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Module 10 Set 4

Exergonic reactions Have –△G
Exergonic reactions Energy is released
Endergonic reactions Have +△G
Endergonic reactions Products have more energy than reactants
Endergonic reactions Reactions can only occur with an input of energy
Reversible reactions Have free energy difference NEAR ZERO
Reversible reactions Reaction is at equilibrium
Reaction at equilibrium when Rate of forward reaction = rate of reverse reaction
Equilibrium constant (Keq) Expresses equilibrium concentrations of products and reactants to one another
Standard reduction potential (Eo) Equilibrium constant for oxidation–reduction reaction
Standard reduction potential (Eo) Measure tendency of reducing agent to lose electrons
More negative Eo Better electron donor
More positive Eo Better electron acceptor
The greater the difference between the E0 of the donor and the E0 of the acceptor the more negative the ΔGo´
many metabolic processes involve oxidation-reduction reactions (electron transfers)
electron carriers are often used to transfer electrons from an electron donor to an electron acceptor
redox reactions: transfer of electrons from a donor to an acceptor
reducing agent or reductant electron donor
oxidizing agent or oxidant electron acceptor
redox reactions can result in energy release, which can be conserved and used to form ATP
Created by: Whereis_raye