Question

The Nernst Equation enables the determination of cell potential under non-standard conditions. It relates the measured cell potential to the reaction quotient and allows the accurate determination of equilibrium constants: E = Eº - RT/nF ln(Q) with E = cell potential in volts [J/ coulomb] n = moles of electrons F = Faraday's constant: 96,485 [coulombs/mole] of electrons Using the free energy equation: ?G = ?Gº + RTln(Q) SHOW: ?Gº = -nFEº

          The Nernst Equation enables the determination of cell potential under non-standard conditions. It
relates the measured cell potential to the reaction quotient and allows the accurate determination
of equilibrium constants:

E = Eº - RT/nF ln(Q)

with

E = cell potential in volts [J/ coulomb]

n = moles of electrons

F = Faraday's constant: 96,485 [coulombs/mole] of electrons

Using the free energy equation:

?G = ?Gº + RTln(Q)

SHOW:

?Gº = -nFEº

The Nernst Equation enables the determination of cell potential under non-standard conditions. It
relates the measured cell potential to the reaction quotient and allows the accurate determination
of equilibrium constants:

E = Eº - RT/nF ln(Q)

with

E = cell potential in volts [J/ coulomb]

n = moles of electrons

F = Faraday's constant: 96,485 [coulombs/mole] of electrons

Using the free energy equation:

?G = ?Gº + RTln(Q)

SHOW:

?Gº = -nFEº

Added by Dwayne C.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Madhur L

04/23/2023

Step 1

First, we have the Nernst Equation: $$E = E^o - \frac{RT}{nF} \ln(Q)$$ Now, we have the free energy equation: $$\Delta G = \Delta G^o + RT \ln(Q)$$ We know that: $$\Delta G = -nFE$$ So, we can substitute this into the free energy equation: $$-nFE = \Delta Show more…

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The Nernst Equation enables the determination of cell potential under non-standard conditions. It relates the measured cell potential to the reaction quotient and allows the accurate determination of equilibrium constants: E = Eº - (RT/nF)ln(Q) with E = cell potential in volts [J/ coulomb] n = moles of electrons F = Faraday's constant: 96,485 [coulombs/mole] of electrons Using the free energy equation: ΔG = ΔGº + RTln(Q) SHOW: ΔGº = -nFEº