Use tabulated electrode potentials to calculate ΔGrxn^∘ for each reaction at 25^∘ C. a. 2 Fe^3+(

step 1 Here we need two equations that relate to our redox reactions. So we need delta G0, 0, reaction

Use tabulated electrode potentials to calculate ΔGrxn^∘ for...

Use tabulated electrode potentials to calculate $\Delta G_{\mathrm{rxn}}^{\circ}$ for each reaction at $25^{\circ} \mathrm{C}$. a. $2 \mathrm{Fe}^{3+}(a q)+3 \mathrm{Sn}(s) \longrightarrow 2 \mathrm{Fe}(s)+3 \mathrm{Sn}^{2+}(a q)$ b. $\mathrm{O}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(l)+2 \mathrm{Cu}(s) \longrightarrow$ $4 \mathrm{OH}^{-}(a q)+2 \mathrm{Cu}^{2+}(a q)$ c. $\mathrm{Br}_{2}(l)+2 \mathrm{I}^{-}(a q) \longrightarrow 2 \mathrm{Br}^{-}(a q)+\mathrm{I}_{2}(s)$

Use tabulated electrode potentials to calculate $\Delta G_{\mathrm{rxn}}^{\circ}$ for each reaction at $25^{\circ} \mathrm{C}$.
a. $2 \mathrm{Fe}^{3+}(a q)+3 \mathrm{Sn}(s) \longrightarrow 2 \mathrm{Fe}(s)+3 \mathrm{Sn}^{2+}(a q)$
b. $\mathrm{O}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(l)+2 \mathrm{Cu}(s) \longrightarrow$
$4 \mathrm{OH}^{-}(a q)+2 \mathrm{Cu}^{2+}(a q)$
c. $\mathrm{Br}_{2}(l)+2 \mathrm{I}^{-}(a q) \longrightarrow 2 \mathrm{Br}^{-}(a q)+\mathrm{I}_{2}(s)$

Key Concepts

Faraday Constant

Faraday's constant is a fundamental physical constant that represents the total electric charge carried by one mole of electrons, approximately 96485 coulombs per mole. It serves as a conversion factor in the equation ?G° = –nFE°, linking the number of electrons to the energy change in an electrochemical reaction.

Electron Stoichiometry

Electron stoichiometry is crucial in redox reactions as it involves determining the total number of electrons transferred during the reaction. This count is necessary when applying the ?G° = –nFE° formula, ensuring that the energy calculation correctly corresponds to the actual electron flow in the overall reaction.

Standard Electrode Potentials

Standard electrode potentials are measured for half-reactions under standard conditions and indicate the intrinsic tendency of a species to be reduced. They are tabulated values used as a reference to predict the direction and feasibility of redox reactions by comparing the relative strengths of oxidizing and reducing agents.

Gibbs Free Energy and Cell Potential Relationship

The relationship between the standard Gibbs free energy change (?G°) and the standard cell potential (E°) is given by the equation ?G° = –nFE°. This equation links the electrical work obtainable from a redox reaction with its thermodynamic spontaneity, where 'n' is the number of electrons transferred and 'F' is the Faraday constant.

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