Chem_208_Lecture_4_Color - Today: Finishing through 7.8....

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Today: Finishing through 7.8. (7.9 Optional) PS1 due tomorrow at 2:00PM; PS2 assigned online today
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State Functions (Depends only on state): Altitude (h) Position (x,y) Pot. Energy (PE) Path Dependent Function (depends upon path taken): Distance traveled (d) Another statement of the First Law of Thermodynamics: Δ U = U f –U i = q + w Internal Energy (U) Heat transferred (q) Work done (w) U is a state function; q and w are not state functions
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Bomb Calorimeter W = 0 ( Δ V = 0) Δ U = q + w = q + 0 = q v U i U f Δ U = q V q V The heat of reaction measured in a bomb calorimeter (constant V) is the change in internal energy ( Δ U)
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Coffee-Cup Calorimeter Reaction occurs under the constant pressure of the atmosphere P is constant, so if gases are formed, V will change: Δ U = q + w = q p -P Δ V U i U f Δ U= q P + w = q P -P Δ V
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For reactions in open containers, we are interested in the heat of reaction at constant pressure (q p ): q p = Δ U + P Δ V Enthalpy (H): We introduce a new state function, enthalpy (H):
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Chem_208_Lecture_4_Color - Today: Finishing through 7.8....

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