It has to be explained the reason for if the paint is placed between the copper and the zinc, the zinc will still corrode in seawater, but it will not protect the copper from corrosion. Concept introduction: Corrosion is a natural process. The destruction of metals by electrochemical reaction with water and oxygen in the air. Sacrificial anodes are highly active metals that are used to prevent a less active metal surface from corrosion. The loss of electrons is called oxidation whereas the gain of electrons is called reduction. In an electrochemical cell, at anode oxidation takes place and at cathode reduction takes place. The copper is oxidized by air in seawater. The chemical reaction is written as, Cu ( s ) + H 2 O ( l ) + 1 2 O 2 ( g ) → Cu ( OH ) 2 ( s )

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Answer 1

Question

Chapter 19.8, Problem 1Q

Interpretation Introduction

Interpretation: It has to be explained the reason for if the paint is placed between the copper and the zinc, the zinc will still corrode in seawater, but it will not protect the copper from corrosion.

Concept introduction: Corrosion is a natural process. The destruction of metals by electrochemical reaction with water and oxygen in the air.

Sacrificial anodes are highly active metals that are used to prevent a less active metal surface from corrosion.

The loss of electrons is called oxidation whereas the gain of electrons is called reduction.

In an electrochemical cell, at anode oxidation takes place and at cathode reduction takes place.

The copper is oxidized by air in seawater. The chemical reaction is written as,

Cu(s)+H2O(l)+12O2(g)→Cu(OH)2(s)

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Answer 2

Question

Chapter 19.8, Problem 1Q

Interpretation Introduction

Interpretation: It has to be explained the reason for if the paint is placed between the copper and the zinc, the zinc will still corrode in seawater, but it will not protect the copper from corrosion.

Concept introduction: Corrosion is a natural process. The destruction of metals by electrochemical reaction with water and oxygen in the air.

Sacrificial anodes are highly active metals that are used to prevent a less active metal surface from corrosion.

The loss of electrons is called oxidation whereas the gain of electrons is called reduction.

In an electrochemical cell, at anode oxidation takes place and at cathode reduction takes place.

The copper is oxidized by air in seawater. The chemical reaction is written as,

Cu(s)+H2O(l)+12O2(g)→Cu(OH)2(s)

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Answer 3

Question

Chapter 19.8, Problem 1Q

Interpretation Introduction

Interpretation: It has to be explained the reason for if the paint is placed between the copper and the zinc, the zinc will still corrode in seawater, but it will not protect the copper from corrosion.

Concept introduction: Corrosion is a natural process. The destruction of metals by electrochemical reaction with water and oxygen in the air.

Sacrificial anodes are highly active metals that are used to prevent a less active metal surface from corrosion.

The loss of electrons is called oxidation whereas the gain of electrons is called reduction.

In an electrochemical cell, at anode oxidation takes place and at cathode reduction takes place.

The copper is oxidized by air in seawater. The chemical reaction is written as,

Cu(s)+H2O(l)+12O2(g)→Cu(OH)2(s)

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Answer 4

Question

Chapter 19.8, Problem 1Q

Interpretation Introduction

Interpretation: It has to be explained the reason for if the paint is placed between the copper and the zinc, the zinc will still corrode in seawater, but it will not protect the copper from corrosion.

Concept introduction: Corrosion is a natural process. The destruction of metals by electrochemical reaction with water and oxygen in the air.

Sacrificial anodes are highly active metals that are used to prevent a less active metal surface from corrosion.

The loss of electrons is called oxidation whereas the gain of electrons is called reduction.

In an electrochemical cell, at anode oxidation takes place and at cathode reduction takes place.

The copper is oxidized by air in seawater. The chemical reaction is written as,

Cu(s)+H2O(l)+12O2(g)→Cu(OH)2(s)

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Answer 5

Chapter 19.8, Problem 1Q

Interpretation Introduction

Interpretation: It has to be explained the reason for if the paint is placed between the copper and the zinc, the zinc will still corrode in seawater, but it will not protect the copper from corrosion.

Concept introduction: Corrosion is a natural process. The destruction of metals by electrochemical reaction with water and oxygen in the air.

Sacrificial anodes are highly active metals that are used to prevent a less active metal surface from corrosion.

The loss of electrons is called oxidation whereas the gain of electrons is called reduction.

In an electrochemical cell, at anode oxidation takes place and at cathode reduction takes place.

The copper is oxidized by air in seawater. The chemical reaction is written as,

Cu(s)+H2O(l)+12O2(g)→Cu(OH)2(s)

Answer 6

Chapter 19.8, Problem 1Q

Interpretation Introduction

Interpretation: It has to be explained the reason for if the paint is placed between the copper and the zinc, the zinc will still corrode in seawater, but it will not protect the copper from corrosion.

Concept introduction: Corrosion is a natural process. The destruction of metals by electrochemical reaction with water and oxygen in the air.

Sacrificial anodes are highly active metals that are used to prevent a less active metal surface from corrosion.

The loss of electrons is called oxidation whereas the gain of electrons is called reduction.

In an electrochemical cell, at anode oxidation takes place and at cathode reduction takes place.

The copper is oxidized by air in seawater. The chemical reaction is written as,

Cu(s)+H2O(l)+12O2(g)→Cu(OH)2(s)

Answer 7

Chapter 19.8, Problem 1Q

Interpretation Introduction

Interpretation: It has to be explained the reason for if the paint is placed between the copper and the zinc, the zinc will still corrode in seawater, but it will not protect the copper from corrosion.

Concept introduction: Corrosion is a natural process. The destruction of metals by electrochemical reaction with water and oxygen in the air.

Sacrificial anodes are highly active metals that are used to prevent a less active metal surface from corrosion.

The loss of electrons is called oxidation whereas the gain of electrons is called reduction.

In an electrochemical cell, at anode oxidation takes place and at cathode reduction takes place.

The copper is oxidized by air in seawater. The chemical reaction is written as,

Cu(s)+H2O(l)+12O2(g)→Cu(OH)2(s)

Answer 8

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Answer 9

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Answer 10

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Answer 11

Ch. 19.1 - Prob. 2CYU Ch. 19.1 - Prob. 3CYU Ch. 19.1 - 1. Copper(II) sulfide reacts with nitric acid...Ch. 19.1 - Prob. 2RC Ch. 19.1 - The balanced half-reaction for Br2 BrO3 in basic...Ch. 19.2 - Describe how to set up a voltaic cell using the...Ch. 19.2 - The following overall chemical reaction occurs in...Ch. 19.2 - Prob. 1RC Ch. 19.2 - Prob. 2RC Ch. 19.2 - Prob. 3RC

Solution Summary: The author explains that if paint is placed between copper and zinc, the zinc will still corrode in seawater, but it will not protect the copper from corrosion.

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