Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
2nd Edition
ISBN: 9781305079243
Author: Steven S. Zumdahl, Susan A. Zumdahl
Publisher: Cengage Learning
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Textbook Question
Chapter 17, Problem 95E

What mass of each of the following substances can be produced in 1.0 h with a current of 15 A?

a. Co from aqueous Co2+

b. Hf from aqueous Hf4+

c. I2 from aqueous KI

d. Cr from molten CrO3

(a)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The mass of each of the following substances produced in one hour with a current of 15 A is to be calculated.

Concept introduction: The mass of molten salt and ionic solution is calculated by the process of electrolysis in which an electric current is passed through a molten salt or either an ionic solution. In the process of electrolysis the ions are forced to undergo redox reactions or either an oxidation or reduction reaction.

To determine: The mass of Co from aqueous Co2 in one hour with a current of 15 A .

Answer to Problem 95E

  1. a. The mass of Co from aqueous Co2 is 16.4 g_ .

Explanation of Solution

Explanation

The mass of Co from aqueous Co2 is 16.4 g_ .

Given

Current (C) is 15 A .

The conversion of A to C/s is done as,

1A=1 C/s

Therefore, the conversion of 15A to C/s is done as,

15 A=15 C/s

Time (t) is 1.0 hr .

The conversion of hr to sec is done as,

1hr=60min=3600 sec

Therefore, the conversion of 1 hr to sec is done as,

1 hr=3600 sec

The atomic weight of Cobalt is 58.93 g/mol .

The equivalent weight of Cobalt is calculated by using the formula,

Equivalent weight of Cobalt = Atomic weight of CobaltNumber ofvalence electrons

Substitute the value of atomic weight of Cobalt and number of valence electrons in the above expression.

Equivalent weight of Cobalt = Atomic weight of CobaltNumber ofvalence electrons=58.93 g/mol2e=29.465 g/mol e

Hence, the electro chemical equivalent (Z) of Cobalt is calculated by using formula,

Z=Equivalent weightF

Where,

  • F is the faradays constant (96,485 C/mol e) .

Substitute the values of equivalent weight and F in the above expression,

Z=Equivalent weightF=29.465 g/mol e96,485 C/mol e=3.0×104 g/C

Now, the mass is calculated by using the formula,

W=Z.C.t

Where,

  • Z is the electro chemical equivalent.
  • C is the current.
  • t is the time.

Substitute the values of Z, C and t in the above expression,

W=Z.C.t=3.0×10-4 g/C×15 C/s ×3600 s=16.4 g_

Therefore, the mass of Co from aqueous Co2 is 16.4 g_ .

(b)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The mass of each of the following substances produced in one hour with a current of 15 A is to be calculated.

Concept introduction: The mass of molten salt and ionic solution is calculated by the process of electrolysis in which an electric current is passed through a molten salt or either an ionic solution. In the process of electrolysis the ions are forced to undergo redox reactions or either an oxidation or reduction reaction.

To determine: The mass of Hf from aqueous Hf4+ in one hour with a current of 15 A .

Answer to Problem 95E

  1. b. The mass of Hf from aqueous Hf4+ is 25.0 g_ .

Explanation of Solution

Explanation

The mass of Hf from aqueous Hf4+ is 25.0 g_ .

The atomic weight of Hf is 178.49 g/mol .

The equivalent weight of Hf is calculated by using the formula,

Equivalent weight of Hf = Atomic weight of HfNumber ofvalence electrons

Substitute the value of atomic weight of Hf and number of valence electrons in the above expression.

Equivalent weight of Hf = Atomic weight of HfNumber ofvalence electrons=178.49 g/mol4e=44.62 g/mol e

Hence, the electro chemical equivalent (Z) of Hf is calculated by using formula,

Z=Equivalent weightF

Where,

  • F is the faradays constant (96,485 C/mol e) .

Substitute the values of equivalent weight and F in the above expression,

Z=Equivalent weightF=44.62g/mol e96,485 C/mol e=4.6×104 g/C

Now, the mass is calculated by using the formula,

W=Z.C.t

Where,

  • Z is the electro chemical equivalent.
  • C is the current.
  • t is the time.

Substitute the values of Z, C and t in the above expression,

W=Z.C.t=4.6×10-4 g/C×15 C/s ×3600 s=24.97g_25.0 g_

The mass of Hf from aqueous Hf4+ is 25.0 g_ .

(c)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The mass of each of the following substances produced in one hour with a current of 15 A is to be calculated.

Concept introduction: The mass of molten salt and ionic solution is calculated by the process of electrolysis in which an electric current is passed through a molten salt or either an ionic solution. In the process of electrolysis the ions are forced to undergo redox reactions or either an oxidation or reduction reaction.

To determine: The mass of I2 from aqueous KI in one hour with a current of 15 A .

Answer to Problem 95E

  1. c. The mass of I2 from aqueous KI is 71.0 g_ .

Explanation of Solution

Explanation

The mass of I2 from aqueous KI is 71.0 g_ .

The atomic weight of Iodine is 126.90 g/mol

The equivalent weight of Iodine is calculated by using the formula,

Equivalent weight of Iodine = Atomic weight of IodineNumber ofvalence electrons

Substitute the value of atomic weight of Iodine and number of valence electrons in the above expression.

Equivalent weight of Iodine = Atomic weight of IodineNumber ofvalence electrons=126.90 g/mol1e=126.90 g/mol e

Hence, the electro chemical equivalent (Z) of Iodine is calculated by using formula,

Z=Equivalent weightF

Where,

  • F is the faradays constant (96,485 C/mol e) .

Substitute the values of equivalent weight and F in the above expression,

Z=Equivalent weightF=126.90 g/mol e96,485 C/mol e=13.1×104 g/C

Now, the mass is calculated by using the formula,

W=Z.C.t

Where,

  • Z is the electro chemical equivalent.
  • C is the current.
  • t is the time.

Substitute the values of Z, C and t in the above expression,

W=Z.C.t=13.1×10-4 g/C×15 C/s ×3600 s=71.0g_

The mass of I2 from aqueous KI is 71.0 g_ .

(d)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The mass of each of the following substances produced in one hour with a current of 15 A is to be calculated.

Concept introduction: The mass of molten salt and ionic solution is calculated by the process of electrolysis in which an electric current is passed through a molten salt or either an ionic solution. In the process of electrolysis the ions are forced to undergo redox reactions or either an oxidation or reduction reaction.

To determine: The mass of Cr from molten CrO3 in one hour with a current of 15 A .

Answer to Problem 95E

  1. d. The mass of Cr from molten CrO3 is 4.84 g_ .

Explanation of Solution

Explanation

The mass of Cr from molten CrO3 is 4.84 g_ .

The atomic weight of Cr is 51.996 g/mol

The equivalent weight of Cr is calculated by using the formula,

Equivalent weight of Cr = Atomic weight of CrNumber ofvalence electrons

Substitute the value of atomic weight of Cr and number of valence electrons in the above expression.

Equivalent weight of Cr = Atomic weight of CrNumber ofvalence electrons=51.996 g/mol6e=8.666 g/mol e

Hence, the electro chemical equivalent (Z) of Iodine is calculated by using formula,

Z=Equivalent weightF

Where,

  • F is the faradays constant (96,485 C/mol e) .

Substitute the values of equivalent weight and F in the above expression,

Z=Equivalent weightF=8.666 g/mol e96,485 C/mol e=8.9817×105 g/C

Now, the mass is calculated by using the formula,

W=Z.C.t

Where,

  • Z is the electro chemical equivalent.
  • C is the current.
  • t is the time.

Substitute the values of Z, C and t in the above expression,

W=Z.C.t=8.9817×10-5 g/C×15 C/s ×3600 s=4.85g_

The mass of Cr from molten CrO3 is 4.84 g_ .

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Chapter 17 Solutions

Chemistry: An Atoms First Approach

Ch. 17 - Prob. 2ALQCh. 17 - Prob. 3ALQCh. 17 - Prob. 4ALQCh. 17 - Sketch a cell that forms iron metal from iron(II)...Ch. 17 - Which of the following is the best reducing agent:...Ch. 17 - Prob. 7ALQCh. 17 - Prob. 8ALQCh. 17 - Explain why cell potentials are not multiplied by...Ch. 17 - What is the difference between and ? When is equal...Ch. 17 - Prob. 11ALQCh. 17 - Look up the reduction potential for Fe3+ to Fe2+....Ch. 17 - Prob. 13ALQCh. 17 - Is the following statement true or false?...Ch. 17 - Prob. 15RORRCh. 17 - Assign oxidation numbers to all the atoms in each...Ch. 17 - Specify which of the following equations represent...Ch. 17 - The Ostwald process for the commercial production...Ch. 17 - Prob. 19QCh. 17 - Prob. 20QCh. 17 - When magnesium metal is added to a beaker of...Ch. 17 - How can one construct a galvanic cell from two...Ch. 17 - The free energy change for a reaction, G, is an...Ch. 17 - What is wrong with the following statement: The...Ch. 17 - When jump-starting a car with a dead battery, the...Ch. 17 - Prob. 26QCh. 17 - Prob. 27QCh. 17 - Consider the following electrochemical cell: a. If...Ch. 17 - Balance the following oxidationreduction reactions...Ch. 17 - Prob. 30ECh. 17 - Prob. 31ECh. 17 - Prob. 32ECh. 17 - Chlorine gas was first prepared in 1774 by C. W....Ch. 17 - Gold metal will not dissolve in either...Ch. 17 - Prob. 35ECh. 17 - Consider the following galvanic cell: a. 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It took 74.1 s...Ch. 17 - Electrolysis of an alkaline earth metal chloride...Ch. 17 - What volume of F2 gas, at 25C and 1.00 atm, is...Ch. 17 - What volumes of H2(g) and O2(g) at STP are...Ch. 17 - Prob. 101ECh. 17 - A factory wants to produce 1.00 103 kg barium...Ch. 17 - It took 2.30 min using a current of 2.00 A to...Ch. 17 - A solution containing Pt4+ is electrolyzed with a...Ch. 17 - A solution at 25C contains 1.0 M Cd2+, 1.0 M Ag+,...Ch. 17 - Consider the following half-reactions: A...Ch. 17 - In the electrolysis of an aqueous solution of...Ch. 17 - Copper can be plated onto a spoon by placing the...Ch. 17 - Prob. 109ECh. 17 - Prob. 110ECh. 17 - Prob. 111ECh. 17 - What reaction will take place at the Cathode and...Ch. 17 - Gold is produced electrochemically from an aqueous...Ch. 17 - Prob. 114AECh. 17 - The saturated calomel electrode. abbreviated SCE....Ch. 17 - Consider the following half-reactions: Explain why...Ch. 17 - Consider the standard galvanic cell based on the...Ch. 17 - Prob. 118AECh. 17 - The black silver sulfide discoloration of...Ch. 17 - Prob. 120AECh. 17 - When aluminum foil is placed in hydrochloric acid,...Ch. 17 - Prob. 122AECh. 17 - Prob. 123AECh. 17 - The overall reaction and equilibrium constant...Ch. 17 - What is the maximum work that can be obtained from...Ch. 17 - The overall reaction and standard cell potential...Ch. 17 - Prob. 127AECh. 17 - Prob. 128AECh. 17 - Prob. 129AECh. 17 - Prob. 130AECh. 17 - Prob. 131AECh. 17 - Prob. 132AECh. 17 - Prob. 133AECh. 17 - Prob. 134CWPCh. 17 - Consider a galvanic cell based on the following...Ch. 17 - Consider a galvanic cell based on the following...Ch. 17 - Consider a galvanic cell based on the following...Ch. 17 - An electrochemical cell consists of a silver metal...Ch. 17 - An aqueous solution of PdCl2 is electrolyzed for...Ch. 17 - Prob. 140CPCh. 17 - Prob. 141CPCh. 17 - The overall reaction in the lead storage battery...Ch. 17 - Consider the following galvanic cell: Calculate...Ch. 17 - Prob. 144CPCh. 17 - A galvanic cell is based on the following...Ch. 17 - Prob. 146CPCh. 17 - The measurement of pH using a glass electrode...Ch. 17 - Prob. 148CPCh. 17 - A galvanic cell is based on the following...Ch. 17 - Prob. 150CPCh. 17 - Prob. 151CPCh. 17 - Prob. 152CPCh. 17 - Consider the following galvanic cell: A 15 0-mole...Ch. 17 - When copper reacts with nitric acid, a mixture of...Ch. 17 - The following standard reduction potentials have...Ch. 17 - An electrochemical cell is set up using the...Ch. 17 - Three electrochemical cells were connected in...Ch. 17 - A silver concentration cell is set up at 25C as...Ch. 17 - A galvanic cell is based on the following...Ch. 17 - Prob. 160MP
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