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| Questão | Responda |
| What is the relationship between ΔG, ΔH, and ΔS? | |
| Gibbs Free Energy? | The energy of the reaction available to do work. |
| Gibbs Free Energy Plot | |
| Exergonic | ΔG is negative. Free energy released. Favourable, spontaneous. |
| Endergonic | ΔG is positive. Free energy absorbed. Unfavourable, nonspontaneous. |
| Exothermic | ΔH is negative: Heat released. |
| Endothermic | ΔH is positive: Heat absorbed. |
| ΔS is negative | Less disorder. |
| ΔS is positive | More disorder. |
| Explain how ∆G° is different from ∆G'°. | ∆G° is the Standard Gibbs Free Energy change of a reaction (under standard conditions). ∆G'° is the Standard Gibbs Free Energy change (under Biochemistry standard conditions). |
| What are ∆G'° conditions? | - 298 K (25 degrees Celcius) - Gases at partial pressure 101.3 kPa (1 atm) - Well-buffered solution at pH 7, [H+] = 10^-7, Mg^2+ = 1 mM. |
| What are ∆G° conditions? | - 298 K (25 degrees Celcius) - Gases at partial pressure 101.3 kPa (1 atm) - Reactants and Products at 1 M, [H+] = 1 M --> pH 0. |
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