Estimate ℰ^∘ for the half-reaction 2 H2 O+2 e^- ⟶H2+2 OH^- given the following values of ΔGi^∘

step 1 So here we can see the reaction of interest on the screen. And so what we need to do is to calcu

Estimate ℰ^∘ for the half-reaction 2 H2 O+2 e^- ⟶H2+2 OH^-...

Estimate $\mathscr{E}^{\circ}$ for the half-reaction $$ 2 \mathrm{H}_{2} \mathrm{O}+2 \mathrm{e}^{-} \longrightarrow \mathrm{H}_{2}+2 \mathrm{OH}^{-} $$ given the following values of $\Delta G_{i}^{\circ}$ $$ \begin{aligned} \mathrm{H}_{2} \mathrm{O}(l) &=-237 \mathrm{~kJ} / \mathrm{mol} \\ \mathrm{H}_{2}(g) &=0.0 \\ \mathrm{OH}^{-}(a q) &=-157 \mathrm{~kJ} / \mathrm{mol} \\ \mathrm{e}^{-} &=0.0 \end{aligned} $$ Compare this value of $\mathscr{E}^{\circ}$ with the value of $\mathscr{E}^{\circ}$ given in Table $18.1 .$

Estimate $\mathscr{E}^{\circ}$ for the half-reaction
$$
2 \mathrm{H}_{2} \mathrm{O}+2 \mathrm{e}^{-} \longrightarrow \mathrm{H}_{2}+2 \mathrm{OH}^{-}
$$
given the following values of $\Delta G_{i}^{\circ}$
$$
\begin{aligned}
\mathrm{H}_{2} \mathrm{O}(l) &=-237 \mathrm{~kJ} / \mathrm{mol} \\
\mathrm{H}_{2}(g) &=0.0 \\
\mathrm{OH}^{-}(a q) &=-157 \mathrm{~kJ} / \mathrm{mol} \\
\mathrm{e}^{-} &=0.0
\end{aligned}
$$
Compare this value of $\mathscr{E}^{\circ}$ with the value of $\mathscr{E}^{\circ}$ given in Table $18.1 .$

Key Concepts

Standard_Gibbs_Free_Energy_of_Formation

This is a thermodynamic quantity that represents the energy change when one mole of a compound is formed from its elements in their standard states. It is used as a reference to calculate the overall energy change in reactions, including redox processes, by summing the Gibbs energies of reactants and products.

Half-Reaction_Free_Energy_Calculation

In a half-reaction, the total free energy change is determined by summing the standard free energies of formation of the products and subtracting the sum of those for the reactants. This approach allows us to evaluate the spontaneity of the redox process under standard conditions.

Relation_Between_Gibbs_Free_Energy_and_Electrode_Potential

The relationship between the standard Gibbs free energy change (?G°) and the standard electrode potential (E°) is given by the equation ?G° = -nFE°, where n is the number of electrons transferred and F is the Faraday constant. This equation is fundamental in converting thermodynamic data into electrochemical potentials.

Standard_Electrode_Potential

The standard electrode potential reflects the tendency of a chemical species to be reduced or oxidized under standard conditions. It is computed using thermodynamic data and is essential for predicting the direction of electron flow in electrochemical cells and for comparing different redox couples.

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