Question 1

The gas OF2 can be produced from the electrolysis of an aqueous solution of KF,as shown in the equation below. OF2(g) + 2 H+(aq) + 4 e- → H2O(l) + 2 F-(aq) E° = +2.15 V
Using the given standard reduction potential,calculate the amount of OF2 that is produced,and the electrode at which the OF2 is produced,upon the passage of 0.240 faradays through an aqueous KF solution.

Accepted Answer

A)  3.24 g of OF2 at the anode
B)  13.0 g of OF2 at the anode
C)  3.24 g of OF2 at the cathode
D)  13.0 g of OF2 at the cathodeE) All of the above
F) B) and D)

Question 2

For a galvanic cell that uses the following two half-reactions, Cr2O72-(aq) + 14 H+(aq) + 6 e- → 2 Cr3+(aq) + 7 H2O(l) 
Pb(s) → Pb2+(aq) + 2 e-
How many moles of Pb(s) are oxidized by one mole of Cr2O72-?

Accepted Answer

A)  1
B)  2
C)  3
D)  6E) A) and D)
F) A) and C)

Question 3

Given that E°red = -0.26 V for Ni2+/Ni at 25°C,find E° and E for the concentration cell expressed using shorthand notation below. Ni(s) ∣ Ni2+(aq,1.0 × 10-5 M) ∣∣ Ni2+(aq,0.100 M) ∣ Ni(s)

Accepted Answer

A)  E° = 0.00 V and E = +0.24 V
B)  E° = 0.00 V and E = +0.12 V
C)  E° = -0.26 V and E = -0.02 V
D)  E° = -0.26 V and E = -0.14 VE) A) and B)
F) A) and C)

Question 4

Chromium can be electroplated from an aqueous solution containing sulfuric acid and chromic acid,H2CrO4.What current is required to deposit chromium at a rate of 1.25 g/min?

Accepted Answer

A)  38.1 A
B)  38.7 A
C)  116 A
D)  232 AE) A) and B)
F) B) and C)

Question 5

Based on the half-reactions and their respective standard reduction potentials below,what is the standard cell potential for the reaction that is expected to occur? Fe3+(aq) + e- → Fe2+(aq) 0.77 V
Sn4+(aq) + 2 e- → Sn2+(aq) 0.15 V
Pb2+(aq) + 2 e- → Pb(s) -0.13 V

Accepted Answer

A)  0.28 V
B)  0.64 V
C)  0.90 V
D)  1.03 VE) A) and D)
F) All of the above

Question 6

O2(g) + 4 H+(aq) + 4 e-→ 2 H2O(l) E° = +1.23 V I2(s) + 2 e- → 2 I-(aq) E° = +0.54 V
2 H2O(l) + 2 e- → H2(g) + 2 OH-(aq) E° = -0.83 V
Mg2+(aq) + 2 e- → Mg(s) E° = -2.37 V
Based on the data above,electrolysis of an aqueous solution of MgI2,with inert electrodes,is expected to produce

Accepted Answer

A)  Mg at the cathode and I2 at the anode.
B)  H2 at the cathode and I2 at the anode.
C)  Mg at the cathode and O2 at the anode.
D)  H2 at the cathode and O2 at the anode.E) None of the above
F) A) and C)

Question 7

The two half-reactions that are used in the direct methanol fuel cell are shown below.
I.2 CH3OH(aq)+ 2 H2O(l)→ 2 CO2(g)+ 12 H+(aq)+ 12 e-
II.3 O2(g)+ 12 H+(aq)+ 12 e- → 6 H2O(l)
The electrode at which half-reaction I occurs is the ________ at which ________ is oxidized,and half-reaction II occurs at the ________ at which ________ is reduced.

Accepted Answer

anode,CH₃OH...

Question 8

In a galvanic cell,the half-reaction MnO4-(aq) + 8 H+(aq) + 5 e- → Mn2+(aq) + 4 H2O(l) is

Accepted Answer

A)  an oxidation half-reaction and occurs at the anode.
B)  an oxidation half-reaction and occurs at the cathode.
C)  a reduction half-reaction and occurs at the anode.
D)  a reduction half-reaction and occurs at the cathode.E) B) and D)
F) C) and D)

Question 9

According to the balanced chemical equation 5 H2C2O4(aq) + 2 MnO4-(aq) + 6 H+(aq) → 10 CO2(g) + 2 Mn2+(aq) + 8 H2O(l) 
0.875 grams of oxalic acid,H2C2O4 will react with ________ moles of permanganate,MnO4-.

Accepted Answer

A)  0.003885
B)  0.009717
C)  0.019435
D)  0.024295E) All of the above
F) B) and C)

Question 10

What is the relationship between the standard cell potentials,E°,for the following two galvanic cell reactions? I.2 Ag+(aq) + Sn2+(aq) → Sn4+(aq) + 2 Ag(s) 
II.2 Ag(s) + Sn4+(aq) → Sn2+(aq) + 2 Ag+(aq)

Accepted Answer

A)  E°(I) = E°(II) 
B)  .E°(I) = E°(II) 
C)  E°(I) = - E°(II) 
D)  .E°(I) = - E°(II) E) A) and B)
F) B) and C)

Question 11

Which is most often used in the laboratory to measure pH?

Accepted Answer

A)  a standard hydrogen electrode
B)  a glass electrode
C)  a Daniell cell
D)  a conductivity cellE) A) and B)
F) A) and C)

Question 12

In a galvanic cell,the half-reaction H2(g) + 2 OH-(aq) → 2 H2O(l) + 2 e- is

Accepted Answer

A)  an oxidation half-reaction and occurs at the anode.
B)  an oxidation half-reaction and occurs at the cathode.
C)  a reduction half-reaction and occurs at the anode.
D)  a reduction half-reaction and occurs at the cathode.E) C) and D)
F) A) and B)

Question 13

What is the value of the equilibrium constant,K for a redox reaction involving the transfer of 6 mol of electrons if its standard potential is 0.043?

Accepted Answer

A)  4.384 × 105
B)  2.28 × 104
C)  1.70
D)  5.90 × 10-1E) B) and C)
F) A) and D)

Question 14

3+(aq) + Zn(s) → Zn2+(aq) + 2 Fe2+(aq) occurs in the galvanic cell shown above.Which would be the most appropriate choices for the solid electrode in half-cell (A) and in half-cell (B) ? A) Fe(s) for half-cell (A) and Zn(s) for half-cell (B)  B) Pt(s) for half-cell (A) and Zn(s) for half-cell (B)  C) Fe(s) for half-cell (A) and Fe(s) for half-cell (B)  D) Zn(s) for half-cell (A) and Pt(s) for half-cell (B) " class="answers-bank-image d-inline" rel="preload" >
-The cell reaction 2 Fe3+(aq) + Zn(s) → Zn2+(aq) + 2 Fe2+(aq) occurs in the galvanic cell shown above.Which would be the most appropriate choices for the solid electrode in half-cell (A) and in half-cell (B) ?

Accepted Answer

A)  Fe(s) for half-cell (
A)  and Zn(s) for half-cell (
B)  
B)  Pt(s) for half-cell (
A)  and Zn(s) for half-cell (
B)  
C)  Fe(s) for half-cell (
A)  and Fe(s) for half-cell (
B)  
D)  Zn(s) for half-cell (
A)  and Pt(s) for half-cell (
B)  E) All of the above
F) A) and B)

Question 15

Consider the half-reaction: MnO4-(aq) + 8 H+(aq) + 5 e- → Mn2+(aq) + 4 H2O(l) .The formation of MnO4- from Mn2+ occurs most readily when the solution is

Accepted Answer

A)  acidic.
B)  neutral.
C)  basic.
D)  The reaction is not dependent upon pH.E) None of the above
F) A) and C)

Question 16

Determine the number of water molecules necessary to balance the reduction half reaction of  that occurs in an acidic solution.

Accepted Answer

A)  2
B)  4
C)  5
D)  7E) A) and B)
F) None of the above

Question 17

Based on the half-reactions and their respective standard reduction potentials below,the standard cell potential for the reaction that is expected to occur is ________ V.
Ag+(aq)+ e- → Ag(s)0.80 V
2 H+(aq)+ 2 e- → H2(g)0.00 V
Cd2+(aq)+ 2 e- → Cd(s)-0.40 V

Accepted Answer

Question 18

Given: Ag+(aq) + e- → Ag(s) E° = +0.799 V AgI(s) + e- → Ag(s) + I-(aq) E° = -0.152 V
Ni2+(aq) + 2 e- → Ni(s) E° = -0.267 V
Which of the following reactions should be spontaneous under standard conditions?
I.2 AgI(s) + Ni(s) → 2 Ag(s) + 2 I-(aq) + Ni2+(aq) 
II.Ag+(aq) + I-(aq) → AgI(s)

Accepted Answer

A)  I and II are both nonspontaneous.
B)  I is nonspontaneous and II is spontaneous.
C)  I is spontaneous and II is nonspontaneous.
D)  I and II are both spontaneous.E) All of the above
F) A) and B)

Question 19

Consider the galvanic cell shown below. + ion and NO3- ion flow from the salt bridge. A) Al is the anode and Co is the cathode;Na+ ions flow into half-cell compartment (A) and NO3- ions flow into half-cell compartment (B) . B) Al is the anode and Co is the cathode;NO3- ions flow into half-cell compartment (A) and Na+ ions flow into half-cell compartment (B) . C) Co is the anode and Al is the cathode;Na+ ions flow into half-cell compartment (A) and NO3- ions flow into half-cell compartment (B) . D) Co is the anode and Al is the cathode;NO3- ions flow into half-cell compartment (A) and Na+ ions flow into half-cell compartment (B) ." class="answers-bank-image d-inline" rel="preload" >
-Identify the anode and cathode,and indicate the direction of Na+ ion and NO3- ion flow from the salt bridge.

Accepted Answer

A)  Al is the anode and Co is the cathode;Na+ ions flow into half-cell compartment (
A)  and NO3- ions flow into half-cell compartment (
B)  .
B)  Al is the anode and Co is the cathode;NO3- ions flow into half-cell compartment (
A)  and Na+ ions flow into half-cell compartment (
B)  .
C)  Co is the anode and Al is the cathode;Na+ ions flow into half-cell compartment (
A)  and NO3- ions flow into half-cell compartment (
B)  .
D)  Co is the anode and Al is the cathode;NO3- ions flow into half-cell compartment (
A)  and Na+ ions flow into half-cell compartment (
B)  .E) C) and D)
F) A) and B)

Question 20

For the galvanic cell that uses the reaction
2 Al(s)+ 3 Ni2+(aq)→ 2 Al3+(aq)+ 3 Ni(s)
the value of n in the relationship ΔG° = -nFE° is ________.

Accepted Answer

Exam 18: Electrochemistry

In a galvanic cell,the half-reaction MnO₄^-(aq) + 8 H⁺(aq) + 5 e^- → Mn²⁺(aq) + 4 H₂O(l) is

Correct Answer
verified

Determine the number of water molecules necessary to balance the reduction half reaction of that occurs in an acidic solution.

Correct Answer
verified

For the galvanic cell that uses the reaction 2 Al(s)+ 3 Ni²⁺(aq)→ 2 Al³⁺(aq)+ 3 Ni(s) the value of n in the relationship ΔG° = -nFE° is ________.

Correct Answer
verified

Which is most often used in the laboratory to measure pH?

Correct Answer
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Chromium can be electroplated from an aqueous solution containing sulfuric acid and chromic acid,H₂CrO₄.What current is required to deposit chromium at a rate of 1.25 g/min?

Correct Answer
verified

For a galvanic cell that uses the following two half-reactions, Cr₂O₇^2-(aq) + 14 H⁺(aq) + 6 e^- → 2 Cr³⁺(aq) + 7 H₂O(l) Pb(s) → Pb²⁺(aq) + 2 e^- How many moles of Pb(s) are oxidized by one mole of Cr₂O₇^2-?

Correct Answer
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Based on the half-reactions and their respective standard reduction potentials below,what is the standard cell potential for the reaction that is expected to occur? Fe³⁺(aq) + e^- → Fe²⁺(aq) 0.77 V Sn⁴⁺(aq) + 2 e^- → Sn²⁺(aq) 0.15 V Pb²⁺(aq) + 2 e^- → Pb(s) -0.13 V

Correct Answer
verified

According to the balanced chemical equation 5 H₂C₂O₄(aq) + 2 MnO₄^-(aq) + 6 H⁺(aq) → 10 CO₂(g) + 2 Mn²⁺(aq) + 8 H₂O(l) 0.875 grams of oxalic acid,H₂C₂O₄ will react with ________ moles of permanganate,MnO₄^-.

Correct Answer
verified

Correct Answer
verified
anode,CH₃OH...
View Answer

Correct Answer
verified

Correct Answer
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What is the relationship between the standard cell potentials,E°,for the following two galvanic cell reactions? I.2 Ag⁺(aq) + Sn²⁺(aq) → Sn⁴⁺(aq) + 2 Ag(s) II.2 Ag(s) + Sn⁴⁺(aq) → Sn²⁺(aq) + 2 Ag⁺(aq)

Correct Answer
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Consider the galvanic cell shown below. -Identify the anode and cathode,and indicate the direction of Na⁺ ion and NO₃^- ion flow from the salt bridge.

Correct Answer
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What is the value of the equilibrium constant,K for a redox reaction involving the transfer of 6 mol of electrons if its standard potential is 0.043?

Correct Answer
verified

Given that E°_red = -0.26 V for Ni²⁺/Ni at 25°C,find E° and E for the concentration cell expressed using shorthand notation below. Ni(s) ∣ Ni²⁺(aq,1.0 × 10^-5 M) ∣∣ Ni²⁺(aq,0.100 M) ∣ Ni(s)

Correct Answer
verified

In a galvanic cell,the half-reaction H₂(g) + 2 OH^-(aq) → 2 H₂O(l) + 2 e^-is

Correct Answer
verified

Based on the half-reactions and their respective standard reduction potentials below,the standard cell potential for the reaction that is expected to occur is ________ V. Ag⁺(aq)+ e^- → Ag(s)0.80 V 2 H⁺(aq)+ 2 e^- → H₂(g)0.00 V Cd²⁺(aq)+ 2 e^- → Cd(s)-0.40 V

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-The cell reaction 2 Fe³⁺(aq) + Zn(s) → Zn²⁺(aq) + 2 Fe²⁺(aq) occurs in the galvanic cell shown above.Which would be the most appropriate choices for the solid electrode in half-cell (A) and in half-cell (B) ?

Correct Answer
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Correct Answer
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Consider the half-reaction: MnO₄^-(aq) + 8 H⁺(aq) + 5 e- → Mn²⁺(aq) + 4 H₂O(l) .The formation of MnO₄^- from Mn²⁺ occurs most readily when the solution is

Correct Answer
verified

Exam 18: Electrochemistry

In a galvanic cell,the half-reaction MnO4-(aq) + 8 H+(aq) + 5 e- → Mn2+(aq) + 4 H2O(l) is

Correct AnswerverifiedShow Answer

Determine the number of water molecules necessary to balance the reduction half reaction of that occurs in an acidic solution.

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For the galvanic cell that uses the reaction 2 Al(s)+ 3 Ni2+(aq)→ 2 Al3+(aq)+ 3 Ni(s) the value of n in the relationship ΔG° = -nFE° is ________.

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Which is most often used in the laboratory to measure pH?

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Chromium can be electroplated from an aqueous solution containing sulfuric acid and chromic acid,H2CrO4.What current is required to deposit chromium at a rate of 1.25 g/min?

Correct AnswerverifiedShow Answer

For a galvanic cell that uses the following two half-reactions, Cr2O72-(aq) + 14 H+(aq) + 6 e- → 2 Cr3+(aq) + 7 H2O(l) Pb(s) → Pb2+(aq) + 2 e- How many moles of Pb(s) are oxidized by one mole of Cr2O72-?

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Based on the half-reactions and their respective standard reduction potentials below,what is the standard cell potential for the reaction that is expected to occur? Fe3+(aq) + e- → Fe2+(aq) 0.77 V Sn4+(aq) + 2 e- → Sn2+(aq) 0.15 V Pb2+(aq) + 2 e- → Pb(s) -0.13 V

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According to the balanced chemical equation 5 H2C2O4(aq) + 2 MnO4-(aq) + 6 H+(aq) → 10 CO2(g) + 2 Mn2+(aq) + 8 H2O(l) 0.875 grams of oxalic acid,H2C2O4 will react with ________ moles of permanganate,MnO4-.

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Correct Answerverifiedanode,CH3OH...View AnswerShow Answer

Given: Ag+(aq) + e- → Ag(s) E° = +0.799 V AgI(s) + e- → Ag(s) + I-(aq) E° = -0.152 V Ni2+(aq) + 2 e- → Ni(s) E° = -0.267 V Which of the following reactions should be spontaneous under standard conditions? I.2 AgI(s) + Ni(s) → 2 Ag(s) + 2 I-(aq) + Ni2+(aq) II.Ag+(aq) + I-(aq) → AgI(s)

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O2(g) + 4 H+(aq) + 4 e-→ 2 H2O(l) E° = +1.23 V I2(s) + 2 e- → 2 I-(aq) E° = +0.54 V 2 H2O(l) + 2 e- → H2(g) + 2 OH-(aq) E° = -0.83 V Mg2+(aq) + 2 e- → Mg(s) E° = -2.37 V Based on the data above,electrolysis of an aqueous solution of MgI2,with inert electrodes,is expected to produce

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What is the relationship between the standard cell potentials,E°,for the following two galvanic cell reactions? I.2 Ag+(aq) + Sn2+(aq) → Sn4+(aq) + 2 Ag(s) II.2 Ag(s) + Sn4+(aq) → Sn2+(aq) + 2 Ag+(aq)

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Consider the galvanic cell shown below. -Identify the anode and cathode,and indicate the direction of Na+ ion and NO3- ion flow from the salt bridge.

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What is the value of the equilibrium constant,K for a redox reaction involving the transfer of 6 mol of electrons if its standard potential is 0.043?

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Given that E°red = -0.26 V for Ni2+/Ni at 25°C,find E° and E for the concentration cell expressed using shorthand notation below. Ni(s) ∣ Ni2+(aq,1.0 × 10-5 M) ∣∣ Ni2+(aq,0.100 M) ∣ Ni(s)

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In a galvanic cell,the half-reaction H2(g) + 2 OH-(aq) → 2 H2O(l) + 2 e- is

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Based on the half-reactions and their respective standard reduction potentials below,the standard cell potential for the reaction that is expected to occur is ________ V. Ag+(aq)+ e- → Ag(s)0.80 V 2 H+(aq)+ 2 e- → H2(g)0.00 V Cd2+(aq)+ 2 e- → Cd(s)-0.40 V

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-The cell reaction 2 Fe3+(aq) + Zn(s) → Zn2+(aq) + 2 Fe2+(aq) occurs in the galvanic cell shown above.Which would be the most appropriate choices for the solid electrode in half-cell (A) and in half-cell (B) ?

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Consider the half-reaction: MnO4-(aq) + 8 H+(aq) + 5 e- → Mn2+(aq) + 4 H2O(l) .The formation of MnO4- from Mn2+ occurs most readily when the solution is

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In a galvanic cell,the half-reaction MnO₄^-(aq) + 8 H⁺(aq) + 5 e^- → Mn²⁺(aq) + 4 H₂O(l) is

Correct Answer
verified

Correct Answer
verified

For the galvanic cell that uses the reaction 2 Al(s)+ 3 Ni²⁺(aq)→ 2 Al³⁺(aq)+ 3 Ni(s) the value of n in the relationship ΔG° = -nFE° is ________.

Correct Answer
verified

Correct Answer
verified

Chromium can be electroplated from an aqueous solution containing sulfuric acid and chromic acid,H₂CrO₄.What current is required to deposit chromium at a rate of 1.25 g/min?

Correct Answer
verified

For a galvanic cell that uses the following two half-reactions, Cr₂O₇^2-(aq) + 14 H⁺(aq) + 6 e^- → 2 Cr³⁺(aq) + 7 H₂O(l) Pb(s) → Pb²⁺(aq) + 2 e^- How many moles of Pb(s) are oxidized by one mole of Cr₂O₇^2-?

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verified

Based on the half-reactions and their respective standard reduction potentials below,what is the standard cell potential for the reaction that is expected to occur? Fe³⁺(aq) + e^- → Fe²⁺(aq) 0.77 V Sn⁴⁺(aq) + 2 e^- → Sn²⁺(aq) 0.15 V Pb²⁺(aq) + 2 e^- → Pb(s) -0.13 V

Correct Answer
verified

According to the balanced chemical equation 5 H₂C₂O₄(aq) + 2 MnO₄^-(aq) + 6 H⁺(aq) → 10 CO₂(g) + 2 Mn²⁺(aq) + 8 H₂O(l) 0.875 grams of oxalic acid,H₂C₂O₄ will react with ________ moles of permanganate,MnO₄^-.

Correct Answer
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Correct Answer
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anode,CH₃OH...
View Answer

Correct Answer
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Correct Answer
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What is the relationship between the standard cell potentials,E°,for the following two galvanic cell reactions? I.2 Ag⁺(aq) + Sn²⁺(aq) → Sn⁴⁺(aq) + 2 Ag(s) II.2 Ag(s) + Sn⁴⁺(aq) → Sn²⁺(aq) + 2 Ag⁺(aq)

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Consider the galvanic cell shown below. -Identify the anode and cathode,and indicate the direction of Na⁺ ion and NO₃^- ion flow from the salt bridge.

Correct Answer
verified

Correct Answer
verified

Given that E°_red = -0.26 V for Ni²⁺/Ni at 25°C,find E° and E for the concentration cell expressed using shorthand notation below. Ni(s) ∣ Ni²⁺(aq,1.0 × 10^-5 M) ∣∣ Ni²⁺(aq,0.100 M) ∣ Ni(s)

Correct Answer
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In a galvanic cell,the half-reaction H₂(g) + 2 OH^-(aq) → 2 H₂O(l) + 2 e^-is

Correct Answer
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Based on the half-reactions and their respective standard reduction potentials below,the standard cell potential for the reaction that is expected to occur is ________ V. Ag⁺(aq)+ e^- → Ag(s)0.80 V 2 H⁺(aq)+ 2 e^- → H₂(g)0.00 V Cd²⁺(aq)+ 2 e^- → Cd(s)-0.40 V

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-The cell reaction 2 Fe³⁺(aq) + Zn(s) → Zn²⁺(aq) + 2 Fe²⁺(aq) occurs in the galvanic cell shown above.Which would be the most appropriate choices for the solid electrode in half-cell (A) and in half-cell (B) ?

Correct Answer
verified

Correct Answer
verified

Consider the half-reaction: MnO₄^-(aq) + 8 H⁺(aq) + 5 e- → Mn²⁺(aq) + 4 H₂O(l) .The formation of MnO₄^- from Mn²⁺ occurs most readily when the solution is

Correct Answer
verified