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Homework Statement
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.
Homework Equations
ΔG = -nFΔE
ln K = nFE/RT
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?
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