Ch_5_Introduction_Thermchemistry - INTRODUCTION TO...

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INTRODUCTION TO THERMOCHEMISTRY Energy? The capacity to do work or to transfer heat. Kinds of energy? Kinetic energy Change in gravitational potential energy mg Δ h Change in chemical potential energy Change in internal energy Radiant energy Change in nuclear energy E photon = hf Δ E = Δ mc 2 Δ E = C V Δ T ½mv 2 Δ H rxn The change in x = Δ x = x f - x i (at constant pressure) (always true) Δ E rxn (at constant volume)
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Examples: KE and P.E; Heat; Reaction—Exothermic, Endothermic Energy transferred to a system heat q work w Change in Internal Energy = E f - E i = Δ E = q + w Sign convention: q is positive if heat is added to the system and negative if the system loses heat. w is positive if work is done on the system and negative if the system does work on the surroundings. EXAMPLE 1: 6000 J of heat are added to a system. It does 5000 J of work on the surroundings. What is Δ E ? Δ
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This note was uploaded on 11/23/2010 for the course CHEM CHEM125 taught by Professor Ellis during the Fall '10 term at NJIT.

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Ch_5_Introduction_Thermchemistry - INTRODUCTION TO...

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