Question 1

A salt bridge allows movement of cations and anions from one half-cell to the other.

Accepted Answer

A) True 
 B)False

Question 2

What is the minimum voltage required for the electrolysis of 1.0 M NaCl in neutral solution? 2H2O + 2Cl- (1.0 M)  → H2(1 atm)  + Cl2(1 atm)  + 2OH-(1 × 10-7 M)  2O + 2Cl- (1.0 M)  → H2(1 atm)  + Cl2(1 atm)  + 2OH-(1 × 10-7 M)    A)  2.19 V B)  1.77 V C)  0.41 V D)  -0.41 V E)  -1.78 V" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   2.19 V
B)   1.77 V
C)   0.41 V
D)   -0.41 V
E)   -1.78 VF) C) and D)
G) C) and E)

Question 3

Complete and balance the following redox equation using the set of smallest whole numbers coefficients. What is the sum of the coefficients? HI + HNO3 → I2 + NO (acidic solution)

Accepted Answer

A)   5
B)   7
C)   14
D)   17
E)   None of these choices is correct.F) B) and E)
G) A) and E)

Question 4

Consider the reaction in the lead-acid cell Pb(s)  + PbO2(s)  + 2H2SO4(aq)  → 2PbSO4(aq)  + 2H2O(l) 
For which E°cell = 2.04 V at 298 K. ΔG° for this reaction is

Accepted Answer

A)   -3.94 × 105 kJ/mol.
B)   -3.94 × 102 kJ/mol.
C)   -1.97 × 105 kJ/mol.
D)   -7.87 × 102 kJ/mol.
E)   -7.87 × 105 kJ/mol.F) A) and E)
G) A) and B)

Question 5

What is the standard free-energy change for the following reaction at 25°C? (F = 96,500 C • mol-1)  2Al(s)  + 3Sn4+(aq,1 M)  → 2Al3+(aq,1 M)  + 3Sn2+(aq,1 M)  -1)  2Al(s)  + 3Sn4+(aq,1 M)  → 2Al3+(aq,1 M)  + 3Sn2+(aq,1 M)    A)  -1.79 kJ/mol B)  1.79 kJ/mol C)  -1.04 × 103 kJ/mol D)  -3.45 × 102 kJ/mol E)  5.18 × 102 kJ/mol" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   -1.79 kJ/mol
B)   1.79 kJ/mol
C)   -1.04 × 103 kJ/mol
D)   -3.45 × 102 kJ/mol
E)   5.18 × 102 kJ/molF) B) and E)
G) A) and E) C

Question 6

If a substance is reduced, it must undergo a

Accepted Answer

A)   gain of electrons.
B)   loss of oxygen.
C)   gain of hydrogen.
D)   loss of electrons.
E)   gain of oxygen.F) B) and E)
G) A) and B) A

Question 7

A metal object is to be gold-plated by an electrolytic procedure using aqueous AuCl3 electrolyte. How much gold may be deposited in 3.0 min by a constant current of 10. A?

Accepted Answer

A)   6.2 × 10-3 mol
B)   9.3 × 10-3 mol
C)   1.8 × 10-2 mol
D)   3.5 × 10-5 mol
E)   1.6 × 102 molF) A) and C)
G) B) and E)

Question 8

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 9

What is E°cell for a galvanic cell represented by the combination of the following half-reactions? cell for a galvanic cell represented by the combination of the following half-reactions?   A)  -0.18 V B)  0.18 V C)  1.28 V D)  1.66 V E)  2.12 V" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   -0.18 V
B)   0.18 V
C)   1.28 V
D)   1.66 V
E)   2.12 VF) A) and E)
G) C) and E)

Question 10

What is ΔG° for the following reaction? (F = 96,500 C • mol -1)  I2(s)  + 2Br-(aq)  → 2I-(aq)  + Br2(l) 
Given:  -1)  I2(s)  + 2Br-(aq)  → 2I-(aq)  + Br2(l)  Given:   A)  +104 kJ/mol B)  -104 kJ/mol C)  +309 kJ/mol D)  +52 kJ/mol E)  -52 kJ/mol" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   +104 kJ/mol
B)   -104 kJ/mol
C)   +309 kJ/mol
D)   +52 kJ/mol
E)   -52 kJ/molF) B) and C)
G) A) and E)

Question 11

A cell can be prepared from copper and tin. What is the E°cell for the galvanic cell that forms from the following half-reactions? cell for the galvanic cell that forms from the following half-reactions?   A)  0.47 V B)  0.21 V C)  -0.21 V D)  -0.47 V E)  0.42 V" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   0.47 V
B)   0.21 V
C)   -0.21 V
D)   -0.47 V
E)   0.42 VF) None of the above
G) All of the above

Question 12

The redox reaction of peroxydisulfate with iodide has been used for many years as part of the iodine clock reaction. 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 is correct.F) A) and D)
G) C) and E)

Question 13

Which element is associated with the term "galvanized"?

Accepted Answer

A)   Ga
B)   Zn
C)   Cd
D)   Hg
E)   PbF) A) and B)
G) A) and C) B

Question 14

What product forms at the anode during the electrolysis of molten NaBr?

Accepted Answer

A)   Na+(l) 
B)   Na(l) 
C)   Br-(l) 
D)   Br3-(l) 
E)   Br2(g) F) C) and D)
G) B) and D)

Question 15

At equilibrium E° = 0.

Accepted Answer

A) True 
 B)False

Question 16

Which is not a redox reaction?

Accepted Answer

A)   Al(OH) 4-(aq)  + 4H+(aq)  → Al3+(aq)  + 4H2O(l) 
B)   C6H12O6(s)  + 6O2(g)  → 6CO2(g)  + 6H2O(l) 
C)   Na6FeCl8(s)  + 2Na(l)  → 8NaCl(s)  + Fe(s) 
D)   2H2O2(aq)  → 2H2O(l)  + O2(g) 
E)   CO2(g)  + H2(g)  → CO(g)  + H2O(g) F) A) and B)
G) A) and E)

Question 17

The Faraday constant represents the charge of 1 mole of electrons.

Accepted Answer

A) True 
 B)False

Question 18

What would you observe if you set up the following electrochemical cell: Ag|AgNO3(0.001 M) ||AgNO3(1 M) |Ag?

Accepted Answer

A)   Electrons will flow from left to right, causing a decrease in the AgNO3 concentration in the left cell, and an increase in the AgNO3 concentration in the right cell.
B)   Electrons will flow from right to left, causing an increase in the AgNO3 concentration in the left cell, and a decrease in the AgNO3 concentration in the right cell.
C)   Electrons will flow from left to right, causing an increase in the AgNO3 concentration in the left cell, and a decrease in AgNO3 concentration in the right cell.
D)   Electrons will flow from right to left, causing a decrease in the AgNO3 concentration in the left cell, and an increase in the AgNO3 concentration in the right cell.
E)   There will be no electron flow because the reduction potential at both electrodes is the same.F) A) and B)
G) D) and E)

Question 19

How much charge must pass through an electrolytic cell to reduce 0.44 mol Ca2+ ion to calcium metal?

Accepted Answer

A)   1.9 ×105 C
B)   8.5 ×104 C
C)   2.1 ×104 C
D)   4.3 ×104 C
E)   0.88 CF) B) and C)
G) A) and D)

Question 20

What is the equilibrium constant at 25°C for the following reaction? (R = 8.314 J/K • mol, F = 96,500 C • mol-1)  -1)    A)  4.1 × 1020 B)  8.2 × 1030 C)  3.3 × 1051 D)  6.7 × 1061 E)  > 9.9 × 1099" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   4.1 × 1020
B)   8.2 × 1030
C)   3.3 × 1051
D)   6.7 × 1061
E)   > 9.9 × 1099F) D) and E)
G) None of the above

Exam 19: Electrochemistry

A salt bridge allows movement of cations and anions from one half-cell to the other.

Correct AnswerverifiedShow Answer

What is the minimum voltage required for the electrolysis of 1.0 M NaCl in neutral solution? 2H2O + 2Cl- (1.0 M) → H2(1 atm) + Cl2(1 atm) + 2OH-(1 × 10-7 M)

Correct AnswerverifiedShow Answer

Complete and balance the following redox equation using the set of smallest whole numbers coefficients. What is the sum of the coefficients? HI + HNO3 → I2 + NO (acidic solution)

Correct AnswerverifiedShow Answer

Consider the reaction in the lead-acid cell Pb(s) + PbO2(s) + 2H2SO4(aq) → 2PbSO4(aq) + 2H2O(l) For which E°cell = 2.04 V at 298 K. ΔG° for this reaction is

Correct AnswerverifiedShow Answer

What is the standard free-energy change for the following reaction at 25°C? (F = 96,500 C • mol-1) 2Al(s) + 3Sn4+(aq,1 M) → 2Al3+(aq,1 M) + 3Sn2+(aq,1 M)

Correct AnswerverifiedC

If a substance is reduced, it must undergo a

Correct AnswerverifiedA

A metal object is to be gold-plated by an electrolytic procedure using aqueous AuCl3 electrolyte. How much gold may be deposited in 3.0 min by a constant current of 10. A?

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

What is E°cell for a galvanic cell represented by the combination of the following half-reactions?

Correct AnswerverifiedShow Answer

What is ΔG° for the following reaction? (F = 96,500 C • mol -1) I2(s) + 2Br-(aq) → 2I-(aq) + Br2(l) Given:

Correct AnswerverifiedShow Answer

A cell can be prepared from copper and tin. What is the E°cell for the galvanic cell that forms from the following half-reactions?

Correct AnswerverifiedShow Answer

The redox reaction of peroxydisulfate with iodide has been used for many years as part of the iodine clock reaction. 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)

Correct AnswerverifiedShow Answer

Which element is associated with the term "galvanized"?

Correct AnswerverifiedB

What product forms at the anode during the electrolysis of molten NaBr?

Correct AnswerverifiedShow Answer

At equilibrium E° = 0.

Correct AnswerverifiedShow Answer

Which is not a redox reaction?

Correct AnswerverifiedShow Answer

The Faraday constant represents the charge of 1 mole of electrons.

Correct AnswerverifiedShow Answer

What would you observe if you set up the following electrochemical cell: Ag|AgNO3(0.001 M) ||AgNO3(1 M) |Ag?

Correct AnswerverifiedShow Answer

How much charge must pass through an electrolytic cell to reduce 0.44 mol Ca2+ ion to calcium metal?

Correct AnswerverifiedShow Answer

What is the equilibrium constant at 25°C for the following reaction? (R = 8.314 J/K • mol, F = 96,500 C • mol-1)

Correct AnswerverifiedShow Answer

Correct Answer
verified

What is the minimum voltage required for the electrolysis of 1.0 M NaCl in neutral solution? 2H₂O + 2Cl^-(1.0 M) → H₂(1 atm) + Cl₂(1 atm) + 2OH^-(1 × 10^-7^M)

Correct Answer
verified

Complete and balance the following redox equation using the set of smallest whole numbers coefficients. What is the sum of the coefficients? HI + HNO₃ → I₂ + NO (acidic solution)

Correct Answer
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Consider the reaction in the lead-acid cell Pb(s) + PbO₂(s) + 2H₂SO₄(aq) → 2PbSO₄(aq) + 2H₂O(l) For which E°_cell = 2.04 V at 298 K. ΔG° for this reaction is

Correct Answer
verified

What is the standard free-energy change for the following reaction at 25°C? (F = 96,500 C • mol^-1) 2Al(s) + 3Sn⁴⁺(aq,1 M) → 2Al³⁺(aq,1 M) + 3Sn²⁺(aq,1 M)

Correct Answer
verified
C

Correct Answer
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A

A metal object is to be gold-plated by an electrolytic procedure using aqueous AuCl₃electrolyte. How much gold may be deposited in 3.0 min by a constant current of 10. A?

Correct Answer
verified

Correct Answer
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What is E°_cell for a galvanic cell represented by the combination of the following half-reactions?

Correct Answer
verified

What is ΔG° for the following reaction? (F = 96,500 C • mol^-1) I₂(s) + 2Br^-(aq) → 2I^-(aq) + Br₂(l) Given:

Correct Answer
verified

A cell can be prepared from copper and tin. What is the E°_cell for the galvanic cell that forms from the following half-reactions?

Correct Answer
verified

The redox reaction of peroxydisulfate with iodide has been used for many years as part of the iodine clock reaction. 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? S₂O₈^2-(aq) + 2H⁺+ 2I^-(aq) → 2HSO₄^-(aq) + I₂(aq)

Correct Answer
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Correct Answer
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B

Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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What would you observe if you set up the following electrochemical cell: Ag|AgNO₃(0.001 M) ||AgNO₃(1 M) |Ag?

Correct Answer
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How much charge must pass through an electrolytic cell to reduce 0.44 mol Ca²⁺ion to calcium metal?

Correct Answer
verified

What is the equilibrium constant at 25°C for the following reaction? (R = 8.314 J/K • mol, F = 96,500 C • mol^-1)

Correct Answer
verified