1. The problem statement, all variables and given/known data Redox reaction: B-hydroxybutarate + 1/2O2 -> acetoacetate + H2O Half reaction 1: O2 + 4H+ + 4e- -> 2H2O (E = +0.816 V) Half reaction 2: acetoacetate + 2H+ + 2e- -> B-hydroxybutarate (E = -0.346 V) Using standard reduction potentials given, calculate ΔG calculate the equilibrium constant, K Conditions are the biochemist's standard state, pH 7, 298.15 K. 2. Relevant equations ΔG = -nFΔE ln K = nFE/RT 3. The attempt at a solution ΔErxn = (0.816 V) + (0.346 V) ΔErxn = 1.162 V ΔG = -nFΔE ΔG = -n(96485 C/mol)(1.162 V) n = ? (moles of electrons transferred) By writing out both half reactions, the electrons cancel out. Should there not be electrons left over on one side of the equation in order to determine the value of n?