Sketch a galvanic cell, and explain how it works. Look at Figs. 18.1 and 18.5. Explain what is occurring in each container and why the cell in Fig. 18.5 “works,” but the one in Fig. 18.1 does not.

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Answer 1

Textbook Question

Chapter 18, Problem 1ALQ

Sketch a galvanic cell, and explain how it works. Look at Figs. 18.1 and 18.5. Explain what is occurring in each container and why the cell in Fig. 18.5 “works,” but the one in Fig. 18.1 does not.

Expert Solution & Answer

Interpretation Introduction

Interpretation: A galvanic cell should be sketched and how it works should be explained. Considering the figures 18.1 and 18.5 , what is occurring in each container should be explained and why the cell in figure 18.5 works, but the one in figure 18.1 does not should be discussed.

Concept Introduction:A Galvanic cell also known as electrochemical battery, a device that exploits a spontaneous oxidation reduction reaction to produce electrical energy. Here oxidizing agent and reducing agent has been separated, so that the electron/s generated by oxidation should travel through a wire from reducing agent to oxidizing agent.

Explanation of Solution

The galvanic cell is sketched as follows:

Student Solutions Manual for Zumdahl/DeCoste's Introductory Chemistry: A Foundation, 9th, Chapter 18, Problem 1ALQ

When reducing agent and oxidizing agent mixed together in a container, electron transfer occurs. But chemical energy generated by this cannot be used for any work. This can be achieved by separating the reducing agent and oxidizing agent and let the electron transfer happen through a wire. So electrons removing from the reducing agent will travel through the wire to the oxidizing agent. The electric current generated by the electron flow through the wire can be directed through an electronic device. To keep the net charge of each container zero, the two solutions are connected by a salt bridge which filled with strong electrolyte.

In the figure 18.1 , the beaker in the left contains the oxidizing agent, MnO₄²^-, which undergoes reduction by accepting electrons and forms Mn²⁺. The beaker in the right contains the reducing agent, Fe²+ which undergoes oxidation by removing electrons and converts into Fe³⁺.

According to the figure 18.1 , electrons flow only from reducing agent to the oxidizing agent. this will build up a negative charge in the left container and a positive charge in the right container. This will create a charge separation and to create charge separation large amount of energy is needed. So, no electron flow occurs under these conditions. This problem has been solved in the figure 18.5 . The solutions have been connected through a salt bridge without mixing the two solutions. Therefore the electrons from the reducing agent will flow through the wire to the oxidizing agent and the ions in the aqueous solution flows from one container to the other through salt bridge keeping the net charge of the each container zero.

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3. Titanium(III) chloride can be used to catalyze the polymerization of ethylene. It is prepared by hydrogen reduction of Titanium(IV) chloride. Reaction of hydrogen gas with titanium(IV) chloride gas produces solid titanium(III) chloride and hydrogen chloride gas. (a) Write a BALANCED chemical reaction for the preparation of titanium(III) chloride (b) A 250 L reaction vessel at 325°C is filled with hydrogen gas to a pressure of 1.3 atm. Titanium(IV) chloride is then added to bring the total pressure to 3.00 atm. How many grams of titanium(III) chloride will be produced after completion of the reaction? (c) What will be the pressure of the resulting hydrogen chloride gas that is also produced?

Answer 2

Textbook Question

Chapter 18, Problem 1ALQ

Sketch a galvanic cell, and explain how it works. Look at Figs. 18.1 and 18.5. Explain what is occurring in each container and why the cell in Fig. 18.5 “works,” but the one in Fig. 18.1 does not.

Expert Solution & Answer

Interpretation Introduction

Interpretation: A galvanic cell should be sketched and how it works should be explained. Considering the figures 18.1 and 18.5 , what is occurring in each container should be explained and why the cell in figure 18.5 works, but the one in figure 18.1 does not should be discussed.

Concept Introduction:A Galvanic cell also known as electrochemical battery, a device that exploits a spontaneous oxidation reduction reaction to produce electrical energy. Here oxidizing agent and reducing agent has been separated, so that the electron/s generated by oxidation should travel through a wire from reducing agent to oxidizing agent.

Explanation of Solution

The galvanic cell is sketched as follows:

Student Solutions Manual for Zumdahl/DeCoste's Introductory Chemistry: A Foundation, 9th, Chapter 18, Problem 1ALQ

When reducing agent and oxidizing agent mixed together in a container, electron transfer occurs. But chemical energy generated by this cannot be used for any work. This can be achieved by separating the reducing agent and oxidizing agent and let the electron transfer happen through a wire. So electrons removing from the reducing agent will travel through the wire to the oxidizing agent. The electric current generated by the electron flow through the wire can be directed through an electronic device. To keep the net charge of each container zero, the two solutions are connected by a salt bridge which filled with strong electrolyte.

In the figure 18.1 , the beaker in the left contains the oxidizing agent, MnO₄²^-, which undergoes reduction by accepting electrons and forms Mn²⁺. The beaker in the right contains the reducing agent, Fe²+ which undergoes oxidation by removing electrons and converts into Fe³⁺.

According to the figure 18.1 , electrons flow only from reducing agent to the oxidizing agent. this will build up a negative charge in the left container and a positive charge in the right container. This will create a charge separation and to create charge separation large amount of energy is needed. So, no electron flow occurs under these conditions. This problem has been solved in the figure 18.5 . The solutions have been connected through a salt bridge without mixing the two solutions. Therefore the electrons from the reducing agent will flow through the wire to the oxidizing agent and the ions in the aqueous solution flows from one container to the other through salt bridge keeping the net charge of the each container zero.

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Answer 3

Textbook Question

Chapter 18, Problem 1ALQ

Sketch a galvanic cell, and explain how it works. Look at Figs. 18.1 and 18.5. Explain what is occurring in each container and why the cell in Fig. 18.5 “works,” but the one in Fig. 18.1 does not.

Expert Solution & Answer

Interpretation Introduction

Interpretation: A galvanic cell should be sketched and how it works should be explained. Considering the figures 18.1 and 18.5 , what is occurring in each container should be explained and why the cell in figure 18.5 works, but the one in figure 18.1 does not should be discussed.

Concept Introduction:A Galvanic cell also known as electrochemical battery, a device that exploits a spontaneous oxidation reduction reaction to produce electrical energy. Here oxidizing agent and reducing agent has been separated, so that the electron/s generated by oxidation should travel through a wire from reducing agent to oxidizing agent.

Explanation of Solution

The galvanic cell is sketched as follows:

Student Solutions Manual for Zumdahl/DeCoste's Introductory Chemistry: A Foundation, 9th, Chapter 18, Problem 1ALQ

When reducing agent and oxidizing agent mixed together in a container, electron transfer occurs. But chemical energy generated by this cannot be used for any work. This can be achieved by separating the reducing agent and oxidizing agent and let the electron transfer happen through a wire. So electrons removing from the reducing agent will travel through the wire to the oxidizing agent. The electric current generated by the electron flow through the wire can be directed through an electronic device. To keep the net charge of each container zero, the two solutions are connected by a salt bridge which filled with strong electrolyte.

In the figure 18.1 , the beaker in the left contains the oxidizing agent, MnO₄²^-, which undergoes reduction by accepting electrons and forms Mn²⁺. The beaker in the right contains the reducing agent, Fe²+ which undergoes oxidation by removing electrons and converts into Fe³⁺.

According to the figure 18.1 , electrons flow only from reducing agent to the oxidizing agent. this will build up a negative charge in the left container and a positive charge in the right container. This will create a charge separation and to create charge separation large amount of energy is needed. So, no electron flow occurs under these conditions. This problem has been solved in the figure 18.5 . The solutions have been connected through a salt bridge without mixing the two solutions. Therefore the electrons from the reducing agent will flow through the wire to the oxidizing agent and the ions in the aqueous solution flows from one container to the other through salt bridge keeping the net charge of the each container zero.

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Answer 4

Textbook Question

Chapter 18, Problem 1ALQ

Sketch a galvanic cell, and explain how it works. Look at Figs. 18.1 and 18.5. Explain what is occurring in each container and why the cell in Fig. 18.5 “works,” but the one in Fig. 18.1 does not.

Expert Solution & Answer

Interpretation Introduction

Interpretation: A galvanic cell should be sketched and how it works should be explained. Considering the figures 18.1 and 18.5 , what is occurring in each container should be explained and why the cell in figure 18.5 works, but the one in figure 18.1 does not should be discussed.

Concept Introduction:A Galvanic cell also known as electrochemical battery, a device that exploits a spontaneous oxidation reduction reaction to produce electrical energy. Here oxidizing agent and reducing agent has been separated, so that the electron/s generated by oxidation should travel through a wire from reducing agent to oxidizing agent.

Explanation of Solution

The galvanic cell is sketched as follows:

Student Solutions Manual for Zumdahl/DeCoste's Introductory Chemistry: A Foundation, 9th, Chapter 18, Problem 1ALQ

When reducing agent and oxidizing agent mixed together in a container, electron transfer occurs. But chemical energy generated by this cannot be used for any work. This can be achieved by separating the reducing agent and oxidizing agent and let the electron transfer happen through a wire. So electrons removing from the reducing agent will travel through the wire to the oxidizing agent. The electric current generated by the electron flow through the wire can be directed through an electronic device. To keep the net charge of each container zero, the two solutions are connected by a salt bridge which filled with strong electrolyte.

In the figure 18.1 , the beaker in the left contains the oxidizing agent, MnO₄²^-, which undergoes reduction by accepting electrons and forms Mn²⁺. The beaker in the right contains the reducing agent, Fe²+ which undergoes oxidation by removing electrons and converts into Fe³⁺.

According to the figure 18.1 , electrons flow only from reducing agent to the oxidizing agent. this will build up a negative charge in the left container and a positive charge in the right container. This will create a charge separation and to create charge separation large amount of energy is needed. So, no electron flow occurs under these conditions. This problem has been solved in the figure 18.5 . The solutions have been connected through a salt bridge without mixing the two solutions. Therefore the electrons from the reducing agent will flow through the wire to the oxidizing agent and the ions in the aqueous solution flows from one container to the other through salt bridge keeping the net charge of the each container zero.

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Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 5

Textbook Question

Answer 6

Textbook Question

Answer 7

Expert Solution & Answer

Interpretation Introduction

Interpretation: A galvanic cell should be sketched and how it works should be explained. Considering the figures 18.1 and 18.5 , what is occurring in each container should be explained and why the cell in figure 18.5 works, but the one in figure 18.1 does not should be discussed.

Concept Introduction:A Galvanic cell also known as electrochemical battery, a device that exploits a spontaneous oxidation reduction reaction to produce electrical energy. Here oxidizing agent and reducing agent has been separated, so that the electron/s generated by oxidation should travel through a wire from reducing agent to oxidizing agent.

Explanation of Solution

The galvanic cell is sketched as follows:

Student Solutions Manual for Zumdahl/DeCoste's Introductory Chemistry: A Foundation, 9th, Chapter 18, Problem 1ALQ

When reducing agent and oxidizing agent mixed together in a container, electron transfer occurs. But chemical energy generated by this cannot be used for any work. This can be achieved by separating the reducing agent and oxidizing agent and let the electron transfer happen through a wire. So electrons removing from the reducing agent will travel through the wire to the oxidizing agent. The electric current generated by the electron flow through the wire can be directed through an electronic device. To keep the net charge of each container zero, the two solutions are connected by a salt bridge which filled with strong electrolyte.

In the figure 18.1 , the beaker in the left contains the oxidizing agent, MnO₄²^-, which undergoes reduction by accepting electrons and forms Mn²⁺. The beaker in the right contains the reducing agent, Fe²+ which undergoes oxidation by removing electrons and converts into Fe³⁺.

According to the figure 18.1 , electrons flow only from reducing agent to the oxidizing agent. this will build up a negative charge in the left container and a positive charge in the right container. This will create a charge separation and to create charge separation large amount of energy is needed. So, no electron flow occurs under these conditions. This problem has been solved in the figure 18.5 . The solutions have been connected through a salt bridge without mixing the two solutions. Therefore the electrons from the reducing agent will flow through the wire to the oxidizing agent and the ions in the aqueous solution flows from one container to the other through salt bridge keeping the net charge of the each container zero.

Answer 8

Expert Solution & Answer

Interpretation Introduction

Interpretation: A galvanic cell should be sketched and how it works should be explained. Considering the figures 18.1 and 18.5 , what is occurring in each container should be explained and why the cell in figure 18.5 works, but the one in figure 18.1 does not should be discussed.

Concept Introduction:A Galvanic cell also known as electrochemical battery, a device that exploits a spontaneous oxidation reduction reaction to produce electrical energy. Here oxidizing agent and reducing agent has been separated, so that the electron/s generated by oxidation should travel through a wire from reducing agent to oxidizing agent.

Explanation of Solution

The galvanic cell is sketched as follows:

Student Solutions Manual for Zumdahl/DeCoste's Introductory Chemistry: A Foundation, 9th, Chapter 18, Problem 1ALQ

When reducing agent and oxidizing agent mixed together in a container, electron transfer occurs. But chemical energy generated by this cannot be used for any work. This can be achieved by separating the reducing agent and oxidizing agent and let the electron transfer happen through a wire. So electrons removing from the reducing agent will travel through the wire to the oxidizing agent. The electric current generated by the electron flow through the wire can be directed through an electronic device. To keep the net charge of each container zero, the two solutions are connected by a salt bridge which filled with strong electrolyte.

In the figure 18.1 , the beaker in the left contains the oxidizing agent, MnO₄²^-, which undergoes reduction by accepting electrons and forms Mn²⁺. The beaker in the right contains the reducing agent, Fe²+ which undergoes oxidation by removing electrons and converts into Fe³⁺.

According to the figure 18.1 , electrons flow only from reducing agent to the oxidizing agent. this will build up a negative charge in the left container and a positive charge in the right container. This will create a charge separation and to create charge separation large amount of energy is needed. So, no electron flow occurs under these conditions. This problem has been solved in the figure 18.5 . The solutions have been connected through a salt bridge without mixing the two solutions. Therefore the electrons from the reducing agent will flow through the wire to the oxidizing agent and the ions in the aqueous solution flows from one container to the other through salt bridge keeping the net charge of the each container zero.

Answer 9

Expert Solution & Answer

Answer 10

Expert Solution & Answer

Answer 11

Interpretation Introduction

Interpretation: A galvanic cell should be sketched and how it works should be explained. Considering the figures 18.1 and 18.5 , what is occurring in each container should be explained and why the cell in figure 18.5 works, but the one in figure 18.1 does not should be discussed.

Concept Introduction:A Galvanic cell also known as electrochemical battery, a device that exploits a spontaneous oxidation reduction reaction to produce electrical energy. Here oxidizing agent and reducing agent has been separated, so that the electron/s generated by oxidation should travel through a wire from reducing agent to oxidizing agent.

Answer 12

Explanation of Solution

The galvanic cell is sketched as follows:

Student Solutions Manual for Zumdahl/DeCoste's Introductory Chemistry: A Foundation, 9th, Chapter 18, Problem 1ALQ

When reducing agent and oxidizing agent mixed together in a container, electron transfer occurs. But chemical energy generated by this cannot be used for any work. This can be achieved by separating the reducing agent and oxidizing agent and let the electron transfer happen through a wire. So electrons removing from the reducing agent will travel through the wire to the oxidizing agent. The electric current generated by the electron flow through the wire can be directed through an electronic device. To keep the net charge of each container zero, the two solutions are connected by a salt bridge which filled with strong electrolyte.

In the figure 18.1 , the beaker in the left contains the oxidizing agent, MnO₄²^-, which undergoes reduction by accepting electrons and forms Mn²⁺. The beaker in the right contains the reducing agent, Fe²+ which undergoes oxidation by removing electrons and converts into Fe³⁺.

According to the figure 18.1 , electrons flow only from reducing agent to the oxidizing agent. this will build up a negative charge in the left container and a positive charge in the right container. This will create a charge separation and to create charge separation large amount of energy is needed. So, no electron flow occurs under these conditions. This problem has been solved in the figure 18.5 . The solutions have been connected through a salt bridge without mixing the two solutions. Therefore the electrons from the reducing agent will flow through the wire to the oxidizing agent and the ions in the aqueous solution flows from one container to the other through salt bridge keeping the net charge of the each container zero.

Answer 13

Ch. 18.1 - Prob. 18.1SC Ch. 18.2 - Prob. 1CT Ch. 18.2 - Prob. 18.2SC Ch. 18.3 - Prob. 18.3SC Ch. 18.4 - Prob. 18.4SC Ch. 18.7 - Prob. 1CT Ch. 18 - Sketch a galvanic cell, and explain how it works....Ch. 18 - Prob. 2ALQ Ch. 18 - Which of the following are oxidation-reduction...Ch. 18 - Prob. 4ALQ

Sketch a galvanic cell, and explain how it works. Look at Figs. 18.1 and 18.5. Explain what is occurring in each container and why the cell in Fig. 18.5 “works,” but the one in Fig. 18.1 does not.

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