To estimate the mass of lime required to precipitate magneisum from sea water. Concept introduction: Magnesium is an alkaline earth metal and is prsent in sea water. The magnesium present in sea water can be extracted by precipitating it with either CaO or Ca ( OH ) 2 . The pure metal from the salt obtained can be obtained by the process of electrolysis . N u m b e r o f m o l e s = M a s s M o l e c u l a r m a s s Mass = Number of moles × Molecular mass

Question

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Answer 1

Question

Chapter 21, Problem 110SCQ

(a)

Interpretation Introduction

Interpretation:

To estimate the mass of lime required to precipitate magneisum from sea water.

Concept introduction:

Magnesium is an alkaline earth metal and is prsent in sea water. The magnesium present in sea water can be extracted by precipitating it with either CaO or Ca(OH)2. The pure metal from the salt obtained can be obtained by the process of electrolysis.

Number of moles = MassMolecular mass

Mass = Number of moles × Molecular mass

(b)

Interpretation Introduction

Interpretation:

To estimate the mass of product produced at anode and cathode on electrolysis of MgCl2 and also total number of Faradays of electricity used.

Concept introduction:

Magnesium is an alkaline earth metal and is prsent in sea water. The magnesium present in sea water can be extracted by precipitating it with either CaO or Ca(OH)2. The pure metal from the salt obtained can be obtained by the process of electrolysis.

The reduction happens at cathode

The oxidation happens at anode.

Number of moles = MassMolecular mass

Mass = Number of moles × Molecular mass

The total number of Faradays of electricity used is calculated by the number of electrons involved in the reaction

(c)

Interpretation Introduction

Interpretation:

To estimate how many Joules are required per mole for the given industrial process

Concept introduction:

Magnesium is an alkaline earth metal and is prsent in sea water. The magnesium present in sea water can be extracted by precipitating it with either CaO or Ca(OH)2. The pure metal from the salt obtained can be obtained by the process of electrolysis.

Number of moles = MassMolecular mass

Mass = Number of moles × Molecular mass

1kWh= 1 kilowatt hour = 3.6 × 106 J

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Answer 2

Question

Chapter 21, Problem 110SCQ

(a)

Interpretation Introduction

Interpretation:

To estimate the mass of lime required to precipitate magneisum from sea water.

Concept introduction:

Magnesium is an alkaline earth metal and is prsent in sea water. The magnesium present in sea water can be extracted by precipitating it with either CaO or Ca(OH)2. The pure metal from the salt obtained can be obtained by the process of electrolysis.

Number of moles = MassMolecular mass

Mass = Number of moles × Molecular mass

(b)

Interpretation Introduction

Interpretation:

To estimate the mass of product produced at anode and cathode on electrolysis of MgCl2 and also total number of Faradays of electricity used.

Concept introduction:

Magnesium is an alkaline earth metal and is prsent in sea water. The magnesium present in sea water can be extracted by precipitating it with either CaO or Ca(OH)2. The pure metal from the salt obtained can be obtained by the process of electrolysis.

The reduction happens at cathode

The oxidation happens at anode.

Number of moles = MassMolecular mass

Mass = Number of moles × Molecular mass

The total number of Faradays of electricity used is calculated by the number of electrons involved in the reaction

(c)

Interpretation Introduction

Interpretation:

To estimate how many Joules are required per mole for the given industrial process

Concept introduction:

Magnesium is an alkaline earth metal and is prsent in sea water. The magnesium present in sea water can be extracted by precipitating it with either CaO or Ca(OH)2. The pure metal from the salt obtained can be obtained by the process of electrolysis.

Number of moles = MassMolecular mass

Mass = Number of moles × Molecular mass

1kWh= 1 kilowatt hour = 3.6 × 106 J

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 21, Problem 110SCQ

(a)

Interpretation Introduction

Interpretation:

To estimate the mass of lime required to precipitate magneisum from sea water.

Concept introduction:

Magnesium is an alkaline earth metal and is prsent in sea water. The magnesium present in sea water can be extracted by precipitating it with either CaO or Ca(OH)2. The pure metal from the salt obtained can be obtained by the process of electrolysis.

Number of moles = MassMolecular mass

Mass = Number of moles × Molecular mass

(b)

Interpretation Introduction

Interpretation:

To estimate the mass of product produced at anode and cathode on electrolysis of MgCl2 and also total number of Faradays of electricity used.

Concept introduction:

Magnesium is an alkaline earth metal and is prsent in sea water. The magnesium present in sea water can be extracted by precipitating it with either CaO or Ca(OH)2. The pure metal from the salt obtained can be obtained by the process of electrolysis.

The reduction happens at cathode

The oxidation happens at anode.

Number of moles = MassMolecular mass

Mass = Number of moles × Molecular mass

The total number of Faradays of electricity used is calculated by the number of electrons involved in the reaction

(c)

Interpretation Introduction

Interpretation:

To estimate how many Joules are required per mole for the given industrial process

Concept introduction:

Magnesium is an alkaline earth metal and is prsent in sea water. The magnesium present in sea water can be extracted by precipitating it with either CaO or Ca(OH)2. The pure metal from the salt obtained can be obtained by the process of electrolysis.

Number of moles = MassMolecular mass

Mass = Number of moles × Molecular mass

1kWh= 1 kilowatt hour = 3.6 × 106 J

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 21, Problem 110SCQ

(a)

Interpretation Introduction

Interpretation:

To estimate the mass of lime required to precipitate magneisum from sea water.

Concept introduction:

Magnesium is an alkaline earth metal and is prsent in sea water. The magnesium present in sea water can be extracted by precipitating it with either CaO or Ca(OH)2. The pure metal from the salt obtained can be obtained by the process of electrolysis.

Number of moles = MassMolecular mass

Mass = Number of moles × Molecular mass

(b)

Interpretation Introduction

Interpretation:

To estimate the mass of product produced at anode and cathode on electrolysis of MgCl2 and also total number of Faradays of electricity used.

Concept introduction:

Magnesium is an alkaline earth metal and is prsent in sea water. The magnesium present in sea water can be extracted by precipitating it with either CaO or Ca(OH)2. The pure metal from the salt obtained can be obtained by the process of electrolysis.

The reduction happens at cathode

The oxidation happens at anode.

Number of moles = MassMolecular mass

Mass = Number of moles × Molecular mass

The total number of Faradays of electricity used is calculated by the number of electrons involved in the reaction

(c)

Interpretation Introduction

Interpretation:

To estimate how many Joules are required per mole for the given industrial process

Concept introduction:

Magnesium is an alkaline earth metal and is prsent in sea water. The magnesium present in sea water can be extracted by precipitating it with either CaO or Ca(OH)2. The pure metal from the salt obtained can be obtained by the process of electrolysis.

Number of moles = MassMolecular mass

Mass = Number of moles × Molecular mass

1kWh= 1 kilowatt hour = 3.6 × 106 J

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 5

Chapter 21, Problem 110SCQ

(a)

Interpretation Introduction

Interpretation:

To estimate the mass of lime required to precipitate magneisum from sea water.

Concept introduction:

Magnesium is an alkaline earth metal and is prsent in sea water. The magnesium present in sea water can be extracted by precipitating it with either CaO or Ca(OH)2. The pure metal from the salt obtained can be obtained by the process of electrolysis.

Number of moles = MassMolecular mass

Mass = Number of moles × Molecular mass

(b)

Interpretation Introduction

Interpretation:

To estimate the mass of product produced at anode and cathode on electrolysis of MgCl2 and also total number of Faradays of electricity used.

Concept introduction:

Magnesium is an alkaline earth metal and is prsent in sea water. The magnesium present in sea water can be extracted by precipitating it with either CaO or Ca(OH)2. The pure metal from the salt obtained can be obtained by the process of electrolysis.

The reduction happens at cathode

The oxidation happens at anode.

Number of moles = MassMolecular mass

Mass = Number of moles × Molecular mass

The total number of Faradays of electricity used is calculated by the number of electrons involved in the reaction

(c)

Interpretation Introduction

Interpretation:

To estimate how many Joules are required per mole for the given industrial process

Concept introduction:

Magnesium is an alkaline earth metal and is prsent in sea water. The magnesium present in sea water can be extracted by precipitating it with either CaO or Ca(OH)2. The pure metal from the salt obtained can be obtained by the process of electrolysis.

Number of moles = MassMolecular mass

Mass = Number of moles × Molecular mass

1kWh= 1 kilowatt hour = 3.6 × 106 J

Answer 6

Chapter 21, Problem 110SCQ

(a)

Interpretation Introduction

Interpretation:

To estimate the mass of lime required to precipitate magneisum from sea water.

Concept introduction:

Magnesium is an alkaline earth metal and is prsent in sea water. The magnesium present in sea water can be extracted by precipitating it with either CaO or Ca(OH)2. The pure metal from the salt obtained can be obtained by the process of electrolysis.

Number of moles = MassMolecular mass

Mass = Number of moles × Molecular mass

Answer 7

Chapter 21, Problem 110SCQ

(a)

Interpretation Introduction

Interpretation:

To estimate the mass of lime required to precipitate magneisum from sea water.

Concept introduction:

Magnesium is an alkaline earth metal and is prsent in sea water. The magnesium present in sea water can be extracted by precipitating it with either CaO or Ca(OH)2. The pure metal from the salt obtained can be obtained by the process of electrolysis.

Number of moles = MassMolecular mass

Mass = Number of moles × Molecular mass

Answer 8

(b)

Interpretation Introduction

Interpretation:

To estimate the mass of product produced at anode and cathode on electrolysis of MgCl2 and also total number of Faradays of electricity used.

Concept introduction:

Magnesium is an alkaline earth metal and is prsent in sea water. The magnesium present in sea water can be extracted by precipitating it with either CaO or Ca(OH)2. The pure metal from the salt obtained can be obtained by the process of electrolysis.

The reduction happens at cathode

The oxidation happens at anode.

Number of moles = MassMolecular mass

Mass = Number of moles × Molecular mass

The total number of Faradays of electricity used is calculated by the number of electrons involved in the reaction

Answer 9

(b)

Interpretation Introduction

Interpretation:

To estimate the mass of product produced at anode and cathode on electrolysis of MgCl2 and also total number of Faradays of electricity used.

Concept introduction:

Magnesium is an alkaline earth metal and is prsent in sea water. The magnesium present in sea water can be extracted by precipitating it with either CaO or Ca(OH)2. The pure metal from the salt obtained can be obtained by the process of electrolysis.

The reduction happens at cathode

The oxidation happens at anode.

Number of moles = MassMolecular mass

Mass = Number of moles × Molecular mass

The total number of Faradays of electricity used is calculated by the number of electrons involved in the reaction

Answer 10

(c)

Interpretation Introduction

Interpretation:

To estimate how many Joules are required per mole for the given industrial process

Concept introduction:

Magnesium is an alkaline earth metal and is prsent in sea water. The magnesium present in sea water can be extracted by precipitating it with either CaO or Ca(OH)2. The pure metal from the salt obtained can be obtained by the process of electrolysis.

Number of moles = MassMolecular mass

Mass = Number of moles × Molecular mass

1kWh= 1 kilowatt hour = 3.6 × 106 J

Answer 11

(c)

Interpretation Introduction

Interpretation:

To estimate how many Joules are required per mole for the given industrial process

Concept introduction:

Magnesium is an alkaline earth metal and is prsent in sea water. The magnesium present in sea water can be extracted by precipitating it with either CaO or Ca(OH)2. The pure metal from the salt obtained can be obtained by the process of electrolysis.

Number of moles = MassMolecular mass

Mass = Number of moles × Molecular mass

1kWh= 1 kilowatt hour = 3.6 × 106 J

Answer 12

Expert Solution & Answer

Answer 13

Expert Solution & Answer

Answer 14

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Answer 15

Ch. 21.2 - Prob. 1CYU Ch. 21.2 - Write the formula for each of the following (a)...Ch. 21.2 - Prob. 3CYU Ch. 21.2 - Prob. 4CYU Ch. 21.4 - Prob. 3RC Ch. 21.5 - Prob. 1Q Ch. 21.5 - Prob. 2Q Ch. 21.8 - Prob. 1Q Ch. 21.8 - Prob. 2Q Ch. 21.8 - Prob. 3Q

Solution Summary: The author calculates the mass of lime that must be used to precipitate magneisum from sea water.

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Chapter 21 Solutions