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

Question

In the Thermo Fisher application note about wine analysis (Lesson 3), the following chromatogram was collected of nine components of wine. If peak 3 has a retention time of 3.15 minutes and a peak width of 0.070 minutes, and peak 4 has a retention time of 3.24 minutes and a peak width of 0.075 minutes, what is the resolution factor between the two peaks? [Hint: it will help to review Lesson 2 for this question.] MAU 300 200 T 34 5 100- 1 2 CO 6 7 8 9 0 2.4 2.6 2.8 3.0 3.2 3.4 3.6 3.8 4.0 4.2 4.4 4.6 4.8 5.0 5.2 Minutes 3.22 0.62 1.04 O 1.24

Answer 1

Question

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=E0−2.303RTnFlogQ

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 × 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=E0−2.303RTnFlogQ

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.

E=E0−2.303RTnFlogQ

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

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In the Thermo Fisher application note about wine analysis (Lesson 3), the following chromatogram was collected of nine components of wine. If peak 3 has a retention time of 3.15 minutes and a peak width of 0.070 minutes, and peak 4 has a retention time of 3.24 minutes and a peak width of 0.075 minutes, what is the resolution factor between the two peaks? [Hint: it will help to review Lesson 2 for this question.] MAU 300 200 T 34 5 100- 1 2 CO 6 7 8 9 0 2.4 2.6 2.8 3.0 3.2 3.4 3.6 3.8 4.0 4.2 4.4 4.6 4.8 5.0 5.2 Minutes 3.22 0.62 1.04 O 1.24

The diagram shows two metals, A and B, which melt at 1000°C and 1400°C. State the weight percentage of the primary constituent (grains of C) that would be obtained by solidifying a 20% alloy of B. 1000°C a+L L+C 900°С 12 α a+C 45 1200 C L+y 140096 C+Y a+ß 800°C 700°C C+B 96 92 a+B 0 10 20 30 40 50 60 70 80 90 100 A % peso B B

8. Choose the compound that will produce the spectrum below and assign the signals to the corresponding protons. 2 4 3 ō (ppm) OH 4 6 6 СОН 2 1 0

Answer 2

Question

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=E0−2.303RTnFlogQ

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 × 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=E0−2.303RTnFlogQ

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.

E=E0−2.303RTnFlogQ

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

Expert Solution & Answer

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Answer 3

Question

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=E0−2.303RTnFlogQ

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 × 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=E0−2.303RTnFlogQ

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.

E=E0−2.303RTnFlogQ

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

Expert Solution & Answer

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Answer 4

Question

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=E0−2.303RTnFlogQ

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 × 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=E0−2.303RTnFlogQ

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.

E=E0−2.303RTnFlogQ

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

Expert Solution & Answer

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Answer 5

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=E0−2.303RTnFlogQ

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 × 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=E0−2.303RTnFlogQ

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.

E=E0−2.303RTnFlogQ

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

Answer 6

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=E0−2.303RTnFlogQ

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

Answer 7

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=E0−2.303RTnFlogQ

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

Answer 8

(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=E0−2.303RTnFlogQ

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

Answer 9

(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=E0−2.303RTnFlogQ

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

Answer 10

(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.

E=E0−2.303RTnFlogQ

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

Answer 11

(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.

E=E0−2.303RTnFlogQ

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

Answer 12

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Ch. 22 - Calculate the electrode potentials of the...Ch. 22 - Prob. 22.2QAP Ch. 22 - For each of the following half-cells, compare...Ch. 22 - For each of the following half-cells, compare...Ch. 22 - Prob. 22.5QAP Ch. 22 - Calculate the electrode potentials for the...Ch. 22 - Calculate the theoretical potential of each of the...Ch. 22 - Calculate the theoretical potential of each of the...Ch. 22 - Prob. 22.9QAP Ch. 22 - Prob. 22.10QAP

Chapter 22 Solutions