Question 1

Which equation is correct?

Accepted Answer

A)  E = -(RT/nF) lnK
B)  E° = (RT/nF) lnK
C)  E° = (RT/nF) lnQ
D)  E = -(RT/nF) lnQ
E)  E = E° + lnQF) A) and B)
G) A) and C)

Question 2

A voltaic cell consists of an Au/Au3+ electrode (E° = 1.50 V) and a Cu/ Cu2+ electrode (E° = 0.34 V) .Calculate [Au3+] if [Cu2+] = 1.20 M and Ecell = 1.15 V at 25°C.

Accepted Answer

A)  0.0010 M
B)  0.0020 M
C)  0.010 M
D)  0.020 M
E)  0.41 MF) A) and E)
G) A) and D)

Question 3

What mass of copper can be deposited by the passage of 12.0 A for 25.0 min through a solution of copper(II) sulfate? [1 C = 1 A•s; F = 96,500 C]

Accepted Answer

A)  5.93 g
B)  3.95 g
C)  1.97 g
D)  11.85 g
E)  29.6 gF) All of the above
G) A) and C)

Question 4

_______________ is a process used to coat iron in order to protect it from corrosion.

Accepted Answer

Galvanizat...

Question 5

A current of 250.A flows for 24.0 hours at an anode where the reaction occurring is as follows: Mn2+(aq) + 2H2O(l) → MnO2(s) + 4H+(aq) + 2e-
What mass of MnO2 is deposited at this anode?

Accepted Answer

A)  19.5 kg
B)  12.9 kg
C)  9.73 kg
D)  4.87 kg
E)  2.43 kgF) A) and C)
G) D) and E)

Question 6

Based on the data presented below,which is the strongest oxidizing agent? Half-Reaction E°(V) 
Al3++ 3e- → Al(s) -1.66
AgBr(s) + e- → Ag(s) + Br- +0.07
Sn4++ 2e- → Sn2+  +0.14
Fe3++ e- → Fe2+ +0.77

Accepted Answer

A)  Fe3+
B)  Fe2+
C)  Br-
D)  Al3+
E)  Al(s) F) B) and C)
G) A) and E)

Question 7

Given the following standard reduction potentials in acid solution
O2 + 4H+ + 4e- → 2H2O E° = +1.23V
Sn4+ + 2e- → Sn2+ E° = +0.13V
Zn2+ + 2e- → Zn(s)E° = -0.76V
write the formula of the strongest reducing agent.

Accepted Answer

Question 8

A SHE has the acid concentration of 1 M and the H2 pressure is 1 atm.

Accepted Answer

A) True 
 B)False

Question 9

Based on the following electrochemical cell,what is the standard reduction potential of metal M at 298 K? (R = 8.314 J/K • mol,F = 96500 C/mol)  2+(aq) + 2e- → Fe(s) -0.44 A) -0.54 V B) +0.60 V C) -0.30 V D) +0.56 V E) -0.28 V" class="answers-bank-image d-inline" rel="preload" > Half-Reaction E° (V)  Fe2+(aq) + 2e- → Fe(s) -0.44

Accepted Answer

A)  -0.54 V
B)  +0.60 V
C)  -0.30 V
D)  +0.56 V
E)  -0.28 VF) B) and E)
G) A) and C)

Question 10

Based on the data presented below,which is the strongest reducing agent? PbI2(s) + 2e- 2(s) + 2e-   Pb(s) +2I-(aq) E° = -0.365 V Ca2+(aq) + 2e-   Ca(s) E° = -2.868 V Pt2+(aq) + 2e-   Pt(s) E° = 1.18 V Br2(l) + 2e-   2Br-(aq) E° = 1.066 V A) Pb(s)  B) Ca(s)  C) Pt(s)  D) Br-(aq)  E) Pt2+(aq) " class="answers-bank-image d-inline" rel="preload" > Pb(s) +2I-(aq) E° = -0.365 V
Ca2+(aq) + 2e- 2(s) + 2e-   Pb(s) +2I-(aq) E° = -0.365 V Ca2+(aq) + 2e-   Ca(s) E° = -2.868 V Pt2+(aq) + 2e-   Pt(s) E° = 1.18 V Br2(l) + 2e-   2Br-(aq) E° = 1.066 V A) Pb(s)  B) Ca(s)  C) Pt(s)  D) Br-(aq)  E) Pt2+(aq) " class="answers-bank-image d-inline" rel="preload" > Ca(s) E° = -2.868 V
Pt2+(aq) + 2e- 2(s) + 2e-   Pb(s) +2I-(aq) E° = -0.365 V Ca2+(aq) + 2e-   Ca(s) E° = -2.868 V Pt2+(aq) + 2e-   Pt(s) E° = 1.18 V Br2(l) + 2e-   2Br-(aq) E° = 1.066 V A) Pb(s)  B) Ca(s)  C) Pt(s)  D) Br-(aq)  E) Pt2+(aq) " class="answers-bank-image d-inline" rel="preload" > Pt(s) E° = 1.18 V
Br2(l) + 2e- 2(s) + 2e-   Pb(s) +2I-(aq) E° = -0.365 V Ca2+(aq) + 2e-   Ca(s) E° = -2.868 V Pt2+(aq) + 2e-   Pt(s) E° = 1.18 V Br2(l) + 2e-   2Br-(aq) E° = 1.066 V A) Pb(s)  B) Ca(s)  C) Pt(s)  D) Br-(aq)  E) Pt2+(aq) " class="answers-bank-image d-inline" rel="preload" > 2Br-(aq) E° = 1.066 V

Accepted Answer

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

Question 11

What is E°cell for the following reaction? 2 Ag(s) + Sn2+(aq) → 2 Ag+(aq) + Sn(s) 
Ag+(aq) + e- → Ag(s) E° = 0.80 V
Sn4+(aq) + 2e? →Sn2+(aq) E° = 0.13 V
Sn2+(aq) + 2e- → Sn(s) E° = -0.14 V

Accepted Answer

A)  +0.94 V
B)  -0.94 V
C)  +0.67 V
D)  -0.67 V
E)  +1.34 VF) B) and D)
G) A) and B) B

Question 12

What is ΔG° at 298 K for the following reaction? (F = 96,500 C • mol-1)  2Cr3+(aq) + 6Hg(l) → 2Cr(s) + 3Hg22+(aq) E°cell = 1.59V

Accepted Answer

A)  -921 kJ/mol
B)  -767 kJ/mol
C)  -460 kJ/mol
D)  -307 kJ/mol
E)  -1840 kJ/molF) A) and C)
G) All of the above

Question 13

Aluminum does not corrode in the same manner as iron does,because

Accepted Answer

A)  aluminum does not react with oxygen gas.
B)  a protective layer of aluminum oxide forms on the metal surface.
C)  aluminum is harder to oxidize than iron.
D)  iron gives cathodic protection to aluminum.
E)  the electrical circuit cannot be completed on an aluminum surface.F) A) and D)
G) B) and E)

Question 14

Which electrochemical cell pictured below corresponds to the following cell diagram? Cr(s) | Cr3+(aq,1.0 M) || Sn2+(aq,1.0 M) | Sn(s)

Accepted Answer

A)   3+(aq,1.0 M) || Sn2+(aq,1.0 M) | Sn(s)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
B)   3+(aq,1.0 M) || Sn2+(aq,1.0 M) | Sn(s)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
C)   3+(aq,1.0 M) || Sn2+(aq,1.0 M) | Sn(s)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
D)   3+(aq,1.0 M) || Sn2+(aq,1.0 M) | Sn(s)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >
E)   3+(aq,1.0 M) || Sn2+(aq,1.0 M) | Sn(s)  
A)     
B)     
C)     
D)     
E)    " class="answers-bank-image d-inline" rel="preload" >F) None of the above
G) B) and E)

Question 15

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) C) and D)
G) B) and D)

Question 16

If E° for X + e- → Y is larger than E° for A + 2e- → B,then in a spontaneous process under standard-state 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) C) and D)
G) B) and D)

Question 17

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) C) and D)
G) B) and C)

Question 18

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

Question 19

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) C) and D)
G) A) and C)

Question 20

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

Accepted Answer

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

Exam 19: Electrochemistry

Which equation is correct?

Correct AnswerverifiedShow Answer

A voltaic cell consists of an Au/Au3+ electrode (E° = 1.50 V) and a Cu/ Cu2+ electrode (E° = 0.34 V) .Calculate [Au3+] if [Cu2+] = 1.20 M and Ecell = 1.15 V at 25°C.

Correct AnswerverifiedShow Answer

What mass of copper can be deposited by the passage of 12.0 A for 25.0 min through a solution of copper(II) sulfate? [1 C = 1 A•s; F = 96,500 C]

Correct AnswerverifiedShow Answer

_______________ is a process used to coat iron in order to protect it from corrosion.

Correct AnswerverifiedGalvanizat...View AnswerShow Answer

A current of 250.A flows for 24.0 hours at an anode where the reaction occurring is as follows: Mn2+(aq) + 2H2O(l) → MnO2(s) + 4H+(aq) + 2e- What mass of MnO2 is deposited at this anode?

Correct AnswerverifiedShow Answer

Based on the data presented below,which is the strongest oxidizing agent? Half-Reaction E°(V) Al3++ 3e- → Al(s) -1.66 AgBr(s) + e- → Ag(s) + Br- +0.07 Sn4++ 2e- → Sn2+ +0.14 Fe3++ e- → Fe2+ +0.77

Correct AnswerverifiedShow Answer

Given the following standard reduction potentials in acid solution O2 + 4H+ + 4e- → 2H2O E° = +1.23V Sn4+ + 2e- → Sn2+ E° = +0.13V Zn2+ + 2e- → Zn(s)E° = -0.76V write the formula of the strongest reducing agent.

Correct AnswerverifiedShow Answer

A SHE has the acid concentration of 1 M and the H2 pressure is 1 atm.

Correct AnswerverifiedShow Answer

Based on the following electrochemical cell,what is the standard reduction potential of metal M at 298 K? (R = 8.314 J/K • mol,F = 96500 C/mol) Half-Reaction E° (V) Fe2+(aq) + 2e- → Fe(s) -0.44

Correct AnswerverifiedShow Answer

Based on the data presented below,which is the strongest reducing agent? PbI2(s) + 2e- Pb(s) +2I-(aq) E° = -0.365 V Ca2+(aq) + 2e- Ca(s) E° = -2.868 V Pt2+(aq) + 2e- Pt(s) E° = 1.18 V Br2(l) + 2e- 2Br-(aq) E° = 1.066 V

Correct AnswerverifiedB

What is E°cell for the following reaction? 2 Ag(s) + Sn2+(aq) → 2 Ag+(aq) + Sn(s) Ag+(aq) + e- → Ag(s) E° = 0.80 V Sn4+(aq) + 2e? →Sn2+(aq) E° = 0.13 V Sn2+(aq) + 2e- → Sn(s) E° = -0.14 V

Correct AnswerverifiedB

What is ΔG° at 298 K for the following reaction? (F = 96,500 C • mol-1) 2Cr3+(aq) + 6Hg(l) → 2Cr(s) + 3Hg22+(aq) E°cell = 1.59V

Correct AnswerverifiedShow Answer

Aluminum does not corrode in the same manner as iron does,because

Correct AnswerverifiedShow Answer

Which electrochemical cell pictured below corresponds to the following cell diagram? Cr(s) | Cr3+(aq,1.0 M) || Sn2+(aq,1.0 M) | Sn(s)

Correct AnswerverifiedShow Answer

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

If E° for X + e- → Y is larger than E° for A + 2e- → B,then in a spontaneous process under standard-state conditions,

Correct AnswerverifiedShow Answer

Which is not a redox reaction?

Correct AnswerverifiedShow Answer

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

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

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedA

Correct Answer
verified

A voltaic cell consists of an Au/Au³⁺ electrode (E° = 1.50 V) and a Cu/ Cu²⁺ electrode (E° = 0.34 V) .Calculate [Au³⁺] if [Cu²⁺] = 1.20 M and E_cell = 1.15 V at 25°C.

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified
Galvanizat...
View Answer

A current of 250.A flows for 24.0 hours at an anode where the reaction occurring is as follows: Mn²⁺(aq) + 2H₂O(l) → MnO₂(s) + 4H⁺(aq) + 2e^- What mass of MnO₂ is deposited at this anode?

Correct Answer
verified

Based on the data presented below,which is the strongest oxidizing agent? Half-Reaction E°(V) Al³⁺+ 3e^- → Al(s) -1.66 AgBr(s) + e^- → Ag(s) + Br^- +0.07 Sn⁴⁺+ 2e^- → Sn²⁺+0.14 Fe³⁺+ e^- → Fe²⁺ +0.77

Correct Answer
verified

Given the following standard reduction potentials in acid solution O₂ + 4H⁺ + 4e^- → 2H₂O E° = +1.23V Sn⁴⁺ + 2e^- → Sn²⁺ E° = +0.13V Zn²⁺ + 2e^- → Zn(s)E° = -0.76V write the formula of the strongest reducing agent.

Correct Answer
verified

A SHE has the acid concentration of 1 M and the H₂ pressure is 1 atm.

Correct Answer
verified

Based on the following electrochemical cell,what is the standard reduction potential of metal M at 298 K? (R = 8.314 J/K • mol,F = 96500 C/mol) Half-Reaction E° (V) Fe²⁺(aq) + 2e^- → Fe(s) -0.44

Correct Answer
verified

Based on the data presented below,which is the strongest reducing agent? PbI₂(s) + 2e^- Pb(s) +2I^-(aq) E° = -0.365 V Ca²⁺(aq) + 2e^- Ca(s) E° = -2.868 V Pt²⁺(aq) + 2e^- Pt(s) E° = 1.18 V Br₂(l) + 2e^- 2Br^-(aq) E° = 1.066 V

Correct Answer
verified
B

What is E°_cell for the following reaction? 2 Ag(s) + Sn²⁺(aq) → 2 Ag⁺(aq) + Sn(s) Ag⁺(aq) + e^- → Ag(s) E° = 0.80 V Sn⁴⁺(aq) + 2e^? →Sn²⁺(aq) E° = 0.13 V Sn²⁺(aq) + 2e^- → Sn(s) E° = -0.14 V

Correct Answer
verified
B

What is ΔG° at 298 K for the following reaction? (F = 96,500 C • mol^-1) 2Cr³⁺(aq) + 6Hg(l) → 2Cr(s) + 3Hg₂²⁺(aq) E°_cell = 1.59V

Correct Answer
verified

Correct Answer
verified

Which electrochemical cell pictured below corresponds to the following cell diagram? Cr(s) | Cr³⁺(aq,1.0 M) || Sn²⁺(aq,1.0 M) | Sn(s)

Correct Answer
verified

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 Answer
verified

If E° for X + e^- → Y is larger than E° for A + 2e^- → B,then in a spontaneous process under standard-state conditions,

Correct Answer
verified

Correct Answer
verified

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

Correct Answer
verified

Correct Answer
verified
A