Question | Answer |
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 |