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Chemistry The Central Science 11th Edition Brown LeMay Bursten Test Bank

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Chemistry The Central Science 11th Edition Brown LeMay Bursten Test Bank

ISBN-13: 978-0321585615

ISBN-10: 0321585615

 

 

Description

Chemistry The Central Science 11th Edition Brown LeMay Bursten Test Bank

ISBN-13: 978-0321585615

ISBN-10: 0321585615

 

 

 

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20.1 Multiple-Choice and Bimodal Questions

 

1) The gain of electrons by an element is called __________.

 

  1. A) reduction
  2. B) oxidation
  3. C) disproportionation
  4. D) fractionation
  5. E) sublimation

 

 

Answer:  A

Diff: 1

Page Ref: Sec. 20.1

 

 

2) __________ is reduced in the following reaction:

 

 

  1. A) Cr6+
  2. B)
  3. C)
  4. D)
  5. E)

 

 

Answer:  A

Diff: 1

Page Ref: Sec. 20.1

 

3) __________ is the oxidizing agent in the reaction below.

 

 

  1. A)
  2. B)
  3. C)
  4. D)
  5. E)

 

 

Answer:  A

Diff: 1

Page Ref: Sec. 20.1

 

 

4) Which substance is serving as the reducing agent in the following reaction?

 

 

  1. A) Ni
  2. B)
  3. C)
  4. D)
  5. E)

 

 

Answer:  A

Diff: 1

Page Ref: Sec. 20.1

 

5) Which substance is the reducing agent in the reaction below?

 

  1. A) Pb
  2. B)
  3. C)
  4. D)
  5. E)

 

 

Answer:  A

Diff: 1

Page Ref: Sec. 20.1

 

 

6) What is the oxidation number of chromium in  ion?

 

  1. A) +3
  2. B) +12
  3. C) +7
  4. D) +6
  5. E) +14

 

 

Answer:  D

Diff: 1

Page Ref: Sec. 20.1

 

 

7) What is the oxidation number of potassium in ?

 

  1. A) 0
  2. B) +1
  3. C) +2
  4. D) -1
  5. E) +3

 

 

Answer:  B

Diff: 1

Page Ref: Sec. 20.1

 

 

 

8) What is the oxidation number of manganese in the  ion?

 

  1. A) +1
  2. B) +2
  3. C) +5
  4. D) +4
  5. E) +7

 

 

Answer:  E

Diff: 1

Page Ref: Sec. 20.1

 

 

9) What is the oxidation number of manganese in ?

 

  1. A) +3
  2. B) +2
  3. C) +1
  4. D) +4
  5. E) +7

 

 

Answer:  D

Diff: 1

Page Ref: Sec. 20.1

 

 

10) __________ electrons appear in the following half-reaction when it is balanced.

 

 

  1. A) 6
  2. B) 2
  3. C) 4
  4. D) 1
  5. E) 3

 

 

Answer:  B

Diff: 2

Page Ref: Sec. 20.2

 

 

 

11) The balanced half-reaction in which chlorine gas is reduced to the aqueous chloride ion is a __________ process.

 

  1. A) one-electron
  2. B) two-electron
  3. C) four-electron
  4. D) three-electron
  5. E) six-electron

 

 

Answer:  B

Diff: 1

Page Ref: Sec. 20.2

 

 

12) The balanced half-reaction in which dichromate ion is reduced to chromium metal is a __________ process.

 

  1. A) two-electron
  2. B) six-electron
  3. C) three-electron
  4. D) four-electron
  5. E) twelve-electron

 

 

Answer:  E

Diff: 2

Page Ref: Sec. 20.2

 

 

13) The balanced half-reaction in which dichromate ion is reduced to chromium(III) ion is a __________ process.

 

  1. A) four-electron
  2. B) twelve-electron
  3. C) three-electron
  4. D) six-electron
  5. E) two-electron

 

 

Answer:  D

Diff: 1

Page Ref: Sec. 20.2

 

14) The balanced half-reaction in which sulfate ion is reduced to sulfite ion is a __________ process.

 

  1. A) four-electron
  2. B) one-electron
  3. C) two-electron
  4. D) three-electron
  5. E) six-electron

 

 

Answer:  C

Diff: 1

Page Ref: Sec. 20.2

 

 

15) The electrode at which oxidation occurs is called the __________.

 

  1. A) oxidizing agent
  2. B) cathode
  3. C) reducing agent
  4. D) anode
  5. E) voltaic cell

 

 

Answer:  D

Diff: 1

Page Ref: Sec. 20.3

 

 

16) The half-reaction occurring at the anode in the balanced reaction shown below is __________.

 

 

  1. A)
  2. B)
  3. C)
  4. D)
  5. E)

 

 

Answer:  C

Diff: 1

Page Ref: Sec. 20.3

 

 

17) In a voltaic cell, electrons flow from the __________ to the __________.

 

  1. A) salt bride, anode
  2. B) anode, salt bridge
  3. C) cathode, anode
  4. D) salt bridge, cathode
  5. E) anode, cathode

 

 

Answer:  E

Diff: 1

Page Ref: Sec. 20.3

 

 

18) The reduction half reaction occurring in the standard hydrogen electrode is __________.

 

  1. A)
  2. B)
  3. C)
  4. D)
  5. E)

 

 

Answer:  D

Diff: 1

Page Ref: Sec. 20.4

 

 

19) 1V = __________.

 

  1. A) 1 amp ∙ s
  2. B) 1 J/s
  3. C) 96485 C
  4. D) 1 J/C
  5. E) 1 C/J

 

 

Answer:  D

Diff: 1

Page Ref: Sec. 20.4

 

 

20) The more __________ the value of , the greater the driving force for reduction.

 

  1. A) positive
  2. B) negative
  3. C) exothermic
  4. D) endothermic
  5. E) extensive

 

 

Answer:  A

Diff: 1

Page Ref: Sec. 20.4

 

 

Table 20.2

 

21) The standard cell potential  for the voltaic cell based on the reaction below is __________ V.

 

  1. A) +0.46
  2. B) +0.617
  3. C) +1.39
  4. D) -0.46
  5. E) +1.21

 

 

Answer:  B

Diff: 1

Page Ref: Sec. 20.4

 

22) The standard cell potential  for the voltaic cell based on the reaction below is __________ V.

 

 

  1. A) -1.45
  2. B) +2.99
  3. C) +1.51
  4. D) +3.05
  5. E) +1.57

 

 

Answer:  C

Diff: 1

Page Ref: Sec. 20.4

 

 

23) The standard cell potential  for the voltaic cell based on the reaction below is __________ V.

 

 

 

  1. A) +0.30
  2. B) +2.80
  3. C) +3.10
  4. D) +0.83
  5. E) -0.16

 

 

Answer:  A

Diff: 1

Page Ref: Sec. 20.4

 

24) The standard cell potential  for the voltaic cell based on the reaction below is __________ V.

 

 

  1. A) +1.94
  2. B) +0.89
  3. C) +2.53
  4. D) -0.59
  5. E) -1.02

 

 

Answer:  B

Diff: 1

Page Ref: Sec. 20.4

 

 

25) The relationship between the change in Gibbs free energy and the emf of an electrochemical cell is given by __________.

 

  1. A)
  2. B)
  3. C) ΔG = -nFE
  4. D) ΔG = -nRTF
  5. E)

 

 

Answer:  C

Diff: 1

Page Ref: Sec. 20.5

 

26) The standard cell potential  of the reaction below is +0.126 V. The value of  for the reaction is __________ kJ/mol.

 

 

  1. A) -24.3
  2. B) +24.3
  3. C) -12.6
  4. D) +12.6
  5. E) -50.8

 

 

Answer:  A

Diff: 1

Page Ref: Sec. 20.5

 

 

27) The standard cell potential  for the reaction below is +0.63 V. The cell potential for this reaction is __________ V when and

 

 

  1. A) 0.52
  2. B) 0.85
  3. C) 0.41
  4. D) 0.74
  5. E) 0.63

 

 

Answer:  A

Diff: 1

Page Ref: Sec. 20.6

 

28) The standard cell potential  for the reaction below is +1.10 V. The cell potential for this reaction is __________ V when the concentration of  and

 

 

  1. A) 1.40
  2. B) 1.25
  3. C) 0.95
  4. D) 0.80
  5. E) 1.10

 

 

Answer:  C

Diff: 2

Page Ref: Sec. 20.6

 

 

29) The lead-containing reactant(s) consumed during recharging of a lead-acid battery is/are __________.

 

  1. A) Pb (s) only
  2. B) only
  3. C) only
  4. D) both and
  5. E) both Pb (s) and

 

 

Answer:  C

Diff: 1

Page Ref: Sec. 20.7

 

30) Galvanized iron is iron coated with __________.

 

  1. A) magnesium.
  2. B) zinc.
  3. C) chromium.
  4. D) phosphate.
  5. E) iron oxide.

 

 

Answer:  B

Diff: 1

Page Ref: Sec. 20.8

 

 

31) Corrosion of iron is retarded by __________.

 

  1. A) the presence of salts
  2. B) high pH conditions
  3. C) low pH conditions
  4. D) both the presence of salts and high pH conditions
  5. E) both the presence of salts and low pH conditions

 

 

Answer:  B

Diff: 1

Page Ref: Sec. 20.8

 

 

32) How many minutes will it take to plate out 2.19 g of chromium metal from a solution of  using a current of 35.2 amps in an electrolyte cell?

 

  1. A) 5.77
  2. B) 346
  3. C) 115
  4. D) 1.92
  5. E) 17.3

 

 

Answer:  A

Diff: 2

Page Ref: Sec. 20.9

 

33) What current (in A) is required to plate out 1.22 g of nickel from a solution of  in 1.0 hour?

 

  1. A) 65.4
  2. B)
  3. C) 1.11
  4. D) 12.9
  5. E) 2.34

 

 

Answer:  C

Diff: 2

Page Ref: Sec. 20.9

 

 

34) How many grams of Ca metal are produced by the electrolysis of molten  using a current of 30.0 amp for 10.0 hours?

 

  1. A) 22.4
  2. B) 448
  3. C) 0.0622
  4. D) 224
  5. E) 112

 

 

Answer:  D

Diff: 2

Page Ref: Sec. 20.9

 

 

35) How many grams of Cu are obtained by passing a current of 12 A through a solution of  for 15 minutes?

 

  1. A) 0.016
  2. B) 3.6
  3. C) 7.1
  4. D) 14
  5. E) 1.8

 

 

Answer:  B

Diff: 2

Page Ref: Sec. 20.9

 

36) How many seconds are required to produce 1.0 g of silver metal by the electrolysis of a  solution using a current of 30 amps?

 

  1. A)
  2. B)
  3. C)
  4. D)
  5. E) 60

 

 

Answer:  C

Diff: 2

Page Ref: Sec. 20.9

 

 

37) How many grams of copper will be plated out by a current of 2.3 A applied for 25 minutes to a 0.50 M solution of copper(II) sulfate?

 

  1. A)
  2. B) 2.2
  3. C) 1.1
  4. D) 0.036
  5. E) 0.019

 

 

Answer:  C

Diff: 2

Page Ref: Sec. 20.9

 

 

20.2 Multiple-Choice

 

1) What is the oxidation number of bromine in the  ion?

 

  1. A) -1
  2. B) +1
  3. C) +3
  4. D) +5
  5. E) +7

 

 

Answer:  D

Diff: 1

Page Ref: Sec. 20.1

 

 

2) What is the oxidation number of nitrogen in the ?

 

  1. A) -1
  2. B) +1
  3. C) +3
  4. D) +5
  5. E) +7

 

 

Answer:  D

Diff: 1

Page Ref: Sec. 20.1

 

 

3) What is the oxidation number of sulfur in the  ion?

 

  1. A) -2
  2. B) +1
  3. C) +2
  4. D) +4
  5. E) +6

 

 

Answer:  E

Diff: 1

Page Ref: Sec. 20.1

 

 

4) Which element is oxidized in the reaction below?

 

 

  1. A) Fe
  2. B) C
  3. C) O
  4. D) H
  5. E) I

 

 

Answer:  A

Diff: 1

Page Ref: Sec. 20.1

 

5) Which element is reduced in the reaction below?

 

 

  1. A) Fe
  2. B) C
  3. C) O
  4. D) H
  5. E) I

 

 

Answer:  D

Diff: 1

Page Ref: Sec. 20.1

 

 

6) Which element is oxidized in the reaction below?

 

 

  1. A) Fe
  2. B) Cr
  3. C) O
  4. D) H

 

 

Answer:  A

Diff: 1

Page Ref: Sec. 20.1

 

 

7) Which element is reduced in the reaction below?

 

 

  1. A) Fe
  2. B) Cr
  3. C) O
  4. D) H

 

 

Answer:  B

Diff: 1

Page Ref: Sec. 20.1

 

 

8) Which element is oxidized in the reaction below?

 

 

  1. A) I
  2. B) Mn
  3. C) O
  4. D) H

 

 

Answer:  A

Diff: 1

Page Ref: Sec. 20.1

 

 

9) Which element is reduced in the reaction below?

 

 

  1. A) I
  2. B) Mn
  3. C) O
  4. D) H

 

 

Answer:  B

Diff: 1

Page Ref: Sec. 20.1

 

10) Which of the following reactions is a redox reaction?

 

(a)

(b)

(c)

 

  1. A) (a) only
  2. B) (b) only
  3. C) (c) only
  4. D) (a) and (c)
  5. E) (b) and (c)

 

 

Answer:  C

Diff: 1

Page Ref: Sec. 20.1

 

 

11) Which one of the following reactions is a redox reaction?

 

  1. A)
  2. B)
  3. C)
  4. D) None of the above is a redox reaction.

 

 

Answer:  D

Diff: 2

Page Ref: Sec. 20.1

 

 

 

12) Which substance is the reducing agent in the following reaction?

 

 

  1. A)
  2. B)
  3. C)
  4. D)
  5. E)

 

 

Answer:  D

Diff: 1

Page Ref: Sec. 20.1

 

 

13) What is the coefficient of the permanganate ion when the following equation is balanced?

 

(acidic solution)

 

  1. A) 1
  2. B) 2
  3. C) 3
  4. D) 5
  5. E) 4

 

 

Answer:  B

Diff: 2

Page Ref: Sec. 20.2

 

14) What is the coefficient of the dichromate ion when the following equation is balanced?

 

(acidic solution)

 

  1. A) 1
  2. B) 2
  3. C) 3
  4. D) 5
  5. E) 6

 

 

Answer:  A

Diff: 2

Page Ref: Sec. 20.2

 

 

15) What is the coefficient of  when the following equation is balanced?

(basic solution)

 

  1. A) 1
  2. B) 2
  3. C) 3
  4. D) 4
  5. E) 5

 

 

Answer:  B

Diff: 2

Page Ref: Sec. 20.2

 

 

16) Which transformation could take place at the anode of an electrochemical cell?

 

  1. A)
  2. B)
  3. C)
  4. D)
  5. E) None of the above could take place at the anode.

 

 

Answer:  E

Diff: 1

Page Ref: Sec. 20.3

 

 

17) The purpose of the salt bridge in an electrochemical cell is to __________.

 

  1. A) maintain electrical neutrality in the half-cells via migration of ions.
  2. B) provide a source of ions to react at the anode and cathode.
  3. C) provide oxygen to facilitate oxidation at the anode.
  4. D) provide a means for electrons to travel from the anode to the cathode.
  5. E) provide a means for electrons to travel from the cathode to the anode.

 

 

Answer:  A

Diff: 1

Page Ref: Sec. 20.3

 

 

18) Which transformation could take place at the anode of an electrochemical cell?

 

  1. A)
  2. B)
  3. C)
  4. D)
  5. E)

 

 

Answer:  A

Diff: 1

Page Ref: Sec. 20.3

 

 

19) Which transformation could take place at the cathode of an electrochemical cell?

 

  1. A)
  2. B)
  3. C)
  4. D)
  5. E)

 

 

Answer:  D

Diff: 1

Page Ref: Sec. 20.3

 

 

Table 20.1

 

 

20) Which of the halogens in Table 20.1 is the strongest oxidizing agent?

 

  1. A)
  2. B)
  3. C)
  4. D)
  5. E) All of the halogens have equal strength as oxidizing agents.

 

 

Answer:  C

Diff: 1

Page Ref: Sec. 20.4

 

 

21) Which one of the following types of elements is most likely to be a good oxidizing agent?

 

  1. A) alkali metals
  2. B) lanthanides
  3. C) alkaline earth elements
  4. D) transition elements
  5. E) halogens

 

 

Answer:  E

Diff: 1

Page Ref: Sec. 20.4

 

 

22) Which one of the following is the best oxidizing agent?

 

  1. A)
  2. B) Na
  3. C)
  4. D) Li
  5. E) Ca

 

 

Answer:  C

Diff: 1

Page Ref: Sec. 20.4

 

 

Table 20.2

 

23) Which of the following reactions will occur spontaneously as written?

 

  1. A)
  2. B) ss
  3. C)
  4. D)
  5. E)

 

 

Answer:  D

Diff: 2

Page Ref: Sec. 20.5

 

24) Which of the following reactions will occur spontaneously as written?

 

  1. A)
  2. B)
  3. C)
  4. D)
  5. E)

 

 

Answer:  E

Diff: 1

Page Ref: Sec. 20.5

 

 

25) Consider an electrochemical cell based on the reaction:

 

 

Which of the following actions would change the measured cell potential?

 

 

  1. A) increasing the in the cathode compartment
  2. B) lowering the in the cathode compartment
  3. C) increasing the [] in the anode compartment
  4. D) increasing the pressure of hydrogen gas in the cathode compartment
  5. E) Any of the above will change the measure cell potential.

 

 

Answer:  E

Diff: 1

Page Ref: Sec. 20.6

 

26) Consider an electrochemical cell based on the reaction:

 

 

Which of the following actions would not change the measured cell potential?

 

  1. A) lowering the pH in the cathode compartment
  2. B) addition of more tin metal to the anode compartment
  3. C) increasing the tin (II) ion concentration in the anode compartment
  4. D) increasing the pressure of hydrogen gas in the cathode compartment
  5. F) Any of the above will change the measured cell potential.

 

 

Answer:  B

Diff: 1

Page Ref: Sec. 20.6

 

 

27) What is the anode in an alkaline battery?

 

  1. A)
  2. B) KOH
  3. C) Zn powder
  4. D)
  5. E) Pt

 

 

Answer:  C

Diff: 1

Page Ref: Sec. 20.7

 

 

28) What is the cathode in an alkaline battery?

  1. A)
  2. B) KOH
  3. C) Zn powder
  4. D)
  5. E) Pt

 

 

Answer:  A

Diff: 1

Page Ref: Sec. 20.7

 

 

 

29) What is the cathode in the hydrogen fuel cell?

 

  1. A)
  2. B) KOH
  3. C) Li
  4. D)
  5. E) Pt

 

 

Answer:  A

Diff: 1

Page Ref: Sec. 20.7

 

 

30) In a lead-acid battery, the electrodes are consumed. In this battery,

 

  1. A) the anode is Pb
  2. B) the anode is .
  3. C) the anode is .
  4. D) the cathode is .
  5. E) the cathode is. Pb

 

 

Answer:  A

Diff: 1

Page Ref: Sec. 20.7

 

 

31) Cathodic protection of a metal pipe against corrosion usually entails

 

  1. A) attaching an active metal to make the pipe the anode in an electrochemical cell.
  2. B) coating the pipe with another metal whose standard reduction potential is less negative than that of the pipe.
  3. C) attaching an active metal to make the pipe the cathode in an electrochemical cell.
  4. D) attaching a dry cell to reduce any metal ions which might be formed.
  5. E) coating the pipe with a fluoropolymer to act as a source of fluoride ion (since the latter is so hard to oxidize).

 

 

Answer:  C

Diff: 2

Page Ref: Sec. 20.8

 

32) One of the differences between a voltaic cell and an electrolytic cell is that in an electrolytic cell __________.

 

  1. A) an electric current is produced by a chemical reaction
  2. B) electrons flow toward the anode
  3. C) a nonspontaneous reaction is forced to occur
  4. D)gas is produced at the cathode
  5. E) oxidation occurs at the cathode

 

 

Answer:  C

Diff: 1

Page Ref: Sec. 20.9

 

 

33) How many minutes will it take to plate out 4.56 g of Ni metal from a solution of Ni+2 using a current of 45.5 amps in an electrolytic cell?

 

  1. A) 2.75
  2. B) 5.49
  3. C) 4.55
  4. D) 155
  5. E) 330

 

 

Answer:  B

Diff: 2

Page Ref: Sec. 20.9

 

 

34) How many minutes will it take to plate out 16.22 g of Al metal from a solution of Al+3 using a current of 12.9 amps in an electrolytic cell?

 

  1. A) 60.1
  2. B) 74.9
  3. C) 173
  4. D) 225
  5. E) 13480

 

 

Answer:  D

Diff: 2

Page Ref: Sec. 20.9

 

 

 

20.3 Short Answer

 

1) The most difficult species to reduce and the poorest oxidizing agent is __________.

 

 

Answer:  lithium ion ;

Diff: 1

Page Ref: Sec. 20.5

 

 

2) At constant temperature and pressure the Gibbs free energy value is a measure of the __________ of a process.

 

 

Answer:  spontaneity

Diff: 1

Page Ref: Sec. 20.5

 

 

3) In the formula ΔG = -nFE , F is the __________.

 

 

Answer:  Faraday constant or the charge on one mole of electrons

Diff: 1

Page Ref: Sec. 20.5

 

 

4) The dependence of cell emf on concentration is expressed in the __________ equation.

 

 

Answer:  Nernst

Diff: 1

Page Ref: Sec. 20.6

 

 

5) The potential (E) to move  from the extracellular fluid to the intracellular fluid  necessitates work. The sign for this potential is __________.

 

 

Answer:  negative

Diff: 1

Page Ref: Sec. 20.6

 

6) The anode of the alkaline battery is powdered zinc in a gel that contacts __________.

 

 

Answer:  KOH; potassium hydroxide

Diff: 1

Page Ref: Sec. 20.7

 

 

7) The major product of a hydrogen fuel cell is __________.

 

 

Answer:  water

Diff: 1

Page Ref: Sec. 20.7

 

 

8) When iron is coated with a thin layer of zinc to protect against corrosion, the iron is said to be __________.

 

 

Answer:  galvanized

Diff: 1

Page Ref: Sec. 20.7

 

 

9) The quantity of charge passing a point in a circuit in one second when the current is one ampere is called a __________.

 

 

Answer:  coulomb

Diff: 1

Page Ref: Sec. 20.9

 

 

10) Calculate the number of grams of aluminum produced in 30.0 minutes by electrolysis of  at a current of 12.0 A.

 

 

Answer:  2.01 g

Diff: 1

Page Ref: Sec. 20.9

 

20.4 True/False Questions

 

1) The electrode where reduction occurs is called the anode.

Answer:  False

 

Diff: 1

Page Ref: Sec. 20.3

 

 

2) In a voltaic cell electrons flow from the anode to the cathode.

Answer:  True

 

Diff: 1

Page Ref: Sec. 20.3

 

 

3) When the cell potential is negative in a voltaic cell the cell reaction will not proceed spontaneously.

Answer:  True

 

Diff: 1

Page Ref: Sec. 20.4

 

 

4) The standard reduction potential, E°red, is proportional to the stoichiometric coefficient.

Answer:  False

 

Diff: 1

Page Ref: Sec. 20.4

 

 

5) The standard reduction potential of X is 1.23 V and that of Y is -0.44 V therefore X is oxidized by Y.

Answer:  False

 

Diff: 1

Page Ref: Sec. 20.4

 

 

6) The lithium ion battery has more energy per unit mass than nickel-cadmium batteries.

Answer:  True

 

Diff: 1

Page Ref: Sec. 20.7

 

 

7) Disadvantages of the methanol fuel cell compared to the hydrogen fuel cell are consumption of catalyst and the production of a less environmentally safe product.

Answer:  True

 

Diff: 1

Page Ref: Sec. 20.7

 

 

8) In a half reaction the amount of a substance that is reduced or oxidized is directly proportional to the number of electrons generated in the cell.

Answer:  True

 

Diff: 1

Page Ref: Sec. 20.9

 

 

9) A positive number for maximum useful work in a spontaneous process (voltaic cell)  indicates that the cell will perform work on its surroundings.

Answer:  False

 

Diff: 1

Page Ref: Sec. 20.9

 

 

20.5 Algorithmic Questions

 

1) The standard cell potential (E°) of a voltaic cell constructed using the cell reaction below is 0.76 V:

 

 

With  = 1.0 atm and [] = 1.0 M, the cell potential is  0.66 V. The concentration of  in the cathode compartment is __________ M.

 

  1. A)
  2. B)
  3. C)
  4. D)
  5. E)

 

 

Answer:  A

Diff: 3

Page Ref: Sec. 20.6

 

 

2) A voltaic cell is constructed with two silver-silver chloride electrodes, where the half-reaction is

 

E° = +0.222 V

 

The concentrations of chloride ion in the two compartments are  0.0222 M and  2.22 M, respectively. The cell emf is __________ V.

 

  1. A) 0.212
  2. B) 0.118
  3. C) 0.00222
  4. D) 22.2
  5. E) 0.232

 

 

Answer:  B

Diff: 1

Page Ref: Sec. 20.6

 

 

3) A voltaic cell is constructed with two  electrodes, where the half-reaction is

 

E° = -0.763 V

 

The concentrations of zinc ion in the two compartments are  5.50 M and   M, respectively. The cell emf is __________ V.

 

  1. A)
  2. B) -378
  3. C) 0.0798
  4. D) 0.160
  5. E) -0.761

 

 

Answer:  C

Diff: 1

Page Ref: Sec. 20.6

 

 

 

4) The standard emf for the cell using the overall cell reaction below is +2.20 V:

 

 

The emf generated by the cell when [] =  M and [] = 0.15 M is

 

  1. A) 2.20
  2. B) 2.32
  3. C) 2.10
  4. D) 2.39
  5. E) 2.23

 

 

Answer:  B

Diff: 2

Page Ref: Sec. 20.6

 

 

5) The standard emf for the cell using the overall cell reaction below is +0.48 V:

 

 

The emf generated by the cell when [] = 2.50 M and [] = 0.100 M is

 

  1. A) 0.40
  2. B) 0.50
  3. C) 0.52
  4. D) 0.56
  5. E) 0.44

 

 

Answer:  C

Diff: 2

Page Ref: Sec. 20.6

 

 

 

6) How many kilowatt-hours of electricity are used to produce 3.00 kg of magnesium in the electrolysis of molten  with an applied emf of 4.50 V?

 

  1. A) 0.0336
  2. B) 0.0298
  3. C) 7.4
  4. D) 29.8
  5. E) 14.9

 

 

Answer:  D

Diff: 2

Page Ref: Sec. 20.9

 

 

7) The most useful ore of aluminum is bauxite, in which Al is present as hydrated oxides,  The number of kilowatt-hours of electricity required to produce  of aluminum from electrolysis of compounds from bauxite is __________ when the applied emf is 5.00V

 

  1. A) 0.0168
  2. B) 0.0596
  3. C) 39.7
  4. D) 19.9
  5. E) 59.6

 

 

Answer:  E

Diff: 2

Page Ref: Sec. 20.9

 

 

 

8) The town of Natrium, West Virginia, derives its name from the sodium produced in the electrolysis of molten sodium chloride (NaCl) mined from ancient salt deposits. The number of kilowatt-hours of electricity required to produce 4.60 kg of metallic sodium from the electrolysis of molten NaCl(s) is __________ when the applied emf is 4.50 V.

 

  1. A) 24.1
  2. B) 0.0414
  3. C) 0.0241
  4. D) 48.3
  5. E) 12.1

 

 

Answer:  A

Diff: 3

Page Ref: Sec. 20.9

 

 

9) The electrolysis of molten  for 3.25 hr with an electrical current of 15.0 A produces __________ g of aluminum metal.

 

  1. A) 147
  2. B) 0.606
  3. C)
  4. D) 16.4
  5. E) 49.1

 

 

Answer:  D

Diff: 1

Page Ref: Sec. 20.9

 

 

10) How many seconds are required to produce 4.00 g of aluminum metal from the electrolysis of molten  with an electrical current of 12.0 A?

 

  1. A) 27.0
  2. B) 9.00
  3. C)
  4. D)
  5. E)

 

 

Answer:  E

Diff: 2

Page Ref: Sec. 20.9