# 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 = 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 quotient

### Principles of Instrumental Analysis

7th Edition
Douglas A. Skoog + 2 others
Publisher: Cengage Learning
ISBN: 9781305577213

### Principles of Instrumental Analysis

7th Edition
Douglas A. Skoog + 2 others
Publisher: Cengage Learning
ISBN: 9781305577213

#### Solutions

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.   E=E0−2.303RTnFlogQE − cell potentialE0 − standard cell potentialR − universal gas constantT − temperature in Kelvinn − number of electrons transferred F − Faraday constantQ − reaction quotient

(b)

Interpretation Introduction

### Interpretation:The electrode potentials of the IO3- (0.154 M), I2 (2 × 10-4 M), H+(2.75 × 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.   E=E0−2.303RTnFlogQE − cell potentialE0 − standard cell potentialR − universal gas constantT − temperature in Kelvinn − number of electrons transferred F − Faraday constantQ − reaction quotient

(c)

Interpretation Introduction

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