01:119:115 Lecture Notes - Lecture 6: Exergonic Reaction, Endergonic Reaction, Exergonic Process

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Enthalpy (h): total bond e in a system = total potenial e, free e (g): e available to work (assuming constant t and p) Enthalpy = free e + (temperature x entropy) G, h kj/mole kj = kilojoule, unit of e. You break bonds, so h is negaive fewer bonds, less e stored. G = -50 (5k -5kj/k) = -25 kj: exergonic reacions. Potenial e in reactants > potenial e in products. This is a loss of free e can use to do work. Potenial e in reactants < potenial e in products. This is a gain of free e work has done. Sunlight: source of e for biological systems. How do cells get e: coupled reacions, atp. An endergonic reacion (requires e) w/ an exergonic reacion to provide the e. Primary energy molecule of the cell: atp structure, hydrolysis, atp hydrolysis drives endergonic reacion. Exergonic reacions are spontaneous, but not instantaneous oten too slow for cells.

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