Question 1

Consider the following redox equation
Mn(OH) 2(s) + MnO4-(aq)   →	o→ MnO42-(aq) (basic solution) 
When the equation is balanced with smallest whole number coefficients,what is the coefficient for OH-(aq) and on which side of the equation is OH-(aq) present?

Accepted Answer

A)  4,reactant side
B)  4,product side
C)  6,reactant side
D)  6,product side
E)  None of these choices is correct. F) B) and E)
G) A) and C)

Question 2

Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous.
Co3+(aq) + e- cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. Co3+(aq) + e-   Co2+(aq) ;E° = 1.82 V MnO4-(aq) + 2H2O(l) + 3e-   MnO2(s) + 4OH-(aq) ;E° = 0.59 V Overall reaction: MnO4-(aq) + 2H2O(l) + 3Co2+(aq)   	o MnO2(s) + 3Co3+(aq) + 4OH-(aq)  A) E°cell = -1.23 V,spontaneous B) E°cell = -1.23 V,nonspontaneous C) E°cell = 1.23 V,spontaneous D) E°cell = 1.23 V,nonspontaneous E) E°cell = -0.05 V,nonspontaneous " class="answers-bank-image d-inline" rel="preload" >
Co2+(aq) ;E° = 1.82 V
MnO4-(aq) + 2H2O(l) + 3e- cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. Co3+(aq) + e-   Co2+(aq) ;E° = 1.82 V MnO4-(aq) + 2H2O(l) + 3e-   MnO2(s) + 4OH-(aq) ;E° = 0.59 V Overall reaction: MnO4-(aq) + 2H2O(l) + 3Co2+(aq)   	o MnO2(s) + 3Co3+(aq) + 4OH-(aq)  A) E°cell = -1.23 V,spontaneous B) E°cell = -1.23 V,nonspontaneous C) E°cell = 1.23 V,spontaneous D) E°cell = 1.23 V,nonspontaneous E) E°cell = -0.05 V,nonspontaneous " class="answers-bank-image d-inline" rel="preload" >
MnO2(s) + 4OH-(aq) ;E° = 0.59 V
Overall reaction:
MnO4-(aq) + 2H2O(l) + 3Co2+(aq)   →	o→ MnO2(s) + 3Co3+(aq) + 4OH-(aq)

Accepted Answer

A)  E°cell = -1.23 V,spontaneous
B)  E°cell = -1.23 V,nonspontaneous
C)  E°cell = 1.23 V,spontaneous
D)  E°cell = 1.23 V,nonspontaneous
E)  E°cell = -0.05 V,nonspontaneous F) C) and D)
G) A) and B)

Question 3

Which of the following statements about voltaic and electrolytic cells is correct?

Accepted Answer

A)  The anode will definitely gain weight in a voltaic cell.
B)  Oxidation occurs at the cathode of both cells.
C)  The free energy change, Δ\DeltaΔ G,is negative for the voltaic cell.
D)  The electrons in the external wire flow from cathode to anode in an electrolytic cell.
E)  None of these statements is correct. F) C) and D)
G) B) and C)

Question 4

Which one of the following is not a redox reaction?

Accepted Answer

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

Question 5

Calculate  Δ\DeltaΔ G° for the reaction of iron(II) ions with one mole of permanganate ions.
MnO4-(aq) + 8H+(aq) + 5e- 4-(aq) + 8H+(aq) + 5e-   Mn2+(aq) + 4H2O(l) ;E° = 1.51 V Fe3+(aq) + e-   Fe2+(aq) ;E°= 0.77 V 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" >
Mn2+(aq) + 4H2O(l) ;E° = 1.51 V
Fe3+(aq) + e- 4-(aq) + 8H+(aq) + 5e-   Mn2+(aq) + 4H2O(l) ;E° = 1.51 V Fe3+(aq) + e-   Fe2+(aq) ;E°= 0.77 V 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" >
Fe2+(aq) ;E°= 0.77 V

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) A) and D)

Question 6

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

Accepted Answer

A)  -3.94  ×	imes×  105 kJ
B)  -3.94  ×	imes×  102 kJ
C)  -1.97  ×	imes×  105 kJ
D)  -7.87  ×	imes×  102 kJ
E)  None of these choices is correct. F) None of the above
G) B) and E)

Question 7

Examine the following half-reactions and select the strongest reducing agent among the species listed.
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) A) and B)
G) A) and C)

Question 8

In one or two short sentences each,explain what is meant by the following terms.
a.galvanic or voltaic cell
b.electrolytic cell
c.salt bridge
d.secondary battery or cell
e.primary battery or cell
f.glass electrode

Accepted Answer

a.A galvanic (voltaic)cell is one in whi...

Question 9

A secondary cell (battery)can operate either as a galvanic or an electrolytic cell.

Accepted Answer

A) True 
 B)False

Question 10

The redox reaction of peroxydisulfate with iodide has been used for many years as part of the iodine clock reaction which introduces students to kinetics.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)   →	o→  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) C) and D)
G) A) and D)

Question 11

Write down equations representing the anode half-reaction,the cathode half-reaction and the overall cell reaction for the lead-acid battery.

Accepted Answer

Anode half-reaction: Pb(s)+ SO₄

Question 12

Examine the following half-reactions and select the weakest reducing agent among the substances.
Cr(OH) 3(s) + 3e- 3(s) + 3e-   Cr(s) + 3OH-(aq) ;E° = -1.48 V SnO2(s) + 2H2O(l) + 4e-   Sn(s) + 4OH-(aq) ;E° = -0.945 V MnO2(s) + 4H+(aq) + 2e-   Mn2+(aq) + 2H2O(l) ;E° = 1.224 V Hg2SO4(s) + 2e-   2Hg(l) + SO42-(aq) ;E° = 0.613 V A) Cr(s)  B) Sn(s)  C) Mn2+(aq)  D) Hg(l)  E) OH-(aq) " class="answers-bank-image d-inline" rel="preload" >
Cr(s) + 3OH-(aq) ;E° = -1.48 V
SnO2(s) + 2H2O(l) + 4e- 3(s) + 3e-   Cr(s) + 3OH-(aq) ;E° = -1.48 V SnO2(s) + 2H2O(l) + 4e-   Sn(s) + 4OH-(aq) ;E° = -0.945 V MnO2(s) + 4H+(aq) + 2e-   Mn2+(aq) + 2H2O(l) ;E° = 1.224 V Hg2SO4(s) + 2e-   2Hg(l) + SO42-(aq) ;E° = 0.613 V A) Cr(s)  B) Sn(s)  C) Mn2+(aq)  D) Hg(l)  E) OH-(aq) " class="answers-bank-image d-inline" rel="preload" >
Sn(s) + 4OH-(aq) ;E° = -0.945 V
MnO2(s) + 4H+(aq) + 2e- 3(s) + 3e-   Cr(s) + 3OH-(aq) ;E° = -1.48 V SnO2(s) + 2H2O(l) + 4e-   Sn(s) + 4OH-(aq) ;E° = -0.945 V MnO2(s) + 4H+(aq) + 2e-   Mn2+(aq) + 2H2O(l) ;E° = 1.224 V Hg2SO4(s) + 2e-   2Hg(l) + SO42-(aq) ;E° = 0.613 V A) Cr(s)  B) Sn(s)  C) Mn2+(aq)  D) Hg(l)  E) OH-(aq) " class="answers-bank-image d-inline" rel="preload" >
Mn2+(aq) + 2H2O(l) ;E° = 1.224 V
Hg2SO4(s) + 2e- 3(s) + 3e-   Cr(s) + 3OH-(aq) ;E° = -1.48 V SnO2(s) + 2H2O(l) + 4e-   Sn(s) + 4OH-(aq) ;E° = -0.945 V MnO2(s) + 4H+(aq) + 2e-   Mn2+(aq) + 2H2O(l) ;E° = 1.224 V Hg2SO4(s) + 2e-   2Hg(l) + SO42-(aq) ;E° = 0.613 V A) Cr(s)  B) Sn(s)  C) Mn2+(aq)  D) Hg(l)  E) OH-(aq) " class="answers-bank-image d-inline" rel="preload" >
2Hg(l) + SO42-(aq) ;E° = 0.613 V

Accepted Answer

A)  Cr(s) 
B)  Sn(s) 
C)  Mn2+(aq) 
D)  Hg(l) 
E)  OH-(aq) F) D) and E)
G) A) and C) C

Question 13

A battery is considered "dead" when

Accepted Answer

A)  Q 
B)  Q = 1
C)  Q > 1
D)  Q = K
E)  Q/K= 0F) A) and C)
G) A) and D)

Question 14

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.F) A) and B)
G) A) and E)

Question 15

The chlor-alkali process produces chlorine,Cl2(g) ,in large quantities.What other industrially important substances are produced in this process?

Accepted Answer

A)  sodium and hydrogen
B)  hydrogen and oxygen
C)  sodium chloride and hydrogen
D)  sodium and oxygen
E)  sodium hydroxide and hydrogenF) C) and D)
G) B) and E) E

Question 16

What product forms at the cathode during the electrolysis of molten NaCl in the Downs cell?

Accepted Answer

A)  Na+(l) 
B)  Na(l) 
C)  Cl-(l) 
D)  NaOH(aq) 
E)  Cl2(g) F) None of the above
G) B) and E)

Question 17

A voltaic cell consists of a Hg/Hg22+ electrode (E°= 0.85 V) and a Sn/Sn2+ electrode (E°= -0.14 V) .Calculate [Sn2+] if [Hg22+] = 0.24 M and Ecell = 1.04 V at 25°C.

Accepted Answer

A)  0.0001 M
B)  0.0007 M
C)  0.005 M
D)  0.03 M
E)  0.05 MF) A) and C)
G) B) and E)

Question 18

In the electrolyte of an electrochemical cell,current is carried by anions moving toward the anode and cations moving in the opposite direction.

Accepted Answer

A) True 
 B)False  True

Question 19

Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous.
H2O2(aq) + 2H+(aq) + 2e- cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. H2O2(aq) + 2H+(aq) + 2e-   2H2O(l) ;E° = 1.77 V Fe3+ (aq) + e-   Fe2+(aq) ;E° = 0.77 V Overall reaction: 2Fe3+(aq) + 2H2O(l)   	o  H2O2(aq) + 2H+(aq) + 2Fe2+(aq)  A) E°cell = -1.00 V,nonspontaneous B) E°cell = -1.00 V,spontaneous C) E°cell = 1.00 V,nonspontaneous D) E°cell = 1.00 V,spontaneous E) E°cell = -0.23 V,nonspontaneous " class="answers-bank-image d-inline" rel="preload" >
2H2O(l) ;E° = 1.77 V
Fe3+ (aq) + e- cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. H2O2(aq) + 2H+(aq) + 2e-   2H2O(l) ;E° = 1.77 V Fe3+ (aq) + e-   Fe2+(aq) ;E° = 0.77 V Overall reaction: 2Fe3+(aq) + 2H2O(l)   	o  H2O2(aq) + 2H+(aq) + 2Fe2+(aq)  A) E°cell = -1.00 V,nonspontaneous B) E°cell = -1.00 V,spontaneous C) E°cell = 1.00 V,nonspontaneous D) E°cell = 1.00 V,spontaneous E) E°cell = -0.23 V,nonspontaneous " class="answers-bank-image d-inline" rel="preload" >
Fe2+(aq) ;E° = 0.77 V
Overall reaction:
2Fe3+(aq) + 2H2O(l)   →	o→  H2O2(aq) + 2H+(aq) + 2Fe2+(aq)

Accepted Answer

A)  E°cell = -1.00 V,nonspontaneous
B)  E°cell = -1.00 V,spontaneous
C)  E°cell = 1.00 V,nonspontaneous
D)  E°cell = 1.00 V,spontaneous
E)  E°cell = -0.23 V,nonspontaneous F) B) and C)
G) D) and E)

Question 20

Which,if any,of the following metals would not be capable of acting as a sacrificial anode when used with iron E°Fe = -0.44 V;all E° values refer to the M2+/M half-cell reactions.

Accepted Answer

A)  manganese,Mn,E° = -1.18 V
B)  cadmium,Cd,E° = -0.40 V
C)  magnesium,Mg,E° = -2.37 V
D)  zinc,Zn,E° = -0.76 V
E)  All of these metals are capable of acting as sacrificial anodes with iron.F) B) and D)
G) A) and E)

Exam 21: Electrochemistry: Chemical Change and Electrical Work

Consider the following redox equation Mn(OH) ₂(s) + MnO₄^-(aq) $\to$ MnO₄^2-(aq) (basic solution) When the equation is balanced with smallest whole number coefficients,what is the coefficient for OH^-(aq) and on which side of the equation is OH^-(aq) present?

Correct Answer
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Correct Answer
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Which of the following statements about voltaic and electrolytic cells is correct?

Correct Answer
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Which one of the following is not a redox reaction?

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

Correct Answer
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Examine the following half-reactions and select the strongest reducing agent among the species listed. 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
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In one or two short sentences each,explain what is meant by the following terms. a.galvanic or voltaic cell b.electrolytic cell c.salt bridge d.secondary battery or cell e.primary battery or cell f.glass electrode

Correct Answer
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a.A galvanic (voltaic)cell is one in whi...
View Answer

A secondary cell (battery)can operate either as a galvanic or an electrolytic cell.

Correct Answer
verified

Correct Answer
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Write down equations representing the anode half-reaction,the cathode half-reaction and the overall cell reaction for the lead-acid battery.

Correct Answer
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Anode half-reaction: Pb(s)+ SO_{4View Answer}

Correct Answer
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C

A battery is considered "dead" when

Correct Answer
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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

The chlor-alkali process produces chlorine,Cl₂(g) ,in large quantities.What other industrially important substances are produced in this process?

Correct Answer
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E

What product forms at the cathode during the electrolysis of molten NaCl in the Downs cell?

Correct Answer
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A voltaic cell consists of a Hg/Hg₂²⁺ electrode (E°= 0.85 V) and a Sn/Sn²⁺ electrode (E°= -0.14 V) .Calculate [Sn²⁺] if [Hg₂²⁺] = 0.24 M and E_cell = 1.04 V at 25°C.

Correct Answer
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In the electrolyte of an electrochemical cell,current is carried by anions moving toward the anode and cations moving in the opposite direction.

Correct Answer
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True

Correct Answer
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Which,if any,of the following metals would not be capable of acting as a sacrificial anode when used with iron E°_Fe = -0.44 V;all E° values refer to the M²⁺/M half-cell reactions.

Correct Answer
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Exam 21: Electrochemistry: Chemical Change and Electrical Work

Consider the following redox equation Mn(OH) 2(s) + MnO4-(aq) →\to→ MnO42-(aq) (basic solution) When the equation is balanced with smallest whole number coefficients,what is the coefficient for OH-(aq) and on which side of the equation is OH-(aq) present?

Correct AnswerverifiedShow Answer

Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. Co3+(aq) + e- Co2+(aq) ;E° = 1.82 V MnO4-(aq) + 2H2O(l) + 3e- MnO2(s) + 4OH-(aq) ;E° = 0.59 V Overall reaction: MnO4-(aq) + 2H2O(l) + 3Co2+(aq) →\to→ MnO2(s) + 3Co3+(aq) + 4OH-(aq)

Correct AnswerverifiedShow Answer

Which of the following statements about voltaic and electrolytic cells is correct?

Correct AnswerverifiedShow Answer

Which one of the following is not a redox reaction?

Correct AnswerverifiedShow Answer

Calculate Δ\DeltaΔ G° for the reaction of iron(II) ions with one mole of permanganate ions. MnO4-(aq) + 8H+(aq) + 5e- Mn2+(aq) + 4H2O(l) ;E° = 1.51 V Fe3+(aq) + e- Fe2+(aq) ;E°= 0.77 V

Correct AnswerverifiedShow Answer

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

Correct AnswerverifiedShow Answer

Examine the following half-reactions and select the strongest reducing agent among the species listed. 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 AnswerverifiedShow Answer

In one or two short sentences each,explain what is meant by the following terms. a.galvanic or voltaic cell b.electrolytic cell c.salt bridge d.secondary battery or cell e.primary battery or cell f.glass electrode

Correct Answerverifieda.A galvanic (voltaic)cell is one in whi...View AnswerShow Answer

A secondary cell (battery)can operate either as a galvanic or an electrolytic cell.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Write down equations representing the anode half-reaction,the cathode half-reaction and the overall cell reaction for the lead-acid battery.

Correct AnswerverifiedAnode half-reaction: Pb(s)+ SO4View AnswerShow Answer

Correct AnswerverifiedC

A battery is considered "dead" when

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

The chlor-alkali process produces chlorine,Cl2(g) ,in large quantities.What other industrially important substances are produced in this process?

Correct AnswerverifiedE

What product forms at the cathode during the electrolysis of molten NaCl in the Downs cell?

Correct AnswerverifiedShow Answer

A voltaic cell consists of a Hg/Hg22+ electrode (E°= 0.85 V) and a Sn/Sn2+ electrode (E°= -0.14 V) .Calculate [Sn2+] if [Hg22+] = 0.24 M and Ecell = 1.04 V at 25°C.

Correct AnswerverifiedShow Answer

In the electrolyte of an electrochemical cell,current is carried by anions moving toward the anode and cations moving in the opposite direction.

Correct AnswerverifiedTrue

Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. H2O2(aq) + 2H+(aq) + 2e- 2H2O(l) ;E° = 1.77 V Fe3+ (aq) + e- Fe2+(aq) ;E° = 0.77 V Overall reaction: 2Fe3+(aq) + 2H2O(l) →\to→ H2O2(aq) + 2H+(aq) + 2Fe2+(aq)

Correct AnswerverifiedShow Answer

Which,if any,of the following metals would not be capable of acting as a sacrificial anode when used with iron E°Fe = -0.44 V;all E° values refer to the M2+/M half-cell reactions.

Correct AnswerverifiedShow Answer

Consider the following redox equation Mn(OH) ₂(s) + MnO₄^-(aq) $\to$ MnO₄^2-(aq) (basic solution) When the equation is balanced with smallest whole number coefficients,what is the coefficient for OH^-(aq) and on which side of the equation is OH^-(aq) present?

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

Correct Answer
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Examine the following half-reactions and select the strongest reducing agent among the species listed. 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
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Correct Answer
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a.A galvanic (voltaic)cell is one in whi...
View Answer

Correct Answer
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Correct Answer
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Correct Answer
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Anode half-reaction: Pb(s)+ SO_{4View Answer}

Correct Answer
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C

Correct Answer
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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
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The chlor-alkali process produces chlorine,Cl₂(g) ,in large quantities.What other industrially important substances are produced in this process?

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E

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A voltaic cell consists of a Hg/Hg₂²⁺ electrode (E°= 0.85 V) and a Sn/Sn²⁺ electrode (E°= -0.14 V) .Calculate [Sn²⁺] if [Hg₂²⁺] = 0.24 M and E_cell = 1.04 V at 25°C.

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True

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Which,if any,of the following metals would not be capable of acting as a sacrificial anode when used with iron E°_Fe = -0.44 V;all E° values refer to the M²⁺/M half-cell reactions.

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