Biology 1002B Lecture Notes - Lecture 4: Exergonic Reaction, Exothermic Process, Exergonic Process
9 Apr 2016
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2nd law of thermodynamics disorder of system + surroundings increases. Does life go against this law: nope, life is an open system. We bring in energy, and expel disorder (heat, gases etc. More random (entropy) s < aq < l < g. G = h - t s: = the change in; the difference, g = gibbs; free energy. Exergonic unstable: h = enthalpy (think: overall potential energy) + endothermic (takes in heat, product w/ more pe) Exothermic (gives off heat, reactant w/ more pe: t = temperature, s = entropy (randomness) Reactions tend to be spontaneous (- g) when : exergonic reactions, exothermic; products have more pe than reactants, more disorder in the products than in the reactants. Why does life need enzymes: rather than turning up the temperature, b/c biological molecules can"t handle high temps, so evolution produced enzymes so reactions would occur quicker.
