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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2. Predict the NMR spectra for each of these two compounds by listing, in the NMR tables below, the chemical shift, the splitting, and the number of hydrogens associated with each predicted peak. Sort the peaks from largest chemical shift to lowest. **Not all slots must be filled** Peak Chemical Shift (d) 5.7 1 Multiplicity multiplate .......... 5.04 double of doublet 2 4.98 double of doublet 3 4.05 doublet of quartet 4 5 LO 3.80 quartet 1.3 doublet 6 Peak Chemical Shift (d) Multiplicity

Interpreting NMR spectra is a skill that often requires some amount of practice, which, in turn, necessitates access to a collection of NMR spectra. Beyond Labz Organic Synthesis and Organic Qualitative Analysis have spectral libraries containing over 700 1H NMR spectra. In this assignment, you will take advantage of this by first predicting the NMR spectra for two closely related compounds and then checking your predictions by looking up the actual spectra in the spectra library. After completing this assignment, you may wish to select other compounds for additional practice. 1. Write the IUPAC names for the following two structures: Question 2 Question 3 2. Predict the NMR spectra for each of these two compounds by listing, in the NMR tables below, the chemical shift, the splitting, and the number of hydrogens associated with each predicted peak. Sort the peaks from largest chemical shift to lowest. **Not all slots must be filled**

11:14 ... worksheets.beyondlabz.com 3. To check your predictions, click this link for Interpreting NMR Spectra 1. You will see a list of all the - compounds in the spectra library in alphabetical order by IUPAC name. Hovering over a name in the list will show the structure on the chalkboard. The four buttons on the top of the Spectra tab in the tray are used to select the different spectroscopic techniques for the selected compound. Make sure the NMR button has been selected. 4. Scroll through the list of names to find the names for the two compounds you have been given and click on the name to display the NMR spectrum for each. In the NMR tables below, list the chemical shift, the splitting, and the number of hydrogens associated with each peak for each compound. Compare your answers to your predictions. **Not all slots must be filled** Peak Chemical Shift (d) Multiplicity 1 2 3 4 5

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