00:24 Importance of ATP
01:27 ATP hydrolysis
01:56 Assuming ΔG° = 31 kcal / mol
03:01 Relation between equilibrium constant (K) and standard Gibbs free energy (ΔG°)
08:56 Using that in vivo K = 10⁸
11:26 Role of ATP in overcoming Law of Mass Action

Calculation of the equilibrium constant K, assuming that the standard Gibbs energy ΔGº is 31 kcal / mol. Next, the (actual) standard Gibbs energy, accounting for the influence of Mg ⁺², is calculated, using the fact that the actual equilibrium constant K is 10⁸. Finally, the effect of ATP hydrolysis in transforming unfavorable (but necessary) biochemical reactions into thermodynamically favorable ones, is illustrated.

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