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Chem 113 2nd week

by: Caroline Hurlbut

Chem 113 2nd week Chem 113

Caroline Hurlbut
GPA 3.7

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About this Document

These notes cover mainly entropy: trends, calculations, Gibbs free energy, exo/endothermic reactions, and spontaneity.
General Chemistry II
Ingrid Marie Laughman
Class Notes
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This 1 page Class Notes was uploaded by Caroline Hurlbut on Friday January 29, 2016. The Class Notes belongs to Chem 113 at Colorado State University taught by Ingrid Marie Laughman in Spring 2016. Since its upload, it has received 19 views. For similar materials see General Chemistry II in Chemistry at Colorado State University.


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Date Created: 01/29/16
Entropy Changes & Spontaneity methane from gas leak in LA reacts with O2 in atmosphere and combusts to form • water and CO2 —CH4(g) + 2O2(g)—>CO2(g) + 2H2O(l) —3 gas molecules—> 1 gas molecule + 2 liquid molecules results in decrease in entropy • ∆Ssys=∆Hsys/T • ∆Ssurr=∆Hsurr/T • ∆Suniv=∆Ssys + ∆Ssurr = ∆Ssys - (∆Hsys/T) • ex. Calculate ∆Ssys, ∆Ssurr, and ∆Suniv when 1 mole of water in ice at 0˚C melts to 22˚C. ∆H=6.01 kJ —∆Ssys=6010 J/273 K=22.0 J/K —∆Ssurr=-6010 J/295 K=-20.4 J/K —∆Suniv=22.0 J/K - 20.4 J/K=1.6 J/K • if ∆Suniv>0, the reaction is spontaneous —only ∆Suniv can determine spontaneity, not ∆Ssys (determines # microstates) • ∆Srxn=(#moles x ∆S) products - (#moles x ∆S) reactants • Gibbs free energy formula —∆Gsys=∆Hsys - T∆Ssys • spontaneity of a reaction —if ∆Gsys<0, then ∆Suniv>0 and the reaction is spontaneous —if ∆Gsys>0, then ∆Suniv<0 and the reaction is non spontaneous (no reaction) —if ∆Gsys=0, then ∆Suniv=0 and the reaction has reached chemical equilibrium (forward and reverse reactions occur at the same rate) • spontaneous reactions are not always exothermic • type of thermic reaction determined by enthalpy —if ∆Hsys>0, the reaction is endothermic —if ∆Hsys<0, the reaction is exothermic T∆S Energy Right side ∆G<0—>spontaneous ∆H Temp


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