Question 1

When the following redox equation is balanced with smallest whole number coefficients,the coefficient for the hydrogen sulfate ion will be ______.
Al(s) + HSO4-(aq) + OH-(aq)   →	o→  Al2O3(s) + S2-(aq) + H2O(l)

Accepted Answer

A)  1
B)  3
C)  4
D)  8
E)  None of these choices is correct. F) A) and E)
G) A) and C)

Question 2

Consider the reaction of iodine with manganese dioxide
3I2(s) + 2MnO2(s) + 8OH-(aq)  2(s) + 2MnO2(s) + 8OH-(aq)    6I-(aq) + 2MnO4-(aq) + 4H2O(l)  The equilibrium constant for the overall reaction is 8.30  	imes  10-7.Calculate  \Delta G° for the reaction at 25°C. A) -15.1 kJ B) -34.7 kJ C) 15.1 kJ D) 34.7 kJ E) None of these choices is correct. " class="answers-bank-image d-inline" rel="preload" >
6I-(aq) + 2MnO4-(aq) + 4H2O(l) 
The equilibrium constant for the overall reaction is 8.30  ×	imes×  10-7.Calculate  Δ\DeltaΔ G° for the reaction at 25°C.

Accepted Answer

A)  -15.1 kJ
B)  -34.7 kJ
C)  15.1 kJ
D)  34.7 kJ
E)  None of these choices is correct. F) A) and D)
G) C) and D)

Question 3

For the reaction occurring in a voltaic (galvanic)cell,$\Delta$G > 0.

Accepted Answer

A) True 
 B)False

Question 4

If the electrodes of a voltaic cell are connected with an external wire,electrons will flow in this wire from the cathode to the anode.

Accepted Answer

A) True 
 B)False

Question 5

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

Question 6

A current of 1000.A flows for exactly 1 hour,through a cell in which the following reaction occurs at one of the electrodes.
Mg2+ + 2e- $\to$ Mg
a.Calculate the charge,in coulombs,which passes through the circuit in this time.
b.Calculate the theoretical mass of Mg (magnesium metal)which is produced in this time.

Accepted Answer

a.3.60 x 1...

Question 7

Examine the following half-reactions and select the weakest oxidizing agent among the species listed.
AuBr4-(aq) + 3e- 4-(aq) + 3e-   Au(s) + 4Br-(aq) ;E° = 0.854 V Mn2+(aq) + 2e-   Mn(s) ;E° = -1.185 V K+(aq) + e-   K(s) ;E° = -2.931 V F2O(aq) + 2H+(aq) + 4e-   2F-(aq) + H2O(l) ;E° = 2.153 V A) AuBr4-(aq)  B) Mn2+(aq)  C) K+(aq)  D) F2O(aq)  E) H+(aq) " class="answers-bank-image d-inline" rel="preload" >
Au(s) + 4Br-(aq) ;E° = 0.854 V
Mn2+(aq) + 2e- 4-(aq) + 3e-   Au(s) + 4Br-(aq) ;E° = 0.854 V Mn2+(aq) + 2e-   Mn(s) ;E° = -1.185 V K+(aq) + e-   K(s) ;E° = -2.931 V F2O(aq) + 2H+(aq) + 4e-   2F-(aq) + H2O(l) ;E° = 2.153 V A) AuBr4-(aq)  B) Mn2+(aq)  C) K+(aq)  D) F2O(aq)  E) H+(aq) " class="answers-bank-image d-inline" rel="preload" >
Mn(s) ;E° = -1.185 V
K+(aq) + e- 4-(aq) + 3e-   Au(s) + 4Br-(aq) ;E° = 0.854 V Mn2+(aq) + 2e-   Mn(s) ;E° = -1.185 V K+(aq) + e-   K(s) ;E° = -2.931 V F2O(aq) + 2H+(aq) + 4e-   2F-(aq) + H2O(l) ;E° = 2.153 V A) AuBr4-(aq)  B) Mn2+(aq)  C) K+(aq)  D) F2O(aq)  E) H+(aq) " class="answers-bank-image d-inline" rel="preload" >
K(s) ;E° = -2.931 V
F2O(aq) + 2H+(aq) + 4e- 4-(aq) + 3e-   Au(s) + 4Br-(aq) ;E° = 0.854 V Mn2+(aq) + 2e-   Mn(s) ;E° = -1.185 V K+(aq) + e-   K(s) ;E° = -2.931 V F2O(aq) + 2H+(aq) + 4e-   2F-(aq) + H2O(l) ;E° = 2.153 V A) AuBr4-(aq)  B) Mn2+(aq)  C) K+(aq)  D) F2O(aq)  E) H+(aq) " class="answers-bank-image d-inline" rel="preload" >
2F-(aq) + H2O(l) ;E° = 2.153 V

Accepted Answer

A)  AuBr4-(aq) 
B)  Mn2+(aq) 
C)  K+(aq) 
D)  F2O(aq) 
E)  H+(aq) F) B) and D)
G) C) and E)

Question 8

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 statements is correct.F) B) and C)
G) C) and D)

Question 9

A primary battery is one which can be recharged.

Accepted Answer

A) True 
 B)False

Question 10

When the following redox equation is balanced with smallest whole number coefficients,the coefficient for nitrogen dioxide will be _____.
I2(s) + HNO3(aq)   →	o→  HIO3(aq) + NO2(g) + H2O(l)

Accepted Answer

A)  1
B)  2
C)  4
D)  10
E)  None of these choices is correct. F) B) and C)
G) A) and E)

Question 11

Consider the reaction of iodine with manganese dioxide
3I2(s) + 2MnO2(s) + 8OH-(aq)  2(s) + 2MnO2(s) + 8OH-(aq)    6I-(aq) + 2MnO4-(aq) + 4H2O(l)  The equilibrium constant for the overall reaction is 8.30  	imes  10-7.Calculate E°cell for the reaction at 25°C. A) -0.36 V B) -0.18 V C) -0.12 V D) -0.060 V E) None of these choices is correct. " class="answers-bank-image d-inline" rel="preload" >
6I-(aq) + 2MnO4-(aq) + 4H2O(l) 
The equilibrium constant for the overall reaction is 8.30  ×	imes×  10-7.Calculate E°cell for the reaction at 25°C.

Accepted Answer

A)  -0.36 V
B)  -0.18 V
C)  -0.12 V
D)  -0.060 V
E)  None of these choices is correct. F) D) and E)
G) A) and B)

Question 12

The Downs cell is used in the electrolysis of

Accepted Answer

A)  molten calcium chloride.
B)  aqueous calcium chloride.
C)  molten sodium chloride.
D)  aqueous sodium chloride.
E)  None of the above.F) A) and C)
G) C) and D)

Question 13

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-   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 is correct." class="answers-bank-image d-inline" rel="preload" >
Cl-(aq) + 4H2O(l) ;E° = 1.389 V
VO2+(aq) + 2H+(aq) + 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-   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 is 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 is correct.F) A) and C)
G) D) and E)

Question 14

How many grams of oxygen gas will be produced in the electrolysis of water,for every gram of hydrogen gas formed?
Reaction: 2H2O(l)   →	o→  2H2(g) + O2(g)

Accepted Answer

A)  31.7 g
B)  15.9 g
C)  7.94 g
D)  3.97 g
E)  1.98 g F) A) and B)
G) B) and E)

Question 15

Given that E° for X + e-  →	o→  Y is greater than E° for A + 2e-  →	o→  B,it is correct to say that,under standard conditions

Accepted Answer

A)  X will oxidize A.
B)  Y will oxidize A.
C)  Y will reduce A.
D)  B will oxidize X.
E)  B will reduce X. F) A) and B)
G) B) and E)

Question 16

A battery that cannot be recharged is a

Accepted Answer

A)  fuel cell.
B)  primary battery.
C)  secondary battery.
D)  simple battery.
E)  flow battery.F) A) and B)
G) B) and C)

Question 17

Examine the following half-reactions and select the strongest oxidizing agent among the species listed.
Cr2+(aq) + 2e- 2+(aq) + 2e-   Cr(s) ;E° = -0.913 V Fe2+(aq) + 2e-   Fe(s) ;E° = -0.447 V Sr2+(aq) + 2e-   Sr(s) ;E° = -2.89 V Co2+(aq) + 2e-   Co(s) ;E° = -0.28 V A) Cr2+(aq)  B) Fe(s)  C) Fe2+(aq)  D) Sr2+(aq)  E) Co2+(aq) " class="answers-bank-image d-inline" rel="preload" >
Cr(s) ;E° = -0.913 V
Fe2+(aq) + 2e- 2+(aq) + 2e-   Cr(s) ;E° = -0.913 V Fe2+(aq) + 2e-   Fe(s) ;E° = -0.447 V Sr2+(aq) + 2e-   Sr(s) ;E° = -2.89 V Co2+(aq) + 2e-   Co(s) ;E° = -0.28 V A) Cr2+(aq)  B) Fe(s)  C) Fe2+(aq)  D) Sr2+(aq)  E) Co2+(aq) " class="answers-bank-image d-inline" rel="preload" >
Fe(s) ;E° = -0.447 V
Sr2+(aq) + 2e- 2+(aq) + 2e-   Cr(s) ;E° = -0.913 V Fe2+(aq) + 2e-   Fe(s) ;E° = -0.447 V Sr2+(aq) + 2e-   Sr(s) ;E° = -2.89 V Co2+(aq) + 2e-   Co(s) ;E° = -0.28 V A) Cr2+(aq)  B) Fe(s)  C) Fe2+(aq)  D) Sr2+(aq)  E) Co2+(aq) " class="answers-bank-image d-inline" rel="preload" >
Sr(s) ;E° = -2.89 V
Co2+(aq) + 2e- 2+(aq) + 2e-   Cr(s) ;E° = -0.913 V Fe2+(aq) + 2e-   Fe(s) ;E° = -0.447 V Sr2+(aq) + 2e-   Sr(s) ;E° = -2.89 V Co2+(aq) + 2e-   Co(s) ;E° = -0.28 V A) Cr2+(aq)  B) Fe(s)  C) Fe2+(aq)  D) Sr2+(aq)  E) Co2+(aq) " class="answers-bank-image d-inline" rel="preload" >
Co(s) ;E° = -0.28 V

Accepted Answer

A)  Cr2+(aq) 
B)  Fe(s) 
C)  Fe2+(aq) 
D)  Sr2+(aq) 
E)  Co2+(aq) F) B) and D)
G) C) and D)

Exam 21: Electrochemistry: Chemical Change and Electrical Work

A primary battery is one which can be recharged.

Correct Answer
verified

When the following redox equation is balanced with smallest whole number coefficients,the coefficient for the hydrogen sulfate ion will be ______. Al(s) + HSO₄^-(aq) + OH^-(aq) $\to$ Al₂O₃(s) + S^2-(aq) + H₂O(l)

Correct Answer
verified

Examine the following half-reactions and select the strongest oxidizing agent among the species listed. Cr²⁺(aq) + 2e^- Cr(s) ;E° = -0.913 V Fe²⁺(aq) + 2e^- Fe(s) ;E° = -0.447 V Sr²⁺(aq) + 2e^- Sr(s) ;E° = -2.89 V Co²⁺(aq) + 2e^- Co(s) ;E° = -0.28 V

Correct Answer
verified

Examine the following half-reactions and select the weakest oxidizing agent among the species listed. AuBr₄^-(aq) + 3e^- Au(s) + 4Br^-(aq) ;E° = 0.854 V Mn²⁺(aq) + 2e^- Mn(s) ;E° = -1.185 V K⁺(aq) + e^- K(s) ;E° = -2.931 V F₂O(aq) + 2H⁺(aq) + 4e^- 2F^-(aq) + H₂O(l) ;E° = 2.153 V

Correct Answer
verified

Correct Answer
verified
a.3.60 x 1...
View Answer

If the electrodes of a voltaic cell are connected with an external wire,electrons will flow in this wire from the cathode to the anode.

Correct Answer
verified

Given that E° for X + e^- $\to$ Y is greater than E° for A + 2e^- $\to$ B,it is correct to say that,under standard conditions

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^- VO⁺(aq) + H₂O(l) ;E° = 0.991 V

Correct Answer
verified

Correct Answer
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Correct Answer
verified

A battery that cannot be recharged is a

Correct Answer
verified

When the following redox equation is balanced with smallest whole number coefficients,the coefficient for nitrogen dioxide will be _____. I₂(s) + HNO₃(aq) $\to$ HIO₃(aq) + NO₂(g) + H₂O(l)

Correct Answer
verified

How many grams of oxygen gas will be produced in the electrolysis of water,for every gram of hydrogen gas formed? Reaction: 2H₂O(l) $\to$ 2H₂(g) + O₂(g)

Correct Answer
verified

For the reaction occurring in a voltaic (galvanic)cell, $\Delta$ G > 0.

Correct Answer
verified

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

Correct Answer
verified

The Downs cell is used in the electrolysis of

Correct Answer
verified

Correct Answer
verified

Exam 21: Electrochemistry: Chemical Change and Electrical Work

A primary battery is one which can be recharged.

Correct AnswerverifiedShow Answer

When the following redox equation is balanced with smallest whole number coefficients,the coefficient for the hydrogen sulfate ion will be ______. Al(s) + HSO4-(aq) + OH-(aq) →\to→ Al2O3(s) + S2-(aq) + H2O(l)

Correct AnswerverifiedShow Answer

Examine the following half-reactions and select the strongest oxidizing agent among the species listed. Cr2+(aq) + 2e- Cr(s) ;E° = -0.913 V Fe2+(aq) + 2e- Fe(s) ;E° = -0.447 V Sr2+(aq) + 2e- Sr(s) ;E° = -2.89 V Co2+(aq) + 2e- Co(s) ;E° = -0.28 V

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Examine the following half-reactions and select the weakest oxidizing agent among the species listed. AuBr4-(aq) + 3e- Au(s) + 4Br-(aq) ;E° = 0.854 V Mn2+(aq) + 2e- Mn(s) ;E° = -1.185 V K+(aq) + e- K(s) ;E° = -2.931 V F2O(aq) + 2H+(aq) + 4e- 2F-(aq) + H2O(l) ;E° = 2.153 V

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Correct Answerverifieda.3.60 x 1...View AnswerShow Answer

If the electrodes of a voltaic cell are connected with an external wire,electrons will flow in this wire from the cathode to the anode.

Correct AnswerverifiedShow Answer

Given that E° for X + e- →\to→ Y is greater than E° for A + 2e- →\to→ B,it is correct to say that,under standard conditions

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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- VO+(aq) + H2O(l) ;E° = 0.991 V

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Consider the reaction of iodine with manganese dioxide 3I2(s) + 2MnO2(s) + 8OH-(aq) 6I-(aq) + 2MnO4-(aq) + 4H2O(l) The equilibrium constant for the overall reaction is 8.30 ×\times× 10-7.Calculate E°cell for the reaction at 25°C.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

A battery that cannot be recharged is a

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When the following redox equation is balanced with smallest whole number coefficients,the coefficient for nitrogen dioxide will be _____. I2(s) + HNO3(aq) →\to→ HIO3(aq) + NO2(g) + H2O(l)

Correct AnswerverifiedShow Answer

How many grams of oxygen gas will be produced in the electrolysis of water,for every gram of hydrogen gas formed? Reaction: 2H2O(l) →\to→ 2H2(g) + O2(g)

Correct AnswerverifiedShow Answer

For the reaction occurring in a voltaic (galvanic)cell, Δ\DeltaΔ G > 0.

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

The Downs cell is used in the electrolysis of

Correct AnswerverifiedShow Answer

Consider the reaction of iodine with manganese dioxide 3I2(s) + 2MnO2(s) + 8OH-(aq) 6I-(aq) + 2MnO4-(aq) + 4H2O(l) The equilibrium constant for the overall reaction is 8.30 ×\times× 10-7.Calculate Δ\DeltaΔ G° for the reaction at 25°C.

Correct AnswerverifiedShow Answer

Correct Answer
verified

When the following redox equation is balanced with smallest whole number coefficients,the coefficient for the hydrogen sulfate ion will be ______. Al(s) + HSO₄^-(aq) + OH^-(aq) $\to$ Al₂O₃(s) + S^2-(aq) + H₂O(l)

Correct Answer
verified

Examine the following half-reactions and select the strongest oxidizing agent among the species listed. Cr²⁺(aq) + 2e^- Cr(s) ;E° = -0.913 V Fe²⁺(aq) + 2e^- Fe(s) ;E° = -0.447 V Sr²⁺(aq) + 2e^- Sr(s) ;E° = -2.89 V Co²⁺(aq) + 2e^- Co(s) ;E° = -0.28 V

Correct Answer
verified

Examine the following half-reactions and select the weakest oxidizing agent among the species listed. AuBr₄^-(aq) + 3e^- Au(s) + 4Br^-(aq) ;E° = 0.854 V Mn²⁺(aq) + 2e^- Mn(s) ;E° = -1.185 V K⁺(aq) + e^- K(s) ;E° = -2.931 V F₂O(aq) + 2H⁺(aq) + 4e^- 2F^-(aq) + H₂O(l) ;E° = 2.153 V

Correct Answer
verified

Correct Answer
verified
a.3.60 x 1...
View Answer

Correct Answer
verified

Given that E° for X + e^- $\to$ Y is greater than E° for A + 2e^- $\to$ B,it is correct to say that,under standard conditions

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^- VO⁺(aq) + H₂O(l) ;E° = 0.991 V

Correct Answer
verified

Correct Answer
verified

Correct Answer
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Correct Answer
verified

When the following redox equation is balanced with smallest whole number coefficients,the coefficient for nitrogen dioxide will be _____. I₂(s) + HNO₃(aq) $\to$ HIO₃(aq) + NO₂(g) + H₂O(l)

Correct Answer
verified

How many grams of oxygen gas will be produced in the electrolysis of water,for every gram of hydrogen gas formed? Reaction: 2H₂O(l) $\to$ 2H₂(g) + O₂(g)

Correct Answer
verified

For the reaction occurring in a voltaic (galvanic)cell, $\Delta$ G > 0.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
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