Chapter 6, Problem 6D.3P

(a)

Interpretation Introduction

Interpretation:

The standard cell potential of the ${\text{HCO}}_3^{-}/{\text{CO}}_3^{2-},{\text{H}}_{\text{2}}$ couple has to be predicted.

Concept introduction:

The change in Gibbs free energy for a reaction when reactants and products are present in their standard states of pressure, forms and concentration is represented by ${\Delta }_{\text{r}}G°$ whereas ${\Delta }_{\text{r}}G$ depends on the reaction condition and extent of reaction.

(b)

Interpretation Introduction

Interpretation:

The standard potential for the cell reaction ${\text{Na}}_2{\text{CO}}_3\left(\text{aq}\right)+{\text{H}}_2\text{O}\left(\text{l}\right)\to {\text{NaHCO}}_3\left(\text{aq}\right)+\text{NaOH}\left(\text{aq}\right)$ has to be predicted.

Concept introduction:

Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations. Standard electrode potential is the electrode potential at standard temperature, pressure and concentration.

(c)

Interpretation Introduction

Interpretation:

The Nernst equation for the cell has to be stated.

Concept introduction:

Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations.  The expression for Nernst equation is,

    $E_{\text{cell}}=E_{\text{cell}}^{\text{ο}}-\frac{RT}{vF}\ln Q$

Where,

• $E_{\text{cell}}$ is the electrode potential of the cell.
• $E_{\text{cell}}^{\text{ο}}$ is the standard electrode potential of the cell.
• $R$ is the gas constant.
• $T$ is the temperature.
• $v$ is the number of electrons.
• $F$ is the Faraday’s constant.
• $Q$ is the reaction quotient.

(d)

Interpretation Introduction

Interpretation:

The change in cell potential when the $\text{pH}$ is changed to $7.0$ at $298\text{K}$ has to be stated.

Concept introduction:

Nernst equation is the relation between standard electrode potential and the electrode potential at given conditions of pressures, temperatures and concentrations.  The expression for Nernst equation is,

    $E_{\text{cell}}=E_{\text{cell}}^{\text{ο}}-\frac{RT}{vF}\ln Q$

Where,

• $E_{\text{cell}}$ is the electrode potential of the cell.
• $E_{\text{cell}}^{\text{ο}}$ is the standard electrode potential of the cell.
• $R$ is the gas constant.
• $T$ is the temperature.
• $v$ is the number of electrons.
• $F$ is the Faraday’s constant.
• $Q$ is the reaction quotient.