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

Want to see the full answer?

Answer 1

Question

Chapter 21, Problem 128SCQ

(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

Students have asked these similar questions

Protecting Groups and Carbonyls 6) The synthesis generates allethrolone that exhibits high insect toxicity but low mammalian toxicity. They are used in pet shampoo, human lice shampoo, and industrial sprays for insects and mosquitos. Propose detailed mechanistic steps to generate the allethrolone label the different types of reagents (Grignard, acid/base protonation, acid/base deprotonation, reduction, oxidation, witting, aldol condensation, Robinson annulation, etc.) III + VI HS HS H+ CH,CH,Li III I II IV CI + P(Ph)3 V ༼ Hint: no strong base added VI S VII IX HO VIII -MgBr HgCl2,HgO HO. isomerization aqeuous solution H,SO, ༽༽༤༽༽ X MeOH Hint: enhances selectivity for reaction at the S X ☑

Draw the complete mechanism for the acid-catalyzed hydration of this alkene. esc 田 Explanation Check 1 888 Q A slock Add/Remove step Q F4 F5 F6 A བྲA F7 $ % 5 @ 4 2 3 & 6 87 Click and drag to start drawing a structure. © 2025 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Ce W E R T Y U S D LL G H IK DD 요 F8 F9 F10 F1 * ( 8 9 0 O P J K L Z X C V B N M H He command

Explanation Check F1 H₂O H₂ Pd 1) MCPBA 2) H3O+ 1) Hg(OAc)2, H₂O 2) NaBH4 OH CI OH OH OH hydration halohydrin formation addition halogenation hydrogenation inhalation hydrogenation hydration ☐ halohydrin formation addition halogenation formation chelation hydrogenation halohydrin formation substitution hydration halogenation addition Ohalohydrin formation subtraction halogenation addition hydrogenation hydration F2 80 F3 σ F4 F5 F6 1 ! 2 # 3 $ 4 % 05 Q W & Å © 2025 McGraw Hill LLC. All Rights Reserved. F7 F8 ( 6 7 8 9 LU E R T Y U A F9

Answer 2

Question

Chapter 21, Problem 128SCQ

(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 3

Question

Chapter 21, Problem 128SCQ

(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 4

Question

Chapter 21, Problem 128SCQ

(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 128SCQ

(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 128SCQ

(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 128SCQ

(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

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 15

Ch. 21.2 - Prob. 21.1CYU Ch. 21.2 - Write the formula for each of the following (a)...Ch. 21.2 - Prob. 21.3CYU Ch. 21.2 - Prob. 21.4CYU Ch. 21.11 - Prob. 1.1ACP Ch. 21.11 - Prob. 1.2ACP Ch. 21.11 - Prob. 1.3ACP Ch. 21.11 - Draw the Lewis structure of ammonia borane. What...Ch. 21.11 - Calculate the mass of hydrogen in 1.00 kg of...Ch. 21.11 - What is the hydrogen density (mass H2 per liter)...

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

Want to see the full answer?

Chapter 21 Solutions