Glycolysis and Gibbs Free Energy
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Glycolysis and Gibbs Free Energy
I'm taking LS 7A right now, and a couple weeks ago in class we mentioned that even though some steps of glycolysis were technically nonspontaneous under standard conditions, in cellular conditions, they become spontaneous. Why does this occur?
Re: Glycolysis and Gibbs Free Energy
Delta G and standard delta G are two different things. Standard delta G is under certain conditions (1 bar, 298K, 1 mole of gas, 1M solute). However, changing temperature and the concentrations of the products and reactants can influence the real delta G of a reaction. Glycolysis occurs at a certain temperature or concentration that could delta G positive or negative depending on the conditions the cell is in.
delta G = standard delta G + RT ln Q
delta G = standard delta G + RT ln Q
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Re: Glycolysis and Gibbs Free Energy
Conditions like concentrations of reactants and products can affect delta G at nonstandard conditions and make the reaction spontaneous - this is likely what happens. This relates to the equation ΔG = ΔG° + RT ln Q. Another way a non-spontaneous reaction could be made spontaneous is by coupling the non-spontaneous reaction with a spontaneous one.
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