For the galvanic cell H2(1 bar)|HCl(ai)| Cl2(1 bar) the standard electromotive force at 29

step 1 This standard gives energy change of a reaction denoted by delta G. This is given as negative VE

For the galvanic cell H2(1 bar)|HCl(ai)| Cl2(1 bar) ...

For the galvanic cell \[ \mathrm{H}_{2}(1 \mathrm{bar})|\mathrm{HCl}(\mathrm{ai})| \mathrm{Cl}_{2}(1 \mathrm{bar}) \] the standard electromotive force at $298.15 \mathrm{K}$ is $1.3604 \mathrm{V}$, and $\left(\partial E^{\circ} / \partial T\right)_{P}=-1.247 \times 10^{-3} \mathrm{V} \mathrm{K}^{-1} .(a)$ For the cell reaction, what are the values of $\Delta_{\mathrm{r}} G^{\circ}, \Delta_{\mathrm{r}} H^{\circ},$ and $\Delta_{\mathrm{r}} S^{\circ} ?(b)$ For $\mathrm{Cl}^{-}(\mathrm{ao})$ what are the values of $\Delta_{\mathrm{f}} G^{\circ}, \Delta_{\mathrm{f}} H^{\circ},$ and $\Delta \bar{S}^{\circ} ?$

For the galvanic cell
\[
\mathrm{H}_{2}(1 \mathrm{bar})|\mathrm{HCl}(\mathrm{ai})| \mathrm{Cl}_{2}(1 \mathrm{bar})
\]
the standard electromotive force at $298.15 \mathrm{K}$ is $1.3604 \mathrm{V}$, and $\left(\partial E^{\circ} / \partial T\right)_{P}=-1.247 \times 10^{-3} \mathrm{V} \mathrm{K}^{-1} .(a)$ For the cell reaction, what are the values of $\Delta_{\mathrm{r}} G^{\circ}, \Delta_{\mathrm{r}} H^{\circ},$ and $\Delta_{\mathrm{r}} S^{\circ} ?(b)$ For $\mathrm{Cl}^{-}(\mathrm{ao})$
what are the values of $\Delta_{\mathrm{f}} G^{\circ}, \Delta_{\mathrm{f}} H^{\circ},$ and $\Delta \bar{S}^{\circ} ?$

Key Concepts

Temperature Dependence of Cell Potential

The temperature dependence of the cell potential, expressed as (?E°/?T)_P, is important in understanding how temperature variations affect the driving force of an electrochemical reaction. This derivative is directly connected to the reaction entropy through the relation ?rS° = -nF(?E°/?T)_P, linking the thermal factors to the shifting equilibrium of the redox process.

Standard Electromotive Force and Free Energy Relationship

The standard electromotive force (E°) is directly related to the Gibbs free energy change (?rG°) by the equation ?rG° = -nFE°, where n is the number of electrons transferred and F is Faraday’s constant. This relationship is crucial for determining the feasibility of an electrochemical reaction under standard conditions, with a positive cell potential corresponding to a negative change in free energy.

Standard Formation Thermodynamic Quantities

Standard formation thermodynamic quantities, such as the standard Gibbs free energy of formation (?fG°), the standard enthalpy of formation (?fH°), and the standard molar entropy (S°), are intrinsic properties of chemical species. These values serve as fundamental building blocks for constructing thermodynamic cycles and for calculating the overall energy changes in chemical reactions, thereby providing critical insights into the stability and energetics involved in compound formation.

Galvanic Cell

A galvanic cell is an electrochemical cell that converts chemical energy into electrical energy through spontaneous redox reactions. It typically consists of two half-cells connected by a conductive bridge, where oxidation occurs at the anode and reduction occurs at the cathode. The measured cell potential reflects the thermodynamic drive of the reaction occurring within the cell.

Electrochemical Thermodynamics

Electrochemical thermodynamics combines principles from thermodynamics and electrochemistry to analyze energy changes in redox reactions. Fundamental thermodynamic quantities, including the Gibbs free energy (?G), enthalpy (?H), and entropy (?S), determine the spontaneity and heat exchange of the reactions, and they are directly linked to the measurable electrical properties of the cell.

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