Thermodynamics (L3-1) Flashcards
Enthalpy (H) and its changes (∆H)
H = internal energy of system
∆H = H2 - H1
Negative in exothermic rxns
Positive in endothermic rxns
Entropy (S)
A quantitative measure of the disorder or randomness of a system
Rxns tend to occur spontaneously in the direction in which S increases
Change in Gibbs Free Energy (∆G)
Is the change in free energy during a rxn at any [reactants] and [products]
Predicts direction of reaction
Negative ∆G is favorable
Standard Free Energy (ΔG°)
Same as ΔG, but [Reactants] and [Products] are at 1M, at 25° C
Relationship of Keq and ΔG°
If Keq = 1, then ΔG° = 0
If Keq > 1, then ΔG° < 0
If Keq < 1, then ΔG° > 0
How does energy coupling occur?
Occurs when the energy-requiring and energy-yielding reactions share a common intermediate (ex: ATP)
T/F: Free energy is additive in coupled rxn sequences
True!
A rxn pathway may occur spontaneously (-ΔG) even if individual steps have +ΔG values
Characteristics of ATP
Is often used as the common intermediate
Has 3 phosphate bonds; 2 of which are high energy bonds
T/F: NAD+, NADP+, FAD, FMN are high energy forms
False! NADH, NADPH, FADH2 and FMNH2 are the reduced, high energy forms