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Exam 1 Study Guide - Swamy

by: Sofia Di Cugno

Exam 1 Study Guide - Swamy CHM 1046

Sofia Di Cugno
GPA 3.69
General Chemistry II
Uma Swamy

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General Chemistry II
Uma Swamy
Study Guide
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This 4 page Study Guide was uploaded by Sofia Di Cugno on Thursday January 29, 2015. The Study Guide belongs to CHM 1046 at Florida International University taught by Uma Swamy in Spring2015. Since its upload, it has received 429 views. For similar materials see General Chemistry II in Chemistry at Florida International University.


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Date Created: 01/29/15
General Chemestry ll Exam 1 Review Ch 15 amp 14 1 Characteristics of a system at equilibrium 2 Reaction Quotient Q and Equilibrium Constant K 3 KC and Kp a Differences b Converting KC to Kp c Characteristics 4 Determining direction of reaction by comparing Q and K 5 Manipulating equilibrium constants based on manipulations to chemical equations 6 ICE tables 7 When is x negligible 8 Rates of chemical reactions a Rate of a compound b Average rate of reaction 1 Characteristics of a system at equilibrium de ning equilibrium 0 Rate of forward reaction Rate of reverse reaction 0 Concentrations of products and reactants remain constant o It is a dynamic process reaction keeps going but there is no observable change 0 Can be approached from the left forward reaction or from the right reverse reaction 0 Closed system D constant temperature 2Reaction Quotient and Equilibrium Constant For reaction aA bB ltgt CC dD QZiCiCiDidAKZiCiZqiDiZq Ai iBi AiZquiZq K Q at equilibrium 3 Kp and Kc a Differences Kc is calculated using equilibrium concentrations of reactants and products and Kp is calculated using absolute pressures at equilibrium of reactants and products The expression is the same b Converting Kp to Kc An Kp KCRT Where R gas constant 00821 LatmmolK T temperature in K An moles of gaseous products moles of gaseous reactants moles of products moles of An O Kp Kc reactants moles of products gt moles of An gt O Kp gt Kc reactants moles of products lt moles of An lt O Kp lt Kc reactants c Characteristics of Kc Kc remains constant at a particular temperature 0 Different equilibrium concentrations at the same temperature have the same Kc value 0 Value of Kc indicates whether products or reactants predominate at equilibrium K gt 1 products gt reactants K lt 1 products lt reactants 4Comparing Q and K QK Products and Forward and Reaction is at reactants are at reverse reactions equilibrium equilibrium at constant rate concentrations Q gt K Products gt Reverse reaction is Reaction shifts left reactants favored to reach equilibrium Q lt K Reactants gt Forward reaction is Reaction shifts products favored right to reach equilibrium 5 Manipulating equilibrium constants based on manipulations to chemical equa ons Reverseinvert a reaction equation l tale the reciprocal of the original K 0 Multiply a reaction equation times a factor a raise original K to the power of that factor Ka Add two chemical equations together l multiply their corresponding K values to obtain new K 6ICE Tables a l lnitial Concentration given b C Change in Concentration iAx if compound is decreasing if compound is increasing A is the stoichiometry coef cient of the compound And X is an unknown factor c E Equilibrium Concentration Initial concentration i change in concentration 7 When is x negligible when solving for ICE tables Initial Concentration If the K is gt 500 l x is negligible but only when adding or subtracting lt 500 D x is NOT negligible and in order to solve for x you must use quadratic equation b i V 92 4 ac 2b 0 ax X C I X 2a 8 Rates of chemical reactions A concentration a Rate of a compound Mime Products D increase in concentration Reactants D decrease in concentration a Rate of reaction slows down as reaction goes on b Average rate of reaction depends on stoichiometric coef cient For reaction 2A 38 l C 2D 1AiAi 1AiBi1Aici1MB AVRate 2m 3m At 2m or H depends on whether compound is decreasing or increasing in concentration Factor in denominator is the stoichiometric coef cient of the corresponding compound


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