Chapter 22, Problem 22.2QAP

(a)

Interpretation Introduction

Interpretation:

The electrode potentials of the HCl (1.53 M) | H₂ (0.929 atm), Pt half-cell should be determined.

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

(b)

Interpretation Introduction

Interpretation:

The electrode potentials of the IO₃- (0.154 M), I₂ (2 $\times$ 10-4 M), H⁺(2.75 $\times$ 10-3 M) | H₂ (0.929 atm), Pt half-cell should be determined.

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

(c)

Interpretation Introduction

Interpretation:

The electrode potentials of the Ag₂CrO₄ (sat’d), CrO₄²- (0.0625 M) | Ag half-cell should be determined.

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