What are the values of Δr G^∘ and K for the following reactions at 298 K from Table C .2 ? (a)

Name: Problem 15, Chapter 7: Physical Chemistry
Uploaded: 2020-06-17T12:24:41-08:00
Duration: 3 min 8 s
Channel: Ahmed Ali
Description: What are the values of Δr G^∘ and K for the following reactions at 298 K from Table C .2 ? (a) Cu(s)+Zn^2+(ao)=Cu^2+(ao)+Zn(s) (b) H2(g)+Cl2(g)=2 HCl(ai) (c) Ca^2+(ao)+CO3^2-(ao)=CaCO3(s, calcite ) (d) (1)/(2) Cl2(g)+Br^-(ao)=(1)/(2) Br2(g)+Cl^-(ao) (e) Ag^+(ao)+Fe^2+(ao)=Fe^3+(ao)+Ag(s)

step 1 my name is Ahmed Ali. In this question, first of all, in the first part, we must write the anode

What are the values of Δr G^∘ and K for the following...

What are the values of $\Delta_{\mathrm{r}} G^{\circ}$ and $K$ for the following reactions at $298 \mathrm{K}$ from Table $\mathrm{C} .2 ?$ $(a) \quad \mathrm{Cu}(\mathrm{s})+\mathrm{Zn}^{2+}(\mathrm{ao})=\mathrm{Cu}^{2+}(\mathrm{ao})+\mathrm{Zn}(\mathrm{s})$ $(\boldsymbol{b}) \quad \mathrm{H}_{2}(\mathrm{g})+\mathrm{Cl}_{2}(\mathrm{g})=2 \mathrm{HCl}(\mathrm{ai})$ $(c) \quad \mathrm{Ca}^{2+}(\mathrm{ao})+\mathrm{CO}_{3}^{2-}(\mathrm{ao})=\mathrm{CaCO}_{3}(\mathrm{s}, \text { calcite })$ $(\boldsymbol{d}) \quad \frac{1}{2} \mathrm{Cl}_{2}(\mathrm{g})+\mathrm{Br}^{-}(\mathrm{ao})=\frac{1}{2} \mathrm{Br}_{2}(\mathrm{g})+\mathrm{Cl}^{-}(\mathrm{ao})$ $(e) \quad \mathrm{Ag}^{+}(\mathrm{ao})+\mathrm{Fe}^{2+}(\mathrm{ao})=\mathrm{Fe}^{3+}(\mathrm{ao})+\mathrm{Ag}(\mathrm{s})$

What are the values of $\Delta_{\mathrm{r}} G^{\circ}$ and $K$ for the following reactions at $298 \mathrm{K}$ from Table $\mathrm{C} .2 ?$
$(a) \quad \mathrm{Cu}(\mathrm{s})+\mathrm{Zn}^{2+}(\mathrm{ao})=\mathrm{Cu}^{2+}(\mathrm{ao})+\mathrm{Zn}(\mathrm{s})$
$(\boldsymbol{b}) \quad \mathrm{H}_{2}(\mathrm{g})+\mathrm{Cl}_{2}(\mathrm{g})=2 \mathrm{HCl}(\mathrm{ai})$
$(c) \quad \mathrm{Ca}^{2+}(\mathrm{ao})+\mathrm{CO}_{3}^{2-}(\mathrm{ao})=\mathrm{CaCO}_{3}(\mathrm{s}, \text { calcite })$
$(\boldsymbol{d}) \quad \frac{1}{2} \mathrm{Cl}_{2}(\mathrm{g})+\mathrm{Br}^{-}(\mathrm{ao})=\frac{1}{2} \mathrm{Br}_{2}(\mathrm{g})+\mathrm{Cl}^{-}(\mathrm{ao})$
$(e) \quad \mathrm{Ag}^{+}(\mathrm{ao})+\mathrm{Fe}^{2+}(\mathrm{ao})=\mathrm{Fe}^{3+}(\mathrm{ao})+\mathrm{Ag}(\mathrm{s})$

Key Concepts

Standard Gibbs Free Energy Change

Standard Gibbs free energy change (?rG°) represents the change in free energy when a reaction occurs under standard conditions (typically 298 K, 1 bar for gases, 1 M for solutes, and pure substances for solids and liquids). It is calculated using tabulated standard free energies of formation or electrode potentials and helps determine the spontaneity of a reaction, with negative values indicating spontaneity under the given conditions.

Equilibrium Constant and Its Relation to Gibbs Free Energy

The equilibrium constant (K) of a reaction measures the ratio of product activities to reactant activities at equilibrium under standard conditions. It is directly connected to the standard Gibbs free energy change through the formula ?rG° = -RT ln K, where R is the gas constant and T is the temperature in Kelvin. This relationship provides a way to assess the position of equilibrium based on thermodynamic data.

Standard State Conditions

Standard state conditions define a common reference for all reactants and products in thermodynamic calculations, such as 298 K, 1 bar for gases, 1 M for solutions, and pure substances for solids and liquids. These conditions ensure consistency in the calculation of properties like ?rG° and equilibrium constants across different reactions.

Use of Tabulated Thermodynamic Data

Tabulated thermodynamic data, such as that provided in Table C.2, includes essential values like Gibbs free energies of formation or electrode potentials for various species. This data is crucial for calculating the ?rG° for a given reaction, which in turn is used to determine the equilibrium constant using established thermodynamic relations.

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