- Free Energy: portion of systems energy that can perform work when temperature and pressure are uniform throughout (not heat)
- Formula ΔG= ΔH-TΔH
- ΔG= Free energy change
- ΔH = Enthalpy, change in total energy/heat content
- ΔS = Entropy, what’s lost as heat
- Spontaneous processes occur without energy input, – ΔG (quickly or slowly)
- Increases entropy, decrease H, and releases energy for work
- Nonspontaneous: requires energy, decreases entropy, + ΔG
- monomer to polymer
Free Energy, Stability, and Equilibrium
- ΔG(result energy) = G (final) – G (initial) ← net energy
- –ΔG = system loses free energy and becomes more stable
- More energy/more unstable → lower ΔG/more stable/less work capacity
EQUILIBRIUM
Equilibrium is a state of maximum stability (low energy); forward and reverse actions occur at the same rate so there is no net change→ no net production of reactants or products
- A process is spontaneous and can perform work only if it is moving towards equilibrium
- System at equilibrium = lowest ΔG
- Ex: Chemical reactions where neither reactant or product are used
- A cell at metabolic equilibrium is dead cuz systems can do no work
- So cells constantly have materials in/out which stops from reaching equilibrium
- cellular respiration: the product does not accumulate, instead becomes the reactant in next step
- Reaction at equilibrium will stay that way even if the enzyme is added!
- So cells constantly have materials in/out which stops from reaching equilibrium