Metal ion should be identified after the electrolysis of a metal nitrate solution M(NO 3 ) 2 ( a q ) for 325 min with a constant current of 20 .2 A gives 111 g of the metal. Concept introduction: During the electrolysis, the amount of substance that is produced at an electrode of cell depends on the amount of charge passed through it. The current can be calculated as follows: Charge ( C ) = C u r r e n t ( A ) × T i m e ( s )

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Answer 1

Question

Chapter 19, Problem 19.142SP

Interpretation Introduction

Interpretation:

Metal ion should be identified after the electrolysis of a metal nitrate solution M(NO3)2(aq) for 325min with a constant current of 20.2 A gives 111 g of the metal.

Concept introduction:

During the electrolysis, the amount of substance that is produced at an electrode of cell depends on the amount of charge passed through it. The current can be calculated as follows:

Charge(C)= Current(A)×Time(s)

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Answer 2

Question

Chapter 19, Problem 19.142SP

Interpretation Introduction

Interpretation:

Metal ion should be identified after the electrolysis of a metal nitrate solution M(NO3)2(aq) for 325min with a constant current of 20.2 A gives 111 g of the metal.

Concept introduction:

During the electrolysis, the amount of substance that is produced at an electrode of cell depends on the amount of charge passed through it. The current can be calculated as follows:

Charge(C)= Current(A)×Time(s)

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Answer 3

Question

Chapter 19, Problem 19.142SP

Interpretation Introduction

Interpretation:

Metal ion should be identified after the electrolysis of a metal nitrate solution M(NO3)2(aq) for 325min with a constant current of 20.2 A gives 111 g of the metal.

Concept introduction:

During the electrolysis, the amount of substance that is produced at an electrode of cell depends on the amount of charge passed through it. The current can be calculated as follows:

Charge(C)= Current(A)×Time(s)

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Answer 4

Question

Chapter 19, Problem 19.142SP

Interpretation Introduction

Interpretation:

Metal ion should be identified after the electrolysis of a metal nitrate solution M(NO3)2(aq) for 325min with a constant current of 20.2 A gives 111 g of the metal.

Concept introduction:

During the electrolysis, the amount of substance that is produced at an electrode of cell depends on the amount of charge passed through it. The current can be calculated as follows:

Charge(C)= Current(A)×Time(s)

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Answer 5

Chapter 19, Problem 19.142SP

Interpretation Introduction

Interpretation:

Metal ion should be identified after the electrolysis of a metal nitrate solution M(NO3)2(aq) for 325min with a constant current of 20.2 A gives 111 g of the metal.

Concept introduction:

During the electrolysis, the amount of substance that is produced at an electrode of cell depends on the amount of charge passed through it. The current can be calculated as follows:

Charge(C)= Current(A)×Time(s)

Answer 6

Chapter 19, Problem 19.142SP

Interpretation Introduction

Interpretation:

Metal ion should be identified after the electrolysis of a metal nitrate solution M(NO3)2(aq) for 325min with a constant current of 20.2 A gives 111 g of the metal.

Concept introduction:

During the electrolysis, the amount of substance that is produced at an electrode of cell depends on the amount of charge passed through it. The current can be calculated as follows:

Charge(C)= Current(A)×Time(s)

Answer 7

Chapter 19, Problem 19.142SP

Interpretation Introduction

Interpretation:

Metal ion should be identified after the electrolysis of a metal nitrate solution M(NO3)2(aq) for 325min with a constant current of 20.2 A gives 111 g of the metal.

Concept introduction:

During the electrolysis, the amount of substance that is produced at an electrode of cell depends on the amount of charge passed through it. The current can be calculated as follows:

Charge(C)= Current(A)×Time(s)

Answer 8

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Answer 9

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Answer 10

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Answer 11

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Solution Summary: The author explains that metal ion should be identified after the electrolysis of a metallic nitrate solution. Electrolysis gives two moles of electrons per one mole.

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