Lecturez11SHWeb

Lecturez11SHWeb - 1 Friday. Sept 30, 2011 Today’s Lecture...

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Unformatted text preview: 1 Friday. Sept 30, 2011 Today’s Lecture • Energy, Enthalpy, and Thermochemistry • 9.3 Thermodynamics of Gases • 9.4 Calorimetry Lecture 11 2 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 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 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 6...
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This note was uploaded on 12/10/2011 for the course CHEM 121 taught by Professor Leech during the Fall '11 term at Simon Fraser.

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Lecturez11SHWeb - 1 Friday. Sept 30, 2011 Today’s Lecture...

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