A voltaic cell is given. The greater density of a concentrated solution of CuSO 4 is given to allow a less concentrated solution of ZnSO 4 solution to be layered on top of it. An explanation for the porous bridge not being needed in the given cell is to be stated. Concept introduction: Voltaic cell is a type of electrochemical cell which converts the chemical energy to electrical energy. This chemical energy generates by processing the redox reaction . Redox reaction is the combination of two half reactions. One half reactions is known as reduction half while other is oxidation half. Salt bridge, also known as porous bridge is a U-shaped hollow device which is filled with KOH or other electrolytes. It is used to maintain the electrical neutrality during the process of redox reactions in two different compartments. To determine: An explanation for the porous bridge not being needed in the given cell.

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Answer 1

Question

Chapter 18, Problem 18.1VP

Interpretation Introduction

Interpretation: A voltaic cell is given. The greater density of a concentrated solution of CuSO4 is given to allow a less concentrated solution of ZnSO4 solution to be layered on top of it. An explanation for the porous bridge not being needed in the given cell is to be stated.

Concept introduction: Voltaic cell is a type of electrochemical cell which converts the chemical energy to electrical energy. This chemical energy generates by processing the redox reaction. Redox reaction is the combination of two half reactions. One half reactions is known as reduction half while other is oxidation half.

Salt bridge, also known as porous bridge is a U-shaped hollow device which is filled with KOH or other electrolytes. It is used to maintain the electrical neutrality during the process of redox reactions in two different compartments.

To determine: An explanation for the porous bridge not being needed in the given cell.

Expert Solution & Answer

Answer to Problem 18.1VP

Solution

An explanation for the porous bridge not being needed in the given cell has been rightfully stated.

Explanation of Solution

Explanation

In voltaic cell during the process of redox reaction electrons are generated on anode and then transfer to the cathode by the external circuit. In this way we can say that the process of oxidation occurs at the anode and the process of reduction occurs at cathode.

Oxidation is a process in which loss of electrons take place, while in reduction gain of electron take place.

The voltaic cell is given as,

Chemistry: The Science in Context (Fifth Edition), Chapter 18, Problem 18.1VP

Figure 1

From the above Figure 1 it is clear that two concentrated solutions, have different densities are present in a beaker. The concentrated solution which has the greater density allows the lass concentrated solution to be layered on its top. The Figure 1 shows that one electrode is attached with zinc metal. The other electrode is attached with copper metal. Therefore, the process of oxidation occurs at zinc. Hence, electrons move from zinc metal to copper. After the loss of electrons the zinc metal converts to zinc ion. After the gain of electrons the copper metal converts to copper ion. From the above Figure 1 it is clear that the number of gained and loosed electrons is automatically balanced without interference of external source. Therefore, the electrical neutrality is automatically maintained here. Hence, in the form of reaction the above process is represented as,

Zn(s)+CuSO4(aq)→Cu(s)+ZnSO4(aq)

Hence, it is explained that the porous bridge is not needed in the voltaic cell.

Conclusion

An explanation for the porous bridge not being needed in the given cell has been rightfully stated

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Answer 2

Question

Chapter 18, Problem 18.1VP

Interpretation Introduction

Interpretation: A voltaic cell is given. The greater density of a concentrated solution of CuSO4 is given to allow a less concentrated solution of ZnSO4 solution to be layered on top of it. An explanation for the porous bridge not being needed in the given cell is to be stated.

Concept introduction: Voltaic cell is a type of electrochemical cell which converts the chemical energy to electrical energy. This chemical energy generates by processing the redox reaction. Redox reaction is the combination of two half reactions. One half reactions is known as reduction half while other is oxidation half.

Salt bridge, also known as porous bridge is a U-shaped hollow device which is filled with KOH or other electrolytes. It is used to maintain the electrical neutrality during the process of redox reactions in two different compartments.

To determine: An explanation for the porous bridge not being needed in the given cell.

Expert Solution & Answer

Answer to Problem 18.1VP

Solution

An explanation for the porous bridge not being needed in the given cell has been rightfully stated.

Explanation of Solution

Explanation

In voltaic cell during the process of redox reaction electrons are generated on anode and then transfer to the cathode by the external circuit. In this way we can say that the process of oxidation occurs at the anode and the process of reduction occurs at cathode.

Oxidation is a process in which loss of electrons take place, while in reduction gain of electron take place.

The voltaic cell is given as,

Chemistry: The Science in Context (Fifth Edition), Chapter 18, Problem 18.1VP

Figure 1

From the above Figure 1 it is clear that two concentrated solutions, have different densities are present in a beaker. The concentrated solution which has the greater density allows the lass concentrated solution to be layered on its top. The Figure 1 shows that one electrode is attached with zinc metal. The other electrode is attached with copper metal. Therefore, the process of oxidation occurs at zinc. Hence, electrons move from zinc metal to copper. After the loss of electrons the zinc metal converts to zinc ion. After the gain of electrons the copper metal converts to copper ion. From the above Figure 1 it is clear that the number of gained and loosed electrons is automatically balanced without interference of external source. Therefore, the electrical neutrality is automatically maintained here. Hence, in the form of reaction the above process is represented as,

Zn(s)+CuSO4(aq)→Cu(s)+ZnSO4(aq)

Hence, it is explained that the porous bridge is not needed in the voltaic cell.

Conclusion

An explanation for the porous bridge not being needed in the given cell has been rightfully stated

Want to see more full solutions like this?

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

Answer 3

Question

Chapter 18, Problem 18.1VP

Interpretation Introduction

Interpretation: A voltaic cell is given. The greater density of a concentrated solution of CuSO4 is given to allow a less concentrated solution of ZnSO4 solution to be layered on top of it. An explanation for the porous bridge not being needed in the given cell is to be stated.

Concept introduction: Voltaic cell is a type of electrochemical cell which converts the chemical energy to electrical energy. This chemical energy generates by processing the redox reaction. Redox reaction is the combination of two half reactions. One half reactions is known as reduction half while other is oxidation half.

Salt bridge, also known as porous bridge is a U-shaped hollow device which is filled with KOH or other electrolytes. It is used to maintain the electrical neutrality during the process of redox reactions in two different compartments.

To determine: An explanation for the porous bridge not being needed in the given cell.

Expert Solution & Answer

Answer to Problem 18.1VP

Solution

An explanation for the porous bridge not being needed in the given cell has been rightfully stated.

Explanation of Solution

Explanation

In voltaic cell during the process of redox reaction electrons are generated on anode and then transfer to the cathode by the external circuit. In this way we can say that the process of oxidation occurs at the anode and the process of reduction occurs at cathode.

Oxidation is a process in which loss of electrons take place, while in reduction gain of electron take place.

The voltaic cell is given as,

Chemistry: The Science in Context (Fifth Edition), Chapter 18, Problem 18.1VP

Figure 1

From the above Figure 1 it is clear that two concentrated solutions, have different densities are present in a beaker. The concentrated solution which has the greater density allows the lass concentrated solution to be layered on its top. The Figure 1 shows that one electrode is attached with zinc metal. The other electrode is attached with copper metal. Therefore, the process of oxidation occurs at zinc. Hence, electrons move from zinc metal to copper. After the loss of electrons the zinc metal converts to zinc ion. After the gain of electrons the copper metal converts to copper ion. From the above Figure 1 it is clear that the number of gained and loosed electrons is automatically balanced without interference of external source. Therefore, the electrical neutrality is automatically maintained here. Hence, in the form of reaction the above process is represented as,

Zn(s)+CuSO4(aq)→Cu(s)+ZnSO4(aq)

Hence, it is explained that the porous bridge is not needed in the voltaic cell.

Conclusion

An explanation for the porous bridge not being needed in the given cell has been rightfully stated

Want to see more full solutions like this?

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

Answer 4

Question

Chapter 18, Problem 18.1VP

Interpretation Introduction

Interpretation: A voltaic cell is given. The greater density of a concentrated solution of CuSO4 is given to allow a less concentrated solution of ZnSO4 solution to be layered on top of it. An explanation for the porous bridge not being needed in the given cell is to be stated.

Concept introduction: Voltaic cell is a type of electrochemical cell which converts the chemical energy to electrical energy. This chemical energy generates by processing the redox reaction. Redox reaction is the combination of two half reactions. One half reactions is known as reduction half while other is oxidation half.

Salt bridge, also known as porous bridge is a U-shaped hollow device which is filled with KOH or other electrolytes. It is used to maintain the electrical neutrality during the process of redox reactions in two different compartments.

To determine: An explanation for the porous bridge not being needed in the given cell.

Expert Solution & Answer

Answer to Problem 18.1VP

Solution

An explanation for the porous bridge not being needed in the given cell has been rightfully stated.

Explanation of Solution

Explanation

In voltaic cell during the process of redox reaction electrons are generated on anode and then transfer to the cathode by the external circuit. In this way we can say that the process of oxidation occurs at the anode and the process of reduction occurs at cathode.

Oxidation is a process in which loss of electrons take place, while in reduction gain of electron take place.

The voltaic cell is given as,

Chemistry: The Science in Context (Fifth Edition), Chapter 18, Problem 18.1VP

Figure 1

From the above Figure 1 it is clear that two concentrated solutions, have different densities are present in a beaker. The concentrated solution which has the greater density allows the lass concentrated solution to be layered on its top. The Figure 1 shows that one electrode is attached with zinc metal. The other electrode is attached with copper metal. Therefore, the process of oxidation occurs at zinc. Hence, electrons move from zinc metal to copper. After the loss of electrons the zinc metal converts to zinc ion. After the gain of electrons the copper metal converts to copper ion. From the above Figure 1 it is clear that the number of gained and loosed electrons is automatically balanced without interference of external source. Therefore, the electrical neutrality is automatically maintained here. Hence, in the form of reaction the above process is represented as,

Zn(s)+CuSO4(aq)→Cu(s)+ZnSO4(aq)

Hence, it is explained that the porous bridge is not needed in the voltaic cell.

Conclusion

An explanation for the porous bridge not being needed in the given cell has been rightfully stated

Want to see more full solutions like this?

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

Answer 5

Chapter 18, Problem 18.1VP

Interpretation Introduction

Interpretation: A voltaic cell is given. The greater density of a concentrated solution of CuSO4 is given to allow a less concentrated solution of ZnSO4 solution to be layered on top of it. An explanation for the porous bridge not being needed in the given cell is to be stated.

Concept introduction: Voltaic cell is a type of electrochemical cell which converts the chemical energy to electrical energy. This chemical energy generates by processing the redox reaction. Redox reaction is the combination of two half reactions. One half reactions is known as reduction half while other is oxidation half.

Salt bridge, also known as porous bridge is a U-shaped hollow device which is filled with KOH or other electrolytes. It is used to maintain the electrical neutrality during the process of redox reactions in two different compartments.

To determine: An explanation for the porous bridge not being needed in the given cell.

Expert Solution & Answer

Answer to Problem 18.1VP

Solution

An explanation for the porous bridge not being needed in the given cell has been rightfully stated.

Explanation of Solution

Explanation

In voltaic cell during the process of redox reaction electrons are generated on anode and then transfer to the cathode by the external circuit. In this way we can say that the process of oxidation occurs at the anode and the process of reduction occurs at cathode.

Oxidation is a process in which loss of electrons take place, while in reduction gain of electron take place.

The voltaic cell is given as,

Chemistry: The Science in Context (Fifth Edition), Chapter 18, Problem 18.1VP

Figure 1

From the above Figure 1 it is clear that two concentrated solutions, have different densities are present in a beaker. The concentrated solution which has the greater density allows the lass concentrated solution to be layered on its top. The Figure 1 shows that one electrode is attached with zinc metal. The other electrode is attached with copper metal. Therefore, the process of oxidation occurs at zinc. Hence, electrons move from zinc metal to copper. After the loss of electrons the zinc metal converts to zinc ion. After the gain of electrons the copper metal converts to copper ion. From the above Figure 1 it is clear that the number of gained and loosed electrons is automatically balanced without interference of external source. Therefore, the electrical neutrality is automatically maintained here. Hence, in the form of reaction the above process is represented as,

Zn(s)+CuSO4(aq)→Cu(s)+ZnSO4(aq)

Hence, it is explained that the porous bridge is not needed in the voltaic cell.

Conclusion

An explanation for the porous bridge not being needed in the given cell has been rightfully stated

Answer 6

Chapter 18, Problem 18.1VP

Interpretation Introduction

Interpretation: A voltaic cell is given. The greater density of a concentrated solution of CuSO4 is given to allow a less concentrated solution of ZnSO4 solution to be layered on top of it. An explanation for the porous bridge not being needed in the given cell is to be stated.

Concept introduction: Voltaic cell is a type of electrochemical cell which converts the chemical energy to electrical energy. This chemical energy generates by processing the redox reaction. Redox reaction is the combination of two half reactions. One half reactions is known as reduction half while other is oxidation half.

Salt bridge, also known as porous bridge is a U-shaped hollow device which is filled with KOH or other electrolytes. It is used to maintain the electrical neutrality during the process of redox reactions in two different compartments.

To determine: An explanation for the porous bridge not being needed in the given cell.

Expert Solution & Answer

Answer to Problem 18.1VP

Solution

An explanation for the porous bridge not being needed in the given cell has been rightfully stated.

Explanation of Solution

Explanation

In voltaic cell during the process of redox reaction electrons are generated on anode and then transfer to the cathode by the external circuit. In this way we can say that the process of oxidation occurs at the anode and the process of reduction occurs at cathode.

Oxidation is a process in which loss of electrons take place, while in reduction gain of electron take place.

The voltaic cell is given as,

Chemistry: The Science in Context (Fifth Edition), Chapter 18, Problem 18.1VP

Figure 1

From the above Figure 1 it is clear that two concentrated solutions, have different densities are present in a beaker. The concentrated solution which has the greater density allows the lass concentrated solution to be layered on its top. The Figure 1 shows that one electrode is attached with zinc metal. The other electrode is attached with copper metal. Therefore, the process of oxidation occurs at zinc. Hence, electrons move from zinc metal to copper. After the loss of electrons the zinc metal converts to zinc ion. After the gain of electrons the copper metal converts to copper ion. From the above Figure 1 it is clear that the number of gained and loosed electrons is automatically balanced without interference of external source. Therefore, the electrical neutrality is automatically maintained here. Hence, in the form of reaction the above process is represented as,

Zn(s)+CuSO4(aq)→Cu(s)+ZnSO4(aq)

Hence, it is explained that the porous bridge is not needed in the voltaic cell.

Conclusion

An explanation for the porous bridge not being needed in the given cell has been rightfully stated

Answer 7

Chapter 18, Problem 18.1VP

Interpretation Introduction

Interpretation: A voltaic cell is given. The greater density of a concentrated solution of CuSO4 is given to allow a less concentrated solution of ZnSO4 solution to be layered on top of it. An explanation for the porous bridge not being needed in the given cell is to be stated.

Concept introduction: Voltaic cell is a type of electrochemical cell which converts the chemical energy to electrical energy. This chemical energy generates by processing the redox reaction. Redox reaction is the combination of two half reactions. One half reactions is known as reduction half while other is oxidation half.

Salt bridge, also known as porous bridge is a U-shaped hollow device which is filled with KOH or other electrolytes. It is used to maintain the electrical neutrality during the process of redox reactions in two different compartments.

To determine: An explanation for the porous bridge not being needed in the given cell.

Answer 8

Expert Solution & Answer

Answer to Problem 18.1VP

Solution

An explanation for the porous bridge not being needed in the given cell has been rightfully stated.

Answer 9

Expert Solution & Answer

Answer 10

Expert Solution & Answer

Answer 11

Explanation of Solution

Explanation

In voltaic cell during the process of redox reaction electrons are generated on anode and then transfer to the cathode by the external circuit. In this way we can say that the process of oxidation occurs at the anode and the process of reduction occurs at cathode.

Oxidation is a process in which loss of electrons take place, while in reduction gain of electron take place.

The voltaic cell is given as,

Chemistry: The Science in Context (Fifth Edition), Chapter 18, Problem 18.1VP

Figure 1

From the above Figure 1 it is clear that two concentrated solutions, have different densities are present in a beaker. The concentrated solution which has the greater density allows the lass concentrated solution to be layered on its top. The Figure 1 shows that one electrode is attached with zinc metal. The other electrode is attached with copper metal. Therefore, the process of oxidation occurs at zinc. Hence, electrons move from zinc metal to copper. After the loss of electrons the zinc metal converts to zinc ion. After the gain of electrons the copper metal converts to copper ion. From the above Figure 1 it is clear that the number of gained and loosed electrons is automatically balanced without interference of external source. Therefore, the electrical neutrality is automatically maintained here. Hence, in the form of reaction the above process is represented as,

Zn(s)+CuSO4(aq)→Cu(s)+ZnSO4(aq)