BIOL 111 Lecture Notes - Lecture 13: Methanol, Phosphorylation, Adenosine Triphosphate
Document Summary
Metabolism: all chemical reactions through cells that support functioning. Glycogen to glucose, glucose to co2 and h2o: energy can be transferred or transformed but not created or destroyed, every energy transfer/ change, results in the universe becoming more random (entrophy) Systems tend to spontaneously lose free energy, becoming more stable. Gibbs free energy (g): amount of total energy available to do work. Delta g is the change in the total amount of energy available to do work. A ball on the top of a hill, has more energy than a ball that just rolled down one. Delta g is negative down hill, energy releasing; spontaneous (energetically favorable) Delta g is positive up hill, energy absorbing ( non-spontaneous) non natural. Exergonic reactions: energy released (delta g is negative: glucose and oxygen to carbon dioxide and water (cellular respiration, polypeptides to amino acids. Reactants have more energy than products (releasing energy) Endergonic reaction: energy absorbed (delta g is positive)
