Chapter 23, Problem 23.13QAP

Interpretation Introduction

(a)

Interpretation:

The theoretical potential of the cell ${\text{SCE || Fe}}^{3+}(0.0150{\text{ M), Fe}}^{2+}(0.0250\text{ M)| Pt}$ should be calculated.

Concept introduction:

Nernst equation gives the cell potential under non-standard conditions.

$\text{E}={\text{E}}^0-\frac{2.303RT}{nF}\log Q$

E − cell potential

E⁰ − standard cell potential

R − universal gas constant

T − temperature in Kelvin

n − number of electrons transferred

F − Faraday constant

Q − Reaction quotient

${\text{E}}_{cell}={\text{E}}_{cathode}^0-{\text{E}}_{anode}^0$

Interpretation Introduction

(b)

Interpretation:

The theoretical potential of the cell ${\text{SCE || Zn}}^{2+}(0.00135\text{ M)| Zn}$ should be calculated.

Concept introduction:

Nernst equation gives the cell potential under non-standard conditions.

$\text{E}={\text{E}}^0-\frac{2.303RT}{nF}\log Q$

E − cell potential

E⁰ − standard cell potential

R − universal gas constant

T − temperature in Kelvin

n − number of electrons transferred

F − Faraday constant

Q − Reaction quotient

${\text{E}}_{cell}={\text{E}}_{cathode}^0-{\text{E}}_{anode}^0$

Interpretation Introduction

(c)

Interpretation:

The theoretical potential of the cell ${\text{Saturated Ag/AgCl reference || Ti}}^{3+}(0.0450{\text{ M), Ti}}^{2+}\text{(0}\text{.0250 M)| Pt}$ should be calculated.

Concept introduction:

Nernst equation gives the cell potential under non-standard conditions.

$\text{E}={\text{E}}^0-\frac{2.303RT}{nF}\log Q$

E − cell potential

E⁰ − standard cell potential

R − universal gas constant

T − temperature in Kelvin

n − number of electrons transferred

F − Faraday constant

Q − Reaction quotient

${\text{E}}_{cell}={\text{E}}_{cathode}^0-{\text{E}}_{anode}^0$

Interpretation Introduction

(d)

Interpretation:

The Theoretical potential of the cell ${\text{Saturated Ag/AgCl reference || I}}_3{}^{-}(0.00667{\text{ M), I}}^{-}\text{(0}\text{.00433 M)| Pt}$ should be calculated.

Concept introduction:

Nernst equation gives the cell potential under non-standard conditions.

$\text{E}={\text{E}}^0-\frac{2.303RT}{nF}\log Q$

E − cell potential

E⁰ − standard cell potential

R − universal gas constant

T − temperature in Kelvin

n − number of electrons transferred

F − Faraday constant

Q − Reaction quotient

${\text{E}}_{cell}={\text{E}}_{cathode}^0-{\text{E}}_{anode}^0$