For a certain cell, E^∘=1.20 V. Calculate ΔG^∘ if n is (a) 1 (b) 2 (c) 3 Comment on the effect

step 1 To solve for Delta G standard from E -cell standard, we simply use this little equation. So delt

For a certain cell, E^∘=1.20 V. Calculate ΔG^∘ if n is (a)...

For a certain cell, $E^{\circ}=1.20 \mathrm{~V}$. Calculate $\Delta G^{\circ}$ if $n$ is
(a) 1
(b) 2
(c) 3
Comment on the effect that the number of electrons exchanged has on the spontaneity of a reaction.

Key Concepts

Gibbs Free Energy (?G°)

Gibbs free energy is a thermodynamic quantity that indicates whether a reaction can occur spontaneously under standard conditions. A negative ?G° means the reaction is spontaneous, whereas a positive ?G° implies that it is non-spontaneous under the given conditions. This concept is crucial for understanding the driving force behind chemical reactions.

Standard Cell Potential (E°)

The standard cell potential, E°, measures the voltage difference between two half-cells in an electrochemical cell operating under standard conditions. It represents the inherent ability of the cell to drive an electric current and, when positive, suggests that the overall electrochemical reaction can proceed spontaneously.

Faraday’s Constant (F)

Faraday's constant is the amount of electric charge per mole of electrons, approximately 96485 coulombs per mole. It serves as the bridge between chemical change (moles of electrons) and electrical work (voltage and charge), and is essential when relating the standard cell potential to the Gibbs free energy change.

Electron Transfer Stoichiometry (n)

The number of electrons transferred in an electrochemical reaction directly impacts the magnitude of the Gibbs free energy change. Since ?G° is calculated using the formula ?G° = -nFE°, increasing the number of electrons (n) results in a proportionally larger (more negative) ?G° for a constant cell potential, thereby enhancing the reaction’s drive towards spontaneity.

Please give Ace some feedback