Chemistry II Week 8 Notes
Chemistry II Week 8 Notes CHEM 1120
University of Memphis
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This 2 page Class Notes was uploaded by Annika Coley on Saturday April 2, 2016. The Class Notes belongs to CHEM 1120 at University of Memphis taught by Dr. Brewster in Spring 2016. Since its upload, it has received 12 views. For similar materials see GENERAL CHEMISTRY II in Chemistry at University of Memphis.
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Date Created: 04/02/16
Chemistry II Notes - Week 8 Free Energy and Thermodynamics Thermodynamics o Tells whether or not a process should occur Spontaneous Process that occurs and reduces the amount of energy in the system Irreversible Normally exothermic and releases energy Some can be endothermic High to lower potential energy Nonspontaneous Requires energy input Enthalpy o Difference between the sum of internal energy and PV o Exothermic if the product’s bonds are stronger than the reactants o Delta H is negative for exothermic o kJ/mol Etropy (S) o Increases as the number of energetically equivalent way of arranging the component increases o Potential for disorder o J/mol o Random assortment takes less energy o Favorable changes in entropy Breaking down to produce more molecules Raising the temp Dissolving nd Liquid to gas 2 law of thermodynamics o Total entropy of the universe is increasing Standard state o Pressure at 1 atm o Solution 1 M concentration o Solid/liquid is at 1 atm and room temperature Absolute entropy of a perfect crystal is 0 J/mol K o Can’t have a negative entropy o Evertything has some entropy Larger molar mass or more molecules has a larger entropy because more ways for the electrons to arrange themselves Entropy increases must come from heat released by the system – must be exothermic Endothermic processes decrease the entropy For a high original temperature, a small change in heat will not affect the entropy very much
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