If the equilibrium constant for the dissociation of lactic acid is 1.38 × 10^-⁴, what is the $\Delta$G°' for this reaction? A) 16.3kJ/mol B) -16.3 kJ/mol C) 16.96 kJ/mol D) -16.96 kJ/mol E) 27.5 kJ/mol

Question

Quizplus · Accepted Answer

The standard Gibbs free energy change (ΔG°') can be calculated using the equation ΔG°' = -RTlnK. Substituting the given equilibrium constant (K = 1.38 × 10^-4) and using R = 8.314 J/mol·K and T = 298 K, we find ΔG°' ≈ 16.3 kJ/mol.

If the Equilibrium Constant for the Dissociation of Lactic Acid Δ\DeltaΔ

If the Equilibrium Constant for the Dissociation of Lactic Acid $\Delta$