Question 1

What mass of oxygen gas is produced in the electrolysis of water, for every gram of hydrogen gas formed? Reaction: 2H2O(l)  → 2H2(g)  + O2(g)

Accepted Answer

A)   32 g O2
B)   16 g O2
C)   64 g O2
D)   20 g O2
E)   8 g O2F) A) and E)
G) C) and E)

Question 2

________ is the process that uses electrical energy to drive a nonspontaneous chemical reaction.

Accepted Answer

The answer of ________ is the process that uses electrical...

Question 3

Electrons flow to the cathode in a voltaic cell.

Accepted Answer

A) True 
 B)False

Question 4

What is ΔG° at 200°C for the following reaction? (F = 96,500 C • mol -1)  2Na(l)  + FeCl2(s)   -1)  2Na(l)  + FeCl2(s)    2NaCl(s)  + Fe(s)  E°cell = 2.35 V A)  454 kJ/mol B)  -454 kJ/mol C)  907 kJ/mol D)  -907 kJ/mol E)  227 kJ/mol" class="answers-bank-image d-inline" rel="preload" > 2NaCl(s)  + Fe(s)  E°cell = 2.35 V

Accepted Answer

A)   454 kJ/mol
B)   -454 kJ/mol
C)   907 kJ/mol
D)   -907 kJ/mol
E)   227 kJ/molF) A) and B)
G) All of the above

Question 5

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) C) and E)
G) A) and B)

Question 6

A voltaic cell consists of a Cd/Cd2+ electrode (E° = -0.40 V)  and a Fe/Fe2+ electrode (E° = -0.44 V) . If Ecell = 0 and the temperature is 25°C, what is the ratio [Fe2+]/[Cd2+]?

Accepted Answer

A)   2.3 × 101
B)   1.0 × 101
C)   1.0
D)   1.0 × 10-1
E)   5.0 × 10-2F) C) and D)
G) C) and E)

Question 7

What is E°cell for the following reaction? 2Au(s)  + 3Ca2+(aq)  → 2Au3+(aq)  + 3Ca(s)  cell for the following reaction? 2Au(s)  + 3Ca2+(aq)  → 2Au3+(aq)  + 3Ca(s)    A)  -4.37 V B)  -1.37 V C)  -11.6 V D)  1.37 V E)  4.37 V" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   -4.37 V
B)   -1.37 V
C)   -11.6 V
D)   1.37 V
E)   4.37 VF) B) and D)
G) C) and D)

Question 8

Based on the data presented below, which is the strongest reducing agent? -(aq)  E)  Pt2+(aq) " class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   Pb(s) 
B)   Ca(s) 
C)   Pt(s) 
D)   Br-(aq) 
E)   Pt2+(aq) F) C) and E)
G) B) and E)

Question 9

The voltaic cell composed of Co(s) , Co2+(aq) , Cu(s) , and Cu2+(aq)  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)   0.21 VF) A) and B)
G) A) and C)

Question 10

What is the name given to the apparatus where oxidation occurs in a cell where electricity flows?

Accepted Answer

A)   Cathode
B)   Electrode
C)   Galvanic cell
D)   Anode
E)   Voltaic cellF) D) and E)
G) A) and C)

Question 11

How many minutes would be required to electroplate 25.0 g of chromium by passing a constant current of 4.80 A through a solution containing CrCl3?

Accepted Answer

A)   483 min
B)   161 min
C)   322 min
D)   2.01 × 104 min
E)   1.11 × 104 minF) A) and C)
G) B) and C)

Question 12

What quantity of charge is required to cause reduction of 0.20 mole of Cr3+ to Cr?

Accepted Answer

A)   0.60 C
B)   3.0 C
C)   1.9 × 104 C
D)   5.8 × 104 C
E)   9.7 × 104 CF) C) and E)
G) C) and D)

Question 13

What is ΔG° for the reaction of iron(II)  ions with one mole of permanganate ions? (F = 96,500 C • mol -1)   -1)    A)  -71.4 kJ B)  -286 kJ C)  -357 kJ D)  -428 kJ E)  None of these choices is correct." class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   -71.4 kJ
B)   -286 kJ
C)   -357 kJ
D)   -428 kJ
E)   None of these choices is correct.F) C) and D)
G) B) and D)

Question 14

Which statement is correct?

Accepted Answer

A)   The cathode is the electrode where the oxidation takes place.
B)   The cathode is the electrode where the reduction takes place.
C)   Both oxidation and reduction make take place at the cathode, depending on the cell.
D)   The cathode is always positive.
E)   The anode is always negative.F) D) and E)
G) A) and B)

Question 15

Which is the half-reaction at the cathode in a lead storage battery?

Accepted Answer

A)   Pb(s) + PbO2(s)  + 4H+(aq)  + 2SO42-(aq)  → 2PbSO4(s)  + 2H2O(l) 
B)   PbO2(s)  + 4H+(aq)  + 2SO42-(aq)  + 2e- → PbSO4(s)  + 2H2O(l) 
C)   Pb(s)  + SO42-(aq)  → PbSO4(s)  + 2e-
D)   Pb(s)  → Pb(s)  + 2e-
E)   H2(g)  → 2H+(aq)  + 2e-F) B) and C)
G) A) and C)

Question 16

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)  -0.398 V B)  -2.380 V C)  0.398 V D)  2.380 V E)  6.539 V" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   -0.398 V
B)   -2.380 V
C)   0.398 V
D)   2.380 V
E)   6.539 VF) C) and E)
G) C) and D)

Question 17

Which is the correct cell diagram for the following electrochemical cell? 2+(aq, 1.0 M)  || Fe2+(aq, 1.0 M)  | Fe(s)  B)  Sn(s)  | Fe2+(aq, 1.0 M)  || Sn2+(aq, 1.0 M)  | Fe(s)  C)  Fe(s)  | Sn2+(aq, 1.0 M)  || Fe2+(aq, 1.0 M)  | Sn(s)  D)  Fe(s)  | Fe2+(aq, 1.0 M)  || Sn2+(aq, 1.0 M)  | Sn(s)  E)  Sn(s)  | Fe(s)  || Sn2+(aq, 1.0 M)  | Fe2+(aq, 1.0 M) " class="answers-bank-image d-inline" rel="preload" > 2+(aq, 1.0 M)  || Fe2+(aq, 1.0 M)  | Fe(s)  B)  Sn(s)  | Fe2+(aq, 1.0 M)  || Sn2+(aq, 1.0 M)  | Fe(s)  C)  Fe(s)  | Sn2+(aq, 1.0 M)  || Fe2+(aq, 1.0 M)  | Sn(s)  D)  Fe(s)  | Fe2+(aq, 1.0 M)  || Sn2+(aq, 1.0 M)  | Sn(s)  E)  Sn(s)  | Fe(s)  || Sn2+(aq, 1.0 M)  | Fe2+(aq, 1.0 M) " class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   Sn(s)  | Sn2+(aq, 1.0 M)  || Fe2+(aq, 1.0 M)  | Fe(s) 
B)   Sn(s)  | Fe2+(aq, 1.0 M)  || Sn2+(aq, 1.0 M)  | Fe(s) 
C)   Fe(s)  | Sn2+(aq, 1.0 M)  || Fe2+(aq, 1.0 M)  | Sn(s) 
D)   Fe(s)  | Fe2+(aq, 1.0 M)  || Sn2+(aq, 1.0 M)  | Sn(s) 
E)   Sn(s)  | Fe(s)  || Sn2+(aq, 1.0 M)  | Fe2+(aq, 1.0 M) F) B) and E)
G) A) and E)

Question 18

If ΔG° of the following reaction is -110 kJ/mol, what is E°cell? (F = 96,500 C • mol -1)  A3+(aq)  + 3B(s)  → A(s)  + 3B+(aq)

Accepted Answer

A)   +0.38 V
B)   -0.09 V
C)   -0.38 V
D)   +0.00038 V
E)   +0.09 VF) None of the above
G) B) and D)

Question 19

Which metals may be oxidized by H+ under standard-state conditions? + under standard-state conditions?   A)  Ag, Cu, Sn, and Zn B)  Ag and Cu C)  Sn and Cu D)  Zn and Cu E)  Zn and Sn" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   Ag, Cu, Sn, and Zn
B)   Ag and Cu
C)   Sn and Cu
D)   Zn and Cu
E)   Zn and SnF) A) and B)
G) None of the above

Question 20

Which equation is correct?

Accepted Answer

A)   Ecell = RT lnK
B)   ΔG = -nFEcell
C)   Ecell = -RT lnK
D)   K = E°cell/nRT
E)   E°cell = -nFlnKF) A) and D)
G) B) and C)

Exam 19: Electrochemistry

A voltaic cell consists of a Cd/Cd2+ electrode (E° = -0.40 V) and a Fe/Fe2+ electrode (E° = -0.44 V) . If Ecell = 0 and the temperature is 25°C, what is the ratio [Fe2+]/[Cd2+]?

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

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The voltaic cell composed of Co(s) , Co2+(aq) , Cu(s) , and Cu2+(aq) 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

What is ΔG° at 200°C for the following reaction? (F = 96,500 C • mol -1) 2Na(l) + FeCl2(s) 2NaCl(s) + Fe(s) E°cell = 2.35 V

Correct AnswerverifiedShow Answer

________ is the process that uses electrical energy to drive a nonspontaneous chemical reaction.

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If ΔG° of the following reaction is -110 kJ/mol, what is E°cell? (F = 96,500 C • mol -1) A3+(aq) + 3B(s) → A(s) + 3B+(aq)

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What is ΔG° for the reaction of iron(II) ions with one mole of permanganate ions? (F = 96,500 C • mol -1)

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Which is the correct cell diagram for the following electrochemical cell?

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Which is the half-reaction at the cathode in a lead storage battery?

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Based on the data presented below, which is the strongest reducing agent?

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What is the name given to the apparatus where oxidation occurs in a cell where electricity flows?

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Which metals may be oxidized by H+ under standard-state conditions?

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What mass of oxygen gas is produced in the electrolysis of water, for every gram of hydrogen gas formed? Reaction: 2H2O(l) → 2H2(g) + O2(g)

Correct AnswerverifiedShow Answer

How many minutes would be required to electroplate 25.0 g of chromium by passing a constant current of 4.80 A through a solution containing CrCl3?

Correct AnswerverifiedShow Answer

What quantity of charge is required to cause reduction of 0.20 mole of Cr3+ to Cr?

Correct AnswerverifiedShow Answer

What is E°cell for the following reaction? 2Au(s) + 3Ca2+(aq) → 2Au3+(aq) + 3Ca(s)

Correct AnswerverifiedShow Answer

Electrons flow to the cathode in a voltaic cell.

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Which statement is correct?

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Which equation is correct?

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A voltaic cell consists of a Cd/Cd²⁺ electrode (E° = -0.40 V) and a Fe/Fe²⁺ electrode (E° = -0.44 V) . If E_cell = 0 and the temperature is 25°C, what is the ratio [Fe²⁺]/[Cd²⁺]?

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

Correct Answer
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The voltaic cell composed of Co(s) , Co²⁺(aq) , Cu(s) , and Cu²⁺(aq) 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

What is ΔG° at 200°C for the following reaction? (F = 96,500 C • mol^-1) 2Na(l) + FeCl₂(s) 2NaCl(s) + Fe(s) E°_cell = 2.35 V

Correct Answer
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Correct Answer
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If ΔG° of the following reaction is -110 kJ/mol, what is E°_cell? (F = 96,500 C • mol^-1) A³⁺(aq) + 3B(s) → A(s) + 3B⁺(aq)

Correct Answer
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What is ΔG° for the reaction of iron(II) ions with one mole of permanganate ions? (F = 96,500 C • mol^-1)

Correct Answer
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Correct Answer
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Correct Answer
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Which metals may be oxidized by H⁺ under standard-state conditions?

Correct Answer
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What mass of oxygen gas is produced in the electrolysis of water, for every gram of hydrogen gas formed? Reaction: 2H₂O(l) → 2H₂(g) + O₂(g)

Correct Answer
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How many minutes would be required to electroplate 25.0 g of chromium by passing a constant current of 4.80 A through a solution containing CrCl₃?

Correct Answer
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What quantity of charge is required to cause reduction of 0.20 mole of Cr³⁺ to Cr?

Correct Answer
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What is E°_cell for the following reaction? 2Au(s) + 3Ca²⁺(aq) → 2Au³⁺(aq) + 3Ca(s)

Correct Answer
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Correct Answer
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