by Tyler on Monday February 22, 2016. The Test Prep (MCAT, SAT...) belongs to CHEM 1332 at University of Houston taught by Simon Bott in Spring2015. Since its upload, it has received 201 views.

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Date Created: 02/22/16
Test 1 Chapters 10-11 Equations and Facts Sheet Monday, February 22, 2016 4:04 AM Chapter 10 C= solubility (M) Henry's Law k= Henry's constant ( ) P=Pressureof dissolved gas (atm) Raoult's Law P=Pressure X=MoleFraction of solvent Multiple Liquids Boiling-Point Elevation T = temperature Freezing Point Depression m= molalityof solute ( OsmoticPressure M = molarity R - ideal gas constant T = temperature(K) Chapter 11 For reaction Differential form [A] is concetrationof A in Integrated form Arrhenius Equation K = rate constant A = frequency factor Log form = Activation energy (J) "subtracted form" R = universal gas constant ( T= temperature(K) General facts: Like dissolveslike ΔH is generally small if solution forms (whether +/-) ΔH is generally Large and Positiveif solution does not form ΔH is generally Large and Positiveif solution does not form Kinda like dissolves kinda like LDF slightly miscible in DD DD slightly miscible in HB HB slightly miscible in Ionic Temperaturedependences : T increases -> solubility of gas in water decreases -> solubility of solids in water increases (generally) Henry's Law -> you must be given Henry's Constant Solutions with nonvolatilesolute has a lower vapor pressure than pure solvent(Raoult's Law) Solutes with solute-solventattraction violates Raoult's law (deviation, Raoult's law no longer accurate) Van't Hoff factor, I, is the number of ions per formulate unit of solute. Knowing colligative properties is key Molecularity = number of species that must collide to produce the reaction indicated by the step Rate law is always determined first. A mechanism can never be proved absolutely Mechanism must agree with experimentallydetermined rate law Sum of elementarysteps must be the overall balanced equation Activation energy = 'threshold energy' transition state Catalyst speeds up reaction without being consumed (does not show up in actual balanced equation) Catalyst appears in the first elementarystep and is canceled out somewherealong the way Catalyst LOWERS activation energy of a reaction and increases effectivecollison rate by providing a different pathway for the reaction ( lower-energy pathway) Intermediatescannot be expressed in your final rate law (generally) Intermediatescan be rewritten (substituted) with their reactants in previous "fast" elementarysteps.


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