MCB Lecture 1

Question	Answer
What is the relationship between ΔG, ΔH, and ΔS?	Image: Capture (binary/octet-stream)
Gibbs Free Energy?	The energy of the reaction available to do work.
Gibbs Free Energy Plot	Image: Capture1 (binary/octet-stream)
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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