Question 1

In the electrolyte of an electrochemical cell, current is carried by electrons moving from the anode to the cathode.

Accepted Answer

A) True 
 B)False

Question 2

What product forms at the cathode during the electrolysis of molten lithium iodide?

Accepted Answer

A)   Li+(l) 
B)   Li(l) 
C)   I-(l) 
D)   I2(g) 
E)   I3-(l) F) None of the above
G) B) and D)

Question 3

Select the incorrect statement relating to the corrosion of iron in air.

Accepted Answer

A)   Fe2+ is formed in the anodic region.
B)   O2 is oxidized in the cathodic region.
C)   Electrons travel through the iron metal between the anodic and cathodic regions.
D)   Moisture provides a pathway for ions to migrate.
E)   Rust is a hydrated form of iron(III)  oxide.F) C) and D)
G) A) and B)

Question 4

In the electrolyte of an electrochemical cell, current is carried by anions moving toward the anode and cations moving in the opposite direction.

Accepted Answer

A) True 
 B)False

Question 5

Which one of the following statements relating to the glass electrode is correct?

Accepted Answer

A)   The glass electrode detects hydrogen gas.
B)   The glass of a glass electrode serves to conduct electrons.
C)   When pH is measured, only a single electrode, the glass electrode, need be used.
D)   The potential of the glass electrode varies linearly with the pH of the solution.
E)   None of these choices are correct.F) All of the above
G) A) and C) D

Question 6

In the electrolysis of aqueous potassium nitrate using inert electrodes, which one of the following species is oxidized?

Accepted Answer

A)   potassium ion
B)   nitrate ion
C)   water
D)   oxygen
E)   hydronium ionF) None of the above
G) B) and E)

Question 7

The line notation, Pt | H2(g)  | H+(aq)  || Cu2+(aq)  | Cu(s) , indicates that

Accepted Answer

A)   copper metal is a product of the cell reaction.
B)   hydrogen gas (H2)  is a product of the cell reaction.
C)   Cu is the anode.
D)   Pt is the cathode.
E)   Cu2+ is the reducing agent.F) A) and B)
G) A) and C)

Question 8

Consider the nonaqueous cell reaction 2Na(l)  + FeCl2(s)  2(s)    2NaCl(s)  + Fe(s)  For which E° cell = 2.35 V at 200°C. ΔG° at this temperature is A)  453 kJ. B)  -453 kJ. C)  907 kJ. D)  -907 kJ. E)  None of these choices are correct." class="answers-bank-image d-inline" rel="preload" > 2NaCl(s)  + Fe(s) 
For which E° cell = 2.35 V at 200°C. ΔG° at this temperature is

Accepted Answer

A)   453 kJ.
B)   -453 kJ.
C)   907 kJ.
D)   -907 kJ.
E)   None of these choices are correct.F) All of the above
G) B) and C)

Question 9

The voltaic cell made up of cobalt, copper, and their M2+ ions, has E°cell = 0.62 V. If E° of the cathode half-cell is 0.34 V, what is E° of the anode half-cell? Cu2+(aq)  + Co(s)  → Cu(s)  + Co2+(aq)

Accepted Answer

A)   -0.28 V
B)   -0.96 V
C)   0.28 V
D)   0.96 V
E)   None of these choices are correct.F) B) and C)
G) None of the above

Question 10

When metal A is placed in a solution of metal ions B2+, a reaction occurs between A and B2+, and metal ions A2+ appear in the solution. When metal B is placed in acid solution, gas bubbles form on its surface. When metal A is placed in a solution of metal ions C2+, no reaction occurs. Which of the following reactions would not occur spontaneously?

Accepted Answer

A)   C(s)  + 2H+(aq)  → H2(g)  + C+(aq) 
B)   C(s)  + A2+(aq)  → A(s)  + C2+(aq) 
C)   B(s)  + C2+(aq)  → C(s)  + B2+(aq) 
D)   A(s)  + 2H+(aq)  → H2(g)  + A2+(aq) 
E)   B(s)  + 2H+(aq)  → H2(g)  + B2+(aq) F) A) and E)
G) B) and E)

Question 11

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the iodide ion will be I-(aq)  + NO3-(aq)  → NO(g)  + I2(s)  (acidic solution)

Accepted Answer

A)   2.
B)   3.
C)   6.
D)   8.
E)   None of these choices are correct.F) All of the above
G) A) and B)

Question 12

Consider the following balanced redox reaction Mn2+(aq)  + S2O82-(aq)  + 2H2O(l)  → MnO2(s)  + 4H(aq)  + 2SO42-(aq) 
Which of the following statements is true?

Accepted Answer

A)   Mn2+(aq)  is the oxidizing agent and is reduced.
B)   Mn2+(aq)  is the oxidizing agent and is oxidized.
C)   Mn2+(aq)  is the reducing agent and is oxidized.
D)   Mn2+(aq)  is the reducing agent and is reduced.
E)   Manganese does not change its oxidation number in this reaction.F) B) and D)
G) B) and E)

Question 13

What mass of copper will be deposited when 18.2 A are passed through a CuSO4 solution for 45.0 minutes?

Accepted Answer

A)   16.2 g
B)   33.4 g
C)   40.6 g
D)   81.3 g
E)   163 gF) None of the above
G) A) and C)

Question 14

Chromium metal is electroplated from acidic aqueous solutions containing the dichromate ion, Cr2O72-. What is the minimum time needed to plate out 10.0 g of chromium metal from such a solution, if the current is 50.0 A?

Accepted Answer

A)   6.2 minutes
B)   12.4 minutes
C)   18.6 minutes
D)   24.7 minutes
E)   37.1 minutesF) D) and E)
G) A) and C) C

Question 15

A salt bridge provides a path for electrons to move between the anode and cathode compartments of a voltaic cell.

Accepted Answer

A) True 
 B)False

Question 16

The line notation, Al(s)  | Al3+(aq)  || Co2+(aq)  | Co(s) , indicates that

Accepted Answer

A)   Co is the reducing agent.
B)   Co2+ ions are oxidized.
C)   Al is the reducing agent.
D)   Al3+ is the reducing agent.
E)   aluminum metal is the cathode.F) A) and B)
G) A) and C)

Question 17

Which, if any, of the following metals would be capable of acting as a sacrificial anode when used with iron pipe? E°Fe = -0.44 V; all E° values refer to the M2+/M half-cell reactions.

Accepted Answer

A)   copper, Cu, E° = 0.15 V
B)   cobalt, Co, E° = -0.28 V
C)   chromium, Cr, E° = -0.74 V
D)   tin, Sn, E° = -0.14 V
E)   None of these metals would be capable of acting as a sacrificial anode with iron.F) C) and D)
G) A) and E)

Question 18

The redox reaction of peroxydisulfate with iodide has been used for many years as part of the iodine clock reaction which introduces students to kinetics. If E°cell = 1.587 V and E° of the cathode half-cell is 0.536 V, what is E° of the anode half-cell? S2O82-(aq)  + 2H+ + 2I-(aq)  → 2HSO4-(aq)  + I2(aq)

Accepted Answer

A)   -1.051 V
B)   -2.123 V
C)   1.051 V
D)   2.123 V
E)   None of these choices are correct.F) None of the above
G) A) and E)

Question 19

What is the E°cell for the cell represented by the combination of the following half-reactions? ClO4(aq)  + 8H(aq)  + 8e cell for the cell represented by the combination of the following half-reactions? ClO4(aq)  + 8H(aq)  + 8e   Cl-(aq)  + 4H2O(l)  E° = 1.389 V VO2(aq)  + 2H(aq)  + e- j   VO(aq)  + H2O(l)  E° = 0.991 V A)  -0.398 V B)  -2.380 V C)  0.398 V D)  2.380 V E)  None of these choices are correct." class="answers-bank-image d-inline" rel="preload" > Cl-(aq)  + 4H2O(l)  E° = 1.389 V
VO2(aq)  + 2H(aq)  + e- j cell for the cell represented by the combination of the following half-reactions? ClO4(aq)  + 8H(aq)  + 8e   Cl-(aq)  + 4H2O(l)  E° = 1.389 V VO2(aq)  + 2H(aq)  + e- j   VO(aq)  + H2O(l)  E° = 0.991 V A)  -0.398 V B)  -2.380 V C)  0.398 V D)  2.380 V E)  None of these choices are correct." class="answers-bank-image d-inline" rel="preload" > VO(aq)  + H2O(l)  E° = 0.991 V

Accepted Answer

A)   -0.398 V
B)   -2.380 V
C)   0.398 V
D)   2.380 V
E)   None of these choices are correct.F) C) and D)
G) All of the above

Question 20

What mass of silver will be formed when 15.0 A are passed through molten AgCl for 25.0 minutes?

Accepted Answer

A)   0.419 g
B)   6.29 g
C)   12.6 g
D)   25.2 g
E)   33.4 gF) B) and C)
G) A) and B) D

Exam 21: Electrochemistry Chemical Change and Electrical Work

In the electrolyte of an electrochemical cell, current is carried by electrons moving from the anode to the cathode.

Correct Answer
verified

What product forms at the cathode during the electrolysis of molten lithium iodide?

Correct Answer
verified

Select the incorrect statement relating to the corrosion of iron in air.

Correct Answer
verified

In the electrolyte of an electrochemical cell, current is carried by anions moving toward the anode and cations moving in the opposite direction.

Correct Answer
verified

Which one of the following statements relating to the glass electrode is correct?

Correct Answer
verified
D

In the electrolysis of aqueous potassium nitrate using inert electrodes, which one of the following species is oxidized?

Correct Answer
verified

The line notation, Pt | H₂(g) | H⁺(aq) || Cu²⁺(aq) | Cu(s) , indicates that

Correct Answer
verified

Consider the nonaqueous cell reaction 2Na(l) + FeCl₂(s) 2NaCl(s) + Fe(s) For which E°_cell = 2.35 V at 200°C. ΔG° at this temperature is

Correct Answer
verified

The voltaic cell made up of cobalt, copper, and their M²⁺ ions, has E°_cell = 0.62 V. If E° of the cathode half-cell is 0.34 V, what is E° of the anode half-cell? Cu²⁺(aq) + Co(s) → Cu(s) + Co²⁺(aq)

Correct Answer
verified

Correct Answer
verified

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the iodide ion will be I-(aq) + NO₃-(aq) → NO(g) + I₂(s) (acidic solution)

Correct Answer
verified

Consider the following balanced redox reaction Mn²+(aq) + S₂O8^2-(aq) + 2H₂O(l) → MnO₂(s) + 4H(aq) + 2SO₄^2-(aq) Which of the following statements is true?

Correct Answer
verified

What mass of copper will be deposited when 18.2 A are passed through a CuSO₄ solution for 45.0 minutes?

Correct Answer
verified

Chromium metal is electroplated from acidic aqueous solutions containing the dichromate ion, Cr₂O7^2-. What is the minimum time needed to plate out 10.0 g of chromium metal from such a solution, if the current is 50.0 A?

Correct Answer
verified
C

A salt bridge provides a path for electrons to move between the anode and cathode compartments of a voltaic cell.

Correct Answer
verified

The line notation, Al(s) | Al³⁺(aq) || Co²⁺(aq) | Co(s) , indicates that

Correct Answer
verified

Which, if any, of the following metals would be capable of acting as a sacrificial anode when used with iron pipe? E°_Fe = -0.44 V; all E° values refer to the M²⁺/M half-cell reactions.

Correct Answer
verified

Correct Answer
verified

What is the E°_cell for the cell represented by the combination of the following half-reactions? ClO₄(aq) + 8H(aq) + 8e Cl-(aq) + 4H₂O(l) E° = 1.389 V VO₂(aq) + 2H(aq) + e^- j VO(aq) + H₂O(l) E° = 0.991 V

Correct Answer
verified

What mass of silver will be formed when 15.0 A are passed through molten AgCl for 25.0 minutes?

Correct Answer
verified
D

Exam 21: Electrochemistry Chemical Change and Electrical Work

In the electrolyte of an electrochemical cell, current is carried by electrons moving from the anode to the cathode.

Correct AnswerverifiedShow Answer

What product forms at the cathode during the electrolysis of molten lithium iodide?

Correct AnswerverifiedShow Answer

Select the incorrect statement relating to the corrosion of iron in air.

Correct AnswerverifiedShow Answer

In the electrolyte of an electrochemical cell, current is carried by anions moving toward the anode and cations moving in the opposite direction.

Correct AnswerverifiedShow Answer

Which one of the following statements relating to the glass electrode is correct?

Correct AnswerverifiedD

In the electrolysis of aqueous potassium nitrate using inert electrodes, which one of the following species is oxidized?

Correct AnswerverifiedShow Answer

The line notation, Pt | H2(g) | H+(aq) || Cu2+(aq) | Cu(s) , indicates that

Correct AnswerverifiedShow Answer

Consider the nonaqueous cell reaction 2Na(l) + FeCl2(s) 2NaCl(s) + Fe(s) For which E° cell = 2.35 V at 200°C. ΔG° at this temperature is

Correct AnswerverifiedShow Answer

The voltaic cell made up of cobalt, copper, and their M2+ ions, has E°cell = 0.62 V. If E° of the cathode half-cell is 0.34 V, what is E° of the anode half-cell? Cu2+(aq) + Co(s) → Cu(s) + Co2+(aq)

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the iodide ion will be I-(aq) + NO3-(aq) → NO(g) + I2(s) (acidic solution)

Correct AnswerverifiedShow Answer

Consider the following balanced redox reaction Mn2+(aq) + S2O82-(aq) + 2H2O(l) → MnO2(s) + 4H(aq) + 2SO42-(aq) Which of the following statements is true?

Correct AnswerverifiedShow Answer

What mass of copper will be deposited when 18.2 A are passed through a CuSO4 solution for 45.0 minutes?

Correct AnswerverifiedShow Answer

Chromium metal is electroplated from acidic aqueous solutions containing the dichromate ion, Cr2O72-. What is the minimum time needed to plate out 10.0 g of chromium metal from such a solution, if the current is 50.0 A?

Correct AnswerverifiedC

A salt bridge provides a path for electrons to move between the anode and cathode compartments of a voltaic cell.

Correct AnswerverifiedShow Answer

The line notation, Al(s) | Al3+(aq) || Co2+(aq) | Co(s) , indicates that

Correct AnswerverifiedShow Answer

Which, if any, of the following metals would be capable of acting as a sacrificial anode when used with iron pipe? E°Fe = -0.44 V; all E° values refer to the M2+/M half-cell reactions.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

What is the E°cell for the cell represented by the combination of the following half-reactions? ClO4(aq) + 8H(aq) + 8e Cl-(aq) + 4H2O(l) E° = 1.389 V VO2(aq) + 2H(aq) + e- j VO(aq) + H2O(l) E° = 0.991 V

Correct AnswerverifiedShow Answer

What mass of silver will be formed when 15.0 A are passed through molten AgCl for 25.0 minutes?

Correct AnswerverifiedD

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified
D

Correct Answer
verified

The line notation, Pt | H₂(g) | H⁺(aq) || Cu²⁺(aq) | Cu(s) , indicates that

Correct Answer
verified

Consider the nonaqueous cell reaction 2Na(l) + FeCl₂(s) 2NaCl(s) + Fe(s) For which E°_cell = 2.35 V at 200°C. ΔG° at this temperature is

Correct Answer
verified

The voltaic cell made up of cobalt, copper, and their M²⁺ ions, has E°_cell = 0.62 V. If E° of the cathode half-cell is 0.34 V, what is E° of the anode half-cell? Cu²⁺(aq) + Co(s) → Cu(s) + Co²⁺(aq)

Correct Answer
verified

Correct Answer
verified

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the iodide ion will be I-(aq) + NO₃-(aq) → NO(g) + I₂(s) (acidic solution)

Correct Answer
verified

Consider the following balanced redox reaction Mn²+(aq) + S₂O8^2-(aq) + 2H₂O(l) → MnO₂(s) + 4H(aq) + 2SO₄^2-(aq) Which of the following statements is true?

Correct Answer
verified

What mass of copper will be deposited when 18.2 A are passed through a CuSO₄ solution for 45.0 minutes?

Correct Answer
verified

Chromium metal is electroplated from acidic aqueous solutions containing the dichromate ion, Cr₂O7^2-. What is the minimum time needed to plate out 10.0 g of chromium metal from such a solution, if the current is 50.0 A?

Correct Answer
verified
C

Correct Answer
verified

The line notation, Al(s) | Al³⁺(aq) || Co²⁺(aq) | Co(s) , indicates that

Correct Answer
verified

Which, if any, of the following metals would be capable of acting as a sacrificial anode when used with iron pipe? E°_Fe = -0.44 V; all E° values refer to the M²⁺/M half-cell reactions.

Correct Answer
verified

Correct Answer
verified

What is the E°_cell for the cell represented by the combination of the following half-reactions? ClO₄(aq) + 8H(aq) + 8e Cl-(aq) + 4H₂O(l) E° = 1.389 V VO₂(aq) + 2H(aq) + e^- j VO(aq) + H₂O(l) E° = 0.991 V

Correct Answer
verified

Correct Answer
verified
D