Lecture13 - Notes Midterm Mon. Oct 6. 1 Wed. Oct. 1, 2003...

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1 Notes • Midterm Mon. Oct 6.
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2 Wed. Oct. 1, 2003 Today’s Lecture Energy, Enthalpy, and Thermochemistry • 9.4 Calorimetry • 9.5 Hess’ Law • 9.6 Enthalpies of Formation • 9.7/8 Sources of Energy (Omit)
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3 • Calorimetry: – is the science of measuring heat • based on observations of temperature changes when a body absorbs or discharges energy as heat – Calorimeter: • device used to determine the heat associated with chemical reactions – Heat capacity of a substance: • represents the amount of energy necessary to increase the temperature by 1 o C (1 K) e temperatur in increase absorbed heat Capacity Heat =
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4 – since heat capacity is related to the amount of a substance: oo JJ specifi c hea t capacit y or g C gK = o mola r hea t capacit y or mo l C mo lK =
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5 – Two types of calorimeters: constant-pressure: – measures changes in enthalpy, D H = q P (heats of reaction) – for solution reactions, D V = 0 : » q p = D H = D E – reaction involves gases at constant pressure: » q p = D H „ D E w = -P D V 0 D E =q p + w = D H + w Fig. 9.7
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This note was uploaded on 01/16/2010 for the course CHEM CHEM 121 taught by Professor Peggy during the Spring '09 term at Simon Fraser.

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Lecture13 - Notes Midterm Mon. Oct 6. 1 Wed. Oct. 1, 2003...

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