Flashcards
MCB Lecture 1
Cards in this deck (12)
- 1What is the relationship between ΔG, ΔH, and ΔS?
- 2Gibbs Free Energy?The energy of the reaction available to do work.
- 3Gibbs Free Energy Plot
- 4ExergonicΔG is negative. Free energy released. Favourable, spontaneous.
- 5EndergonicΔG is positive. Free energy absorbed. Unfavourable, nonspontaneous.
- 6ExothermicΔH is negative: Heat released.
- 7EndothermicΔH is positive: Heat absorbed.
- 8ΔS is negativeLess disorder.
- 9ΔS is positiveMore disorder.
- 10Explain 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). - 11What 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. - 12What 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.