Chapter%202_4%20summary

# Chapter%202_4%20summary - Review of Thermodynamics Pure...

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1 Closed system Pure materials Mixture M j j j B n B 1 * M j j j B n B 1 Review of Thermodynamics State 1 State 2 1 st and 2 nd Law govern changes in state variables Processes: - volume expansion - pressurization - heating - phase transition wq State variables: P, T, V, E, H, S, G, C p , C V

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2 Standard State P 0 = 1 atm and T 0 = 25 o C - What are H 0 , S 0 , G 0 as well as f H 0 , f S 0 , f G 0 of pure elements and compounds? - What are H 0 , S 0 , G 0 as well as f H 0 , f S 0 , f G 0 of ions in aqueous solution? - What are r H 0 , r S 0 , r G 0 of reactions? P = P ex = constant T = T ex = constant dS = q rev /T (dG) P,T =dw add,rev In Reversible Process (= Equilibrium Process), Useful work in biological system Molar properties: B m = B/n w= -P ex dV H E + pV G H - TS E = w + q 1 st Law T δ q dS (dG) P,T  w add 2 nd Law ( H) P = q p + w add • Reversible vs irreversible processes in terms of S or G Not considered Not considered q=dE- w (dH) P = C P dT; q P = C P dT only if w = -PdV and P = constant (dE) V = C V dT q V = C V dT only if ex dV and dV = 0
3 1. Derivation of w, q, E, H, S, G for ideal gas 2. For liquid and solid, the volume change is negligible. Thus, - V 0 - E  H -C P = C V - a = 1 (in pure system) In Pure System 3. Phase transition:

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## This note was uploaded on 01/17/2010 for the course BME 100 taught by Professor Yuan during the Fall '07 term at Duke.

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Chapter%202_4%20summary - Review of Thermodynamics Pure...

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