The balanced equation for production of copper should be determined. Concept introduction: Most metals occur in nature as minerals which are generally some form of metal oxide, and the mineral must be refined to isolate the pure metal from the mineral. To isolate the pure metal from an ore (mineral), the ore is often concentrated and undergoes chemical treatment prior to reduction, the ore is then reduced to the free metal and the metal is then refined and purified. This process refers to metallurgy.

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Answer 1

Question

Chapter 21, Problem 21.1P

Interpretation Introduction

Interpretation: The balanced equation for production of copper should be determined.

Concept introduction:

Most metals occur in nature as minerals which are generally some form of metal oxide, and the mineral must be refined to isolate the pure metal from the mineral.

To isolate the pure metal from an ore (mineral), the ore is often concentrated and undergoes chemical treatment prior to reduction, the ore is then reduced to the free metal and the metal is then refined and purified. This process refers to metallurgy.

Expert Solution

Answer to Problem 21.1P

Solution:

Cu2S (s) + O2(g)→2 Cu (s) + SO2(g)

Explanation of Solution

We are asked to produce pure copper by roasting Cu₂S. In this instance, roasting refers to combustion which is a reaction with O₂(g). So, we know that Cu₂S reacts with O₂to produce pure Cu and must balance the remaining atoms:

Cu2S (s) + O2(g)→2 Cu (s) + SO2(g)

(c)

Interpretation Introduction

Interpretation: The balanced equation for production of lead should be determined.

Concept introduction:

Most metals occur in nature as minerals which are generally some form of metal oxide, and the mineral must be refined to isolate the pure metal from the mineral.

To isolate the pure metal from an ore (mineral), the ore is often concentrated and undergoes chemical treatment prior to reduction, the ore is then reduced to the free metal and the metal is then refined and purified. This process refers to metallurgy.

Expert Solution

Answer to Problem 21.1P

Solution:

PbO (s) + C (s)→Pb (s) + CO (g)

Explanation of Solution

We are asked to produce pure lead by reducing PbOwith coke. Coke refers to pure carbon, so we react pure carbon with PbOwhich produces pure Pband then we balance the remaining atoms:

PbO (s) + C (s)→Pb (s) + CO (g)

(d)

Interpretation Introduction

Interpretation: The balanced equation for production of potassium should be determined.

Concept introduction:

Most metals occur in nature as minerals which are generally some form of metal oxide, and the mineral must be refined to isolate the pure metal from the mineral.

To isolate the pure metal from an ore (mineral), the ore is often concentrated and undergoes chemical treatment prior to reduction, the ore is then reduced to the free metal and the metal is then refined and purified. This process refers to metallurgy.

Expert Solution

Answer to Problem 21.1P

Solution:

2 K+(l) + 2 Cl-(l)→2 K (l) + Cl2(g)

Explanation of Solution

We are asked to produce pure potassium by the electrolysis of molten KCl. Molten KClis when the substance ionizes by the ions are in liquid form rather than aqueous. So, we have liquid K+ reacting with liquid Cl- ions to produce pure K. Balancing the equation provides us with the production of Cl₂:

2 K+(l) + 2 Cl-(l)→2 K (l) + Cl2(g)

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Answer 2

Question

Chapter 21, Problem 21.1P

Interpretation Introduction

Interpretation: The balanced equation for production of copper should be determined.

Concept introduction:

Most metals occur in nature as minerals which are generally some form of metal oxide, and the mineral must be refined to isolate the pure metal from the mineral.

To isolate the pure metal from an ore (mineral), the ore is often concentrated and undergoes chemical treatment prior to reduction, the ore is then reduced to the free metal and the metal is then refined and purified. This process refers to metallurgy.

Expert Solution

Answer to Problem 21.1P

Solution:

Cu2S (s) + O2(g)→2 Cu (s) + SO2(g)

Explanation of Solution

We are asked to produce pure copper by roasting Cu₂S. In this instance, roasting refers to combustion which is a reaction with O₂(g). So, we know that Cu₂S reacts with O₂to produce pure Cu and must balance the remaining atoms:

Cu2S (s) + O2(g)→2 Cu (s) + SO2(g)

(c)

Interpretation Introduction

Interpretation: The balanced equation for production of lead should be determined.

Concept introduction:

Most metals occur in nature as minerals which are generally some form of metal oxide, and the mineral must be refined to isolate the pure metal from the mineral.

To isolate the pure metal from an ore (mineral), the ore is often concentrated and undergoes chemical treatment prior to reduction, the ore is then reduced to the free metal and the metal is then refined and purified. This process refers to metallurgy.

Expert Solution

Answer to Problem 21.1P

Solution:

PbO (s) + C (s)→Pb (s) + CO (g)

Explanation of Solution

We are asked to produce pure lead by reducing PbOwith coke. Coke refers to pure carbon, so we react pure carbon with PbOwhich produces pure Pband then we balance the remaining atoms:

PbO (s) + C (s)→Pb (s) + CO (g)

(d)

Interpretation Introduction

Interpretation: The balanced equation for production of potassium should be determined.

Concept introduction:

Most metals occur in nature as minerals which are generally some form of metal oxide, and the mineral must be refined to isolate the pure metal from the mineral.

To isolate the pure metal from an ore (mineral), the ore is often concentrated and undergoes chemical treatment prior to reduction, the ore is then reduced to the free metal and the metal is then refined and purified. This process refers to metallurgy.

Expert Solution

Answer to Problem 21.1P

Solution:

2 K+(l) + 2 Cl-(l)→2 K (l) + Cl2(g)

Explanation of Solution

We are asked to produce pure potassium by the electrolysis of molten KCl. Molten KClis when the substance ionizes by the ions are in liquid form rather than aqueous. So, we have liquid K+ reacting with liquid Cl- ions to produce pure K. Balancing the equation provides us with the production of Cl₂:

2 K+(l) + 2 Cl-(l)→2 K (l) + Cl2(g)

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Answer 3

Question

Chapter 21, Problem 21.1P

Interpretation Introduction

Interpretation: The balanced equation for production of copper should be determined.

Concept introduction:

Most metals occur in nature as minerals which are generally some form of metal oxide, and the mineral must be refined to isolate the pure metal from the mineral.

To isolate the pure metal from an ore (mineral), the ore is often concentrated and undergoes chemical treatment prior to reduction, the ore is then reduced to the free metal and the metal is then refined and purified. This process refers to metallurgy.

Expert Solution

Answer to Problem 21.1P

Solution:

Cu2S (s) + O2(g)→2 Cu (s) + SO2(g)

Explanation of Solution

We are asked to produce pure copper by roasting Cu₂S. In this instance, roasting refers to combustion which is a reaction with O₂(g). So, we know that Cu₂S reacts with O₂to produce pure Cu and must balance the remaining atoms:

Cu2S (s) + O2(g)→2 Cu (s) + SO2(g)

(c)

Interpretation Introduction

Interpretation: The balanced equation for production of lead should be determined.

Concept introduction:

Most metals occur in nature as minerals which are generally some form of metal oxide, and the mineral must be refined to isolate the pure metal from the mineral.

To isolate the pure metal from an ore (mineral), the ore is often concentrated and undergoes chemical treatment prior to reduction, the ore is then reduced to the free metal and the metal is then refined and purified. This process refers to metallurgy.

Expert Solution

Answer to Problem 21.1P

Solution:

PbO (s) + C (s)→Pb (s) + CO (g)

Explanation of Solution

We are asked to produce pure lead by reducing PbOwith coke. Coke refers to pure carbon, so we react pure carbon with PbOwhich produces pure Pband then we balance the remaining atoms:

PbO (s) + C (s)→Pb (s) + CO (g)

(d)

Interpretation Introduction

Interpretation: The balanced equation for production of potassium should be determined.

Concept introduction:

Most metals occur in nature as minerals which are generally some form of metal oxide, and the mineral must be refined to isolate the pure metal from the mineral.

To isolate the pure metal from an ore (mineral), the ore is often concentrated and undergoes chemical treatment prior to reduction, the ore is then reduced to the free metal and the metal is then refined and purified. This process refers to metallurgy.

Expert Solution

Answer to Problem 21.1P

Solution:

2 K+(l) + 2 Cl-(l)→2 K (l) + Cl2(g)

Explanation of Solution

We are asked to produce pure potassium by the electrolysis of molten KCl. Molten KClis when the substance ionizes by the ions are in liquid form rather than aqueous. So, we have liquid K+ reacting with liquid Cl- ions to produce pure K. Balancing the equation provides us with the production of Cl₂:

2 K+(l) + 2 Cl-(l)→2 K (l) + Cl2(g)

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Answer 4

Question

Chapter 21, Problem 21.1P

Interpretation Introduction

Interpretation: The balanced equation for production of copper should be determined.

Concept introduction:

Most metals occur in nature as minerals which are generally some form of metal oxide, and the mineral must be refined to isolate the pure metal from the mineral.

To isolate the pure metal from an ore (mineral), the ore is often concentrated and undergoes chemical treatment prior to reduction, the ore is then reduced to the free metal and the metal is then refined and purified. This process refers to metallurgy.

Expert Solution

Answer to Problem 21.1P

Solution:

Cu2S (s) + O2(g)→2 Cu (s) + SO2(g)

Explanation of Solution

We are asked to produce pure copper by roasting Cu₂S. In this instance, roasting refers to combustion which is a reaction with O₂(g). So, we know that Cu₂S reacts with O₂to produce pure Cu and must balance the remaining atoms:

Cu2S (s) + O2(g)→2 Cu (s) + SO2(g)

(c)

Interpretation Introduction

Interpretation: The balanced equation for production of lead should be determined.

Concept introduction:

Most metals occur in nature as minerals which are generally some form of metal oxide, and the mineral must be refined to isolate the pure metal from the mineral.

To isolate the pure metal from an ore (mineral), the ore is often concentrated and undergoes chemical treatment prior to reduction, the ore is then reduced to the free metal and the metal is then refined and purified. This process refers to metallurgy.

Expert Solution

Answer to Problem 21.1P

Solution:

PbO (s) + C (s)→Pb (s) + CO (g)

Explanation of Solution

We are asked to produce pure lead by reducing PbOwith coke. Coke refers to pure carbon, so we react pure carbon with PbOwhich produces pure Pband then we balance the remaining atoms:

PbO (s) + C (s)→Pb (s) + CO (g)

(d)

Interpretation Introduction

Interpretation: The balanced equation for production of potassium should be determined.

Concept introduction:

Most metals occur in nature as minerals which are generally some form of metal oxide, and the mineral must be refined to isolate the pure metal from the mineral.

To isolate the pure metal from an ore (mineral), the ore is often concentrated and undergoes chemical treatment prior to reduction, the ore is then reduced to the free metal and the metal is then refined and purified. This process refers to metallurgy.

Expert Solution

Answer to Problem 21.1P

Solution:

2 K+(l) + 2 Cl-(l)→2 K (l) + Cl2(g)

Explanation of Solution

We are asked to produce pure potassium by the electrolysis of molten KCl. Molten KClis when the substance ionizes by the ions are in liquid form rather than aqueous. So, we have liquid K+ reacting with liquid Cl- ions to produce pure K. Balancing the equation provides us with the production of Cl₂:

2 K+(l) + 2 Cl-(l)→2 K (l) + Cl2(g)

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Answer 5

Chapter 21, Problem 21.1P

Interpretation Introduction

Interpretation: The balanced equation for production of copper should be determined.

Concept introduction:

Most metals occur in nature as minerals which are generally some form of metal oxide, and the mineral must be refined to isolate the pure metal from the mineral.

To isolate the pure metal from an ore (mineral), the ore is often concentrated and undergoes chemical treatment prior to reduction, the ore is then reduced to the free metal and the metal is then refined and purified. This process refers to metallurgy.

Expert Solution

Answer to Problem 21.1P

Solution:

Cu2S (s) + O2(g)→2 Cu (s) + SO2(g)

Explanation of Solution

We are asked to produce pure copper by roasting Cu₂S. In this instance, roasting refers to combustion which is a reaction with O₂(g). So, we know that Cu₂S reacts with O₂to produce pure Cu and must balance the remaining atoms:

Cu2S (s) + O2(g)→2 Cu (s) + SO2(g)

(c)

Interpretation Introduction

Interpretation: The balanced equation for production of lead should be determined.

Concept introduction:

Most metals occur in nature as minerals which are generally some form of metal oxide, and the mineral must be refined to isolate the pure metal from the mineral.

To isolate the pure metal from an ore (mineral), the ore is often concentrated and undergoes chemical treatment prior to reduction, the ore is then reduced to the free metal and the metal is then refined and purified. This process refers to metallurgy.

Expert Solution

Answer to Problem 21.1P

Solution:

PbO (s) + C (s)→Pb (s) + CO (g)

Explanation of Solution

We are asked to produce pure lead by reducing PbOwith coke. Coke refers to pure carbon, so we react pure carbon with PbOwhich produces pure Pband then we balance the remaining atoms:

PbO (s) + C (s)→Pb (s) + CO (g)

(d)

Interpretation Introduction

Interpretation: The balanced equation for production of potassium should be determined.

Concept introduction:

Most metals occur in nature as minerals which are generally some form of metal oxide, and the mineral must be refined to isolate the pure metal from the mineral.

To isolate the pure metal from an ore (mineral), the ore is often concentrated and undergoes chemical treatment prior to reduction, the ore is then reduced to the free metal and the metal is then refined and purified. This process refers to metallurgy.

Expert Solution

Answer to Problem 21.1P

Solution:

2 K+(l) + 2 Cl-(l)→2 K (l) + Cl2(g)

Explanation of Solution

We are asked to produce pure potassium by the electrolysis of molten KCl. Molten KClis when the substance ionizes by the ions are in liquid form rather than aqueous. So, we have liquid K+ reacting with liquid Cl- ions to produce pure K. Balancing the equation provides us with the production of Cl₂:

2 K+(l) + 2 Cl-(l)→2 K (l) + Cl2(g)

Answer 6

Chapter 21, Problem 21.1P

Interpretation Introduction

Interpretation: The balanced equation for production of copper should be determined.

Concept introduction:

Most metals occur in nature as minerals which are generally some form of metal oxide, and the mineral must be refined to isolate the pure metal from the mineral.

To isolate the pure metal from an ore (mineral), the ore is often concentrated and undergoes chemical treatment prior to reduction, the ore is then reduced to the free metal and the metal is then refined and purified. This process refers to metallurgy.

Expert Solution

Answer to Problem 21.1P

Solution:

Cu2S (s) + O2(g)→2 Cu (s) + SO2(g)

Explanation of Solution

We are asked to produce pure copper by roasting Cu₂S. In this instance, roasting refers to combustion which is a reaction with O₂(g). So, we know that Cu₂S reacts with O₂to produce pure Cu and must balance the remaining atoms:

Cu2S (s) + O2(g)→2 Cu (s) + SO2(g)

(c)

Answer 7

Chapter 21, Problem 21.1P

Interpretation Introduction

Interpretation: The balanced equation for production of copper should be determined.

Concept introduction:

Most metals occur in nature as minerals which are generally some form of metal oxide, and the mineral must be refined to isolate the pure metal from the mineral.

To isolate the pure metal from an ore (mineral), the ore is often concentrated and undergoes chemical treatment prior to reduction, the ore is then reduced to the free metal and the metal is then refined and purified. This process refers to metallurgy.

Answer 8

Expert Solution

Answer to Problem 21.1P

Solution:

Cu2S (s) + O2(g)→2 Cu (s) + SO2(g)

Answer 9

Expert Solution

Answer 10

Expert Solution

Answer 11

Expert Solution

Answer 12

Explanation of Solution

We are asked to produce pure copper by roasting Cu₂S. In this instance, roasting refers to combustion which is a reaction with O₂(g). So, we know that Cu₂S reacts with O₂to produce pure Cu and must balance the remaining atoms:

Cu2S (s) + O2(g)→2 Cu (s) + SO2(g)

(c)

Answer 13

Interpretation Introduction

Interpretation: The balanced equation for production of lead should be determined.

Concept introduction:

Most metals occur in nature as minerals which are generally some form of metal oxide, and the mineral must be refined to isolate the pure metal from the mineral.

To isolate the pure metal from an ore (mineral), the ore is often concentrated and undergoes chemical treatment prior to reduction, the ore is then reduced to the free metal and the metal is then refined and purified. This process refers to metallurgy.

Expert Solution

Answer to Problem 21.1P

Solution:

PbO (s) + C (s)→Pb (s) + CO (g)

Explanation of Solution

We are asked to produce pure lead by reducing PbOwith coke. Coke refers to pure carbon, so we react pure carbon with PbOwhich produces pure Pband then we balance the remaining atoms:

PbO (s) + C (s)→Pb (s) + CO (g)

(d)

Answer 14

Interpretation Introduction

Interpretation: The balanced equation for production of lead should be determined.

Concept introduction:

Most metals occur in nature as minerals which are generally some form of metal oxide, and the mineral must be refined to isolate the pure metal from the mineral.

To isolate the pure metal from an ore (mineral), the ore is often concentrated and undergoes chemical treatment prior to reduction, the ore is then reduced to the free metal and the metal is then refined and purified. This process refers to metallurgy.

Answer 15

Expert Solution

Answer to Problem 21.1P

Solution:

PbO (s) + C (s)→Pb (s) + CO (g)

Answer 16

Expert Solution

Answer 17

Expert Solution

Answer 18

Expert Solution

Answer 19

Explanation of Solution

We are asked to produce pure lead by reducing PbOwith coke. Coke refers to pure carbon, so we react pure carbon with PbOwhich produces pure Pband then we balance the remaining atoms:

PbO (s) + C (s)→Pb (s) + CO (g)

(d)

Answer 20

Interpretation Introduction

Interpretation: The balanced equation for production of potassium should be determined.

Concept introduction:

Most metals occur in nature as minerals which are generally some form of metal oxide, and the mineral must be refined to isolate the pure metal from the mineral.

To isolate the pure metal from an ore (mineral), the ore is often concentrated and undergoes chemical treatment prior to reduction, the ore is then reduced to the free metal and the metal is then refined and purified. This process refers to metallurgy.

Expert Solution

Answer to Problem 21.1P

Solution:

2 K+(l) + 2 Cl-(l)→2 K (l) + Cl2(g)

Explanation of Solution

We are asked to produce pure potassium by the electrolysis of molten KCl. Molten KClis when the substance ionizes by the ions are in liquid form rather than aqueous. So, we have liquid K+ reacting with liquid Cl- ions to produce pure K. Balancing the equation provides us with the production of Cl₂:

2 K+(l) + 2 Cl-(l)→2 K (l) + Cl2(g)

Answer 21

Interpretation Introduction

Interpretation: The balanced equation for production of potassium should be determined.

Concept introduction:

Most metals occur in nature as minerals which are generally some form of metal oxide, and the mineral must be refined to isolate the pure metal from the mineral.

To isolate the pure metal from an ore (mineral), the ore is often concentrated and undergoes chemical treatment prior to reduction, the ore is then reduced to the free metal and the metal is then refined and purified. This process refers to metallurgy.

Answer 22

Expert Solution

Answer to Problem 21.1P

Solution:

2 K+(l) + 2 Cl-(l)→2 K (l) + Cl2(g)

Answer 23

Expert Solution

Answer 24

Expert Solution

Answer 25

Expert Solution

Answer 26

Explanation of Solution

We are asked to produce pure potassium by the electrolysis of molten KCl. Molten KClis when the substance ionizes by the ions are in liquid form rather than aqueous. So, we have liquid K+ reacting with liquid Cl- ions to produce pure K. Balancing the equation provides us with the production of Cl₂:

2 K+(l) + 2 Cl-(l)→2 K (l) + Cl2(g)