Question 1

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

Accepted Answer

A)  Ag, Cu, Sn, and Zn 
B)  Ag and Cu 
C)  Sn and Cu 
D)  Zn and Cu 
E)  Zn and Sn

Question 2

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-

Question 3

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

Accepted Answer

A)  -4.37 V 
B)  -1.37 V 
C)  -11.6 V 
D)  1.37 V 
E)  4.37 V

Question 4

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 × 10-2

Question 5

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.

Question 6

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

Accepted Answer

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

Question 7

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.

Question 8

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 = -nFlnK

Question 9

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 V

Question 10

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

Accepted Answer

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

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 min

Question 12

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 V

Question 13

Electrons flow to the cathode in a voltaic cell.

Accepted Answer

A) True 
 B)False

Question 14

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

Accepted Answer

A)  -0.398 V 
B)  -2.380 V 
C)  0.398 V 
D)  2.380 V 
E)  6.539 V

Question 15

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 C

Question 16

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

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)

Question 17

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

Accepted Answer

A)  454 kJ/mol 
B)  -454 kJ/mol 
C)  907 kJ/mol 
D)  -907 kJ/mol 
E)  227 kJ/mol

Question 18

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 O2

Question 19

________ 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 20

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 cell

Exam 19: Electrochemistry

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

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

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

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⁺]?

Which statement is correct?

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

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?

Which equation is correct?

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)

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

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?

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)

Electrons flow to the cathode in a voltaic cell.

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

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

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

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

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)

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

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

Exam 19: Electrochemistry

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

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

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

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+]?

Which statement is correct?

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

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?

Which equation is correct?

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)

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

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?

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)

Electrons flow to the cathode in a voltaic cell.

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

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

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

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

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)

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

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

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

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

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⁺]?

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?

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)

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

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?

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)

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

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

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

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)