Lecturez11SHWeb - Friday Todays Lecture Energy Enthalpy and...

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1 Friday. Sept 30, 2011 Today’s Lecture Energy, Enthalpy, and Thermochemistry 9.3 Thermodynamics of Gases 9.4 Calorimetry Lecture 11
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3 Enthalpy and calorimetry: – Enthalpy (H): H = E + PV for a process at constant P: Δ E = q p + w = q p - P Δ V – where q p is the heat at constant P q p = Δ E + P Δ V Δ H = Δ E + P Δ V ∴Δ H = q p internal energy of the system Pressure exerted on system by surroundings volume of system Δ H = q p
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4 – Enthalpy is a measure of heat a change in enthalpy ( Δ H ) is equal to the amount of heat ( q P ) given off or absorbed at a constant pressure: Δ H = Δ E + P Δ V =q P Δ H is called heat of reaction for a chemical reaction: Δ H = H products - H reactants Δ H < 0 exothermic : heat is given off Δ H > 0 endothermic : heat is absorbed Important because many reaction carried out in open flasks
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5 9.3 Thermodynamics of ideal gases: recall (Chap 5): KE avg = _______ energy required to change energy of 1 mole of an ideal gas by Δ T : Energy (heat) required = ______ molar heat capacity: is the energy required to raise the temperature of 1 mole of that substance by 1 K molar heat capacity = _______ valid for a monoatomic gas at constant volume
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