CHEM 124 course notes

CHEM 124 course notes - CHE M 124 COURSE NOTES CHAPTER SIX...

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Unformatted text preview: CHE M 124 COURSE NOTES CHAPTER SIX System = part of universe whose change e are going to observe Surroundings = everything else Internal Energy (IE) = sum of all potential and kinetic energies for all particles in system (Usually focus of E) Δ =- =- ∆E Efinal Einital Eproducts Ereactans Heat (q) = energy transferred between system & surroundings as a result of difference in temperature only. Work (w) = energy transferred when object is moved by a force Ex: mechanical, electrical, etc. = + ∆E q w = = + ∆Euniverse 0 ∆Esystem ∆Esurroundings =- ∆Esystem ∆Esurrondings Sign Convention = all relative to the system- Means lost by system Work done by + Means gain by system Work done on State Fuel = property dependent on current state of system Path Function = property that depends on how you reached the current state Calori m e try Heat Capacity = quantity of heat required to change a substances’ temperature by 1°C RELATIONSHIPS = q mc∆T = ( ) q heat J = ( ) m mass g = c specific heatJg℃ =- ∆T Tfinal Tintial If T < 0; q < 0 Δ If T > 0; q > 0 Δ Calorimery = device that measures heat released or absorbed by a physical or chemical process UNITS = Joules (J) 1 calorie = 4.184 J Calc q system = -q surroundings Heat for phase change/Reaction Enthalpy Enthalpy (H) = internal energy plus product of pressure & volume Exothermic = releases heat H < 0 Δ Endothermic = absorbs heat H > 0 Δ Special Types of Enthalpy 1) Heat of Combustion ( H Δ comb ) 2) Heat of Formation ( H Δ f ) 3) Heat of Fusion ( H Δ fus ) - melting 4) Heat of Vaporization ( H Δ vap ) – liquid to gas 5) Heat of Sublimation ( H Δ sub ) – solid to gas During phase change change in heat occurs at constant T Within phase change change in heat accompanied by change in T Calculations Heat for temperature change; no phase change/Reaction = q mc∆t Heat for phase change/Reaction; no temperature change...
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CHEM 124 course notes - CHE M 124 COURSE NOTES CHAPTER SIX...

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