Question 1

In a fuel cell,an external source of electrical power is used to drive a nonspontaneous reaction in which a fuel is produced.

Accepted Answer

A) True 
 B)False

Question 2

E > 0 and ΔG < 0 for a spontaneous process.

Accepted Answer

A) True 
 B)False

Question 3

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

Accepted Answer

A)  1
B)  2
C)  4
D)  5
E)  10

Question 4

___________ - _________ fuel cells provide electrical power and drinking water for space flights.

Accepted Answer

The answer of ___________ - _________ fuel cells provide electrical...

Question 5

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)

Question 6

What is meant by SHE?

Accepted Answer

A)  Shared half electrodes
B)  Shifting half of the electricity
C)  Standard hydrogen electrode
D)  Small helium electrode
E)  Standard Hg electrode

Question 7

Which of the following is correct?

Accepted Answer

A)  total charge = volts/coulombs
B)  electrical energy = volts × coulombs
C)  Faraday = coulombs/joules
D)  coulombs = joules × volts
E)  electrical work = Faraday's constant/Ecell

Question 8

A voltaic cell consists of a Mn/Mn2+ electrode (E° = -1.18 V) and a Fe/Fe2+ electrode (E° = -0.44 V) .Calculate [Fe2+] if [Mn2+] = 0.050 M and Ecell = 0.78 V at 25°C.

Accepted Answer

A)  0.040 M
B)  0.24 M
C)  1.1 M
D)  1.8 M
E)  None of these choices is correct.

Question 9

If the following electrochemical cell is constructed,what voltage will be measured on the voltmeter? 2+(aq) + 2e- →Zn(s) -0.76 Ag+(aq) + e- → Ag(s) +0.80 A) 2.36 V B) 1.56 V C) 0.04 V D) -0.04 V E) -2.36 V" class="answers-bank-image d-inline" rel="preload" > Half-Reaction E° (V)  Zn2+(aq) + 2e- →Zn(s) -0.76
Ag+(aq) + e- → Ag(s) +0.80

Accepted Answer

A)  2.36 V
B)  1.56 V
C)  0.04 V
D)  -0.04 V
E)  -2.36 V

Question 10

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/mol

Question 11

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.

Question 12

Which is incorrect?

Accepted Answer

A)  At equilibrium,Ecell = 0.
B)  E > 0 for a spontaneous process.
C)  E = 0 for a spontaneous process.
D)  ΔG 
E)  ΔG = 0 at equilibrium.

Question 13

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 14

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 15

Consider the following balanced redox reaction. 3CuO(s) + 2NH3(aq) → N2(g) + 3H2O(l) + 3Cu(s) 
Which of the following statements is true?

Accepted Answer

A)  CuO(s) is the oxidizing agent and copper is reduced.
B)  CuO(s) is the oxidizing agent and copper is oxidized.
C)  CuO(s) is the reducing agent and copper is oxidized.
D)  CuO(s) is the reducing agent and copper is reduced.
E)  CuO(s) is the oxidizing agent and N2(g) is the reducing agent.

Question 16

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) 
Half-Reaction Eo (V) 
Al3+(aq) + 3e- → Al(s) -1.66
Sn4+(aq) + 2e- →Sn2+(aq) +0.13

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/mol

Question 17

______________ 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 18

What is ΔG° for the following reaction? (F = 96,500 C • mol-1)  I2(s) + 2Br-(aq) → 2I-(aq) + Br2(l) 
Given:
I2(s)  (aq) + 2e- → 2I-(aq) E°= 0.53 V
Br2(l) + 2e- → 2Br-(aq) E° = 1.07 V

Accepted Answer

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

Question 19

What is E°cell for the following reaction? 2Fe2+(aq) + Cd2+(aq) → 2Fe3+(aq) + Cd(s) 
Fe3+(aq) + e- →Fe2+ (aq) E° = 0.77 V
Cd2+(aq) + 2e- → Cd(s) E° = -0.40 V

Accepted Answer

A)  -0.37 V
B)  0.37 V
C)  -1.17 V
D)  1.17 V
E)  None of these choices is correct

Question 20

Which of the following elements can be isolated by electrolysis of the aqueous salt shown?

Accepted Answer

A)  Phosphorus from K3PO4(aq) 
B)  Sodium from NaBr(aq) 
C)  Aluminum from AlCl3(aq) 
D)  Fluorine from KF(aq) 
E)  Iodine from NaI(aq)

Exam 19: Electrochemistry

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

What is E°cell for the following reaction? 2Fe2+(aq) + Cd2+(aq) → 2Fe3+(aq) + Cd(s) Fe3+(aq) + e- →Fe2+ (aq) E° = 0.77 V Cd2+(aq) + 2e- → Cd(s) E° = -0.40 V

Correct AnswerverifiedShow Answer

A voltaic cell consists of a Mn/Mn2+ electrode (E° = -1.18 V) and a Fe/Fe2+ electrode (E° = -0.44 V) .Calculate [Fe2+] if [Mn2+] = 0.050 M and Ecell = 0.78 V at 25°C.

Correct AnswerverifiedShow Answer

Which is incorrect?

Correct AnswerverifiedShow Answer

___________ - _________ fuel cells provide electrical power and drinking water for space flights.

Correct AnswerverifiedShow Answer

In a fuel cell,an external source of electrical power is used to drive a nonspontaneous reaction in which a fuel is produced.

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

E > 0 and ΔG < 0 for a spontaneous process.

Correct AnswerverifiedShow Answer

Which of the following is correct?

Correct AnswerverifiedShow Answer

Which of the following elements can be isolated by electrolysis of the aqueous salt shown?

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

Consider the following balanced redox reaction. 3CuO(s) + 2NH3(aq) → N2(g) + 3H2O(l) + 3Cu(s) Which of the following statements is true?

Correct AnswerverifiedShow Answer

If the following electrochemical cell is constructed,what voltage will be measured on the voltmeter? Half-Reaction E° (V) Zn2+(aq) + 2e- →Zn(s) -0.76 Ag+(aq) + e- → Ag(s) +0.80

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

What is ΔG° for the following reaction? (F = 96,500 C • mol-1) I2(s) + 2Br-(aq) → 2I-(aq) + Br2(l) Given: I2(s) (aq) + 2e- → 2I-(aq) E°= 0.53 V Br2(l) + 2e- → 2Br-(aq) E° = 1.07 V

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

What is meant by SHE?

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) Half-Reaction Eo (V) Al3+(aq) + 3e- → Al(s) -1.66 Sn4+(aq) + 2e- →Sn2+(aq) +0.13

Correct AnswerverifiedShow Answer

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 AnswerverifiedShow Answer

Correct Answer
verified

Correct Answer
verified

What is E°_cell for the following reaction? 2Fe²⁺(aq) + Cd²⁺(aq) → 2Fe³⁺(aq) + Cd(s) Fe³⁺(aq) + e^- →Fe²⁺ (aq) E° = 0.77 V Cd²⁺(aq) + 2e^- → Cd(s) E° = -0.40 V

Correct Answer
verified

A voltaic cell consists of a Mn/Mn²⁺ electrode (E° = -1.18 V) and a Fe/Fe²⁺ electrode (E° = -0.44 V) .Calculate [Fe²⁺] if [Mn²⁺] = 0.050 M and E_cell = 0.78 V at 25°C.

Correct Answer
verified

Correct Answer
verified

___ - _ fuel cells provide electrical power and drinking water for space flights.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

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

Consider the following balanced redox reaction. 3CuO(s) + 2NH₃(aq) → N₂(g) + 3H₂O(l) + 3Cu(s) Which of the following statements is true?

Correct Answer
verified

If the following electrochemical cell is constructed,what voltage will be measured on the voltmeter? Half-Reaction E° (V) Zn²⁺(aq) + 2e^- →Zn(s) -0.76 Ag⁺(aq) + e^- → Ag(s) +0.80

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
verified

What is ΔG° for the following reaction? (F = 96,500 C • mol^-1) I₂(s) + 2Br^-(aq) → 2I^-(aq) + Br₂(l) Given: I₂(s) (aq) + 2e^- → 2I^-(aq) E°= 0.53 V Br₂(l) + 2e^- → 2Br^-(aq) E° = 1.07 V

Correct Answer
verified

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

Correct Answer
verified

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) Half-Reaction Eo (V) Al³⁺(aq) + 3e^- → Al(s) -1.66 Sn⁴⁺(aq) + 2e^- →Sn²⁺(aq) +0.13

Correct Answer
verified

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
verified