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ChemistryPrinciples of Instrumental AnalysisThe electrode potentials of the HCl (1.53 M) | H 2 (0.929 atm), Pt half-cell should be determined. Concept Introduction : Nernst equation gives the cell potential under non-standard conditions. E = E 0 − 2.303 R T n F log Q E − cell potential E 0 − standard cell potential R − universal gas constant T − temperature in Kelvin n − number of electrons transferred F − Faraday constant Q − reaction quotientStart your trial now! First week only $4.99!*arrow_forward*

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7th Edition

Douglas A. Skoog + 2 others

Publisher: Cengage Learning

ISBN: 9781305577213

Chapter 22, Problem 22.2QAP

**(a)**

Interpretation Introduction

**Interpretation:**

The electrode potentials of the HCl (1.53 M) | H_{2} (0.929 atm), Pt half-cell should be determined.

**Concept Introduction** **:**

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

E − cell potential

E^{0} − 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 IO_{3}- (0.154 M), I_{2} (2 ^{+}(2.75 _{2} (0.929 atm), Pt half-cell should be determined.

**Concept Introduction** **:**

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

E − cell potential

E^{0} − 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 Ag_{2}CrO_{4} (sat’d), CrO_{4}^{2}- (0.0625 M) | Ag half-cell should be determined.

**Concept Introduction** **:**

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

E − cell potential

E^{0} − standard cell potential

R − universal gas constant

T − temperature in Kelvin

n − number of electrons transferred

F − Faraday constant

Q − reaction quotient