Question 1

When the following redox equation is balanced with the smallest whole number coefficients,what is the coefficient of Sb3+(aq)? BrO3-(aq)+ Sb3+(aq)→ Br-(aq)+ Sb5+(aq) (acidic solution)

Accepted Answer

A) 1 
B) 2 
C) 3 
D) 4 
E) 6

Question 2

Which equation is correct?

Accepted Answer

A) E°cell = E°anode - E°cathode 
B) E°cell = E°cathode + E°anode 
C) E°cell = E°cathode - E°anode 
D) E°cell = E°cathode / E°anode

Question 3

What mass of Cu may be deposited from a Cu2+ solution during electrolysis by a current of 3.00 A for 10.0 hours?

Accepted Answer

A) 63.6 g Cu 
B) 35.6 g Cu 
C) 6.4 g Cu 
D) 3.6 g Cu 
E) 71.2 g Cu

Question 4

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 5

Which metal is not capable of acting as a sacrificial anode when used with iron pipe?

Accepted Answer

A)   
B)   
C)   
D)   
E)

Question 6

A voltaic cell is prepared using copper and silver.Its cell notation is shown below. Cu(s)| Cu2+(aq)|| Ag+(aq)| Ag(s)
Which reaction occurs at the cathode?

Accepted Answer

A) Cu(s)→ Cu2+(aq)+ 2e- 
B) Cu2+(aq)+ 2e- → Cu(s) 
C) Ag(s)→ Ag+(aq)+ e- 
D) Ag+(aq)+ e- → Ag(s) 
E) Cu(s)+ 2Ag+(aq)→ Cu2+(aq)+ 2Ag(s)

Question 7

Which is the correct cell notation for the following reaction? Au3+(aq)+ Al(s)→ Al3+(aq)+ Au(s)

Accepted Answer

A) Al3+(aq)|Al(s)||Au3+(aq)|Au(s) 
B) Al(s)|Al3+(aq)||Au3+(aq)|Au(s) 
C) Al3+(aq)|Au3+(aq)||Al(s)|Au(s) 
D) Al3+(aq)|Au(s)||Au3+(aq)|Al(s) 
E) Au(s)|Al(s)||Au3+(aq)|Al3+(aq)

Question 8

A galvanic cell is constructed using the two hypothetical half-reactions A + e^- → B E° = +1.50 V and C + 2e^- → D E° = -0.50 V a.Calculate the standard potential of this cell,E°_cell . b.Calculate ΔG° for the cell reaction.(1 faraday = 96,500 C)

Accepted Answer

The answer of A galvanic cell is constructed using the...

Question 9

Given Cu2+(aq)+ 2e- → Cu(s)E° = +0.34 V Al3+(aq)+ 3e- → Al(s)E° = -1.66 V
Na+(aq)+ e- → Na(s)E° = -2.71 V
Which of the following reactions will occur?

Accepted Answer

A) 2Na+(aq)+ Cu(s)→ Cu2+(aq)+ 2Na(s) 
B) Al(s)+ 3Na+(aq)→ Al3+(aq)+ 3Na(s) 
C) 2Na(s)+ Cu2+(aq)→ Cu(s)+ 2Na+(aq) 
D) 2Al3+(aq)+ 3Cu(s)→ 3Cu2+(aq)+ 2Al(s) 
E) None of the will occur.

Question 10

Based on the data presented below,which is the strongest oxidizing agent? [PtCl4]2-(aq)+ 2e-
   Pt(s)+ 4Cl-(aq)E° = 0.755V
RuO4(s)+ 8H+(aq)+ 8e-  Ru(s)+ 4H2O(l)E° = 1.038V
FeO42-(aq)+ 8H+(aq)+ 3e-  Fe3+(aq)+4H2O(l)E° = 2.07 V
H4XeO6(aq)+ 2H+(aq)+ 2e-  XeO3(aq)+3H2O(l)E° = 2.42 V

Accepted Answer

A) [PtCl4]2-(aq) 
B) RuO4(s) 
C) HFeO4-(aq) 
D) H4XeO6(aq) 
E) Cl-(aq)

Question 11

Complete and balance the following redox equation.Now sum the coefficients of all species in the balanced equation.(Remember to add the coefficients that are equal to one,and to add the coefficients of any species added to the equation.)The sum of the smallest whole number coefficients is Bi(OH)3 + SnO22- → Bi + SnO32- (basic solution)

Accepted Answer

A) 32 
B) 25 
C) 16 
D) 13 
E) 4

Question 12

Which is the correct cell diagram for the following electrochemical cell?  Half-Reaction E° (V) Sn2+(aq)+ 2e- →Sn(s)-0.14
Fe2+(aq)+ 2e- →Fe(s)-0.44

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 13

Lithium-ion batteries can be recharged many times.

Accepted Answer

A) True 
 B)False

Question 14

What is the cell potential at 25°C for the following reaction if [Zn2+] = 1.0 × 10-4 M and [Sn2+] = 0.20 M ? (R = 8.314 J/K • mol,F = 96,500 C • mol-1) Zn2+(aq)+ Sn(s)→ Zn(s)+ Sn2+(aq)E°cell = -0.62 V

Accepted Answer

A) -0.62 V 
B) +0.52 V 
C) -0.52 V 
D) -0.72 V 
E) +0.72 V

Question 15

What is E°cell for the following reaction? 2Au(s)+ 3Ca2+(aq)→ 2Au3+(aq)+ 3Ca(s)
Au3+(aq)+ 3e- → Au(s)E° = 1.50 V
Ca2+ (aq)+ 2e- → Ca(s)E° = -2.87 V

Accepted Answer

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

Question 16

Consider the reaction CuO(s)+ H2(g)→ Cu(s)+ H2O(l)
In this reaction,which substances are the oxidizing agent and reducing agent,
Respectively?

Accepted Answer

A) CuO and H2 
B) H2 and CuO 
C) CuO and Cu 
D) H2O and H2 
E) Cu and H2O

Question 17

The redox reaction of peroxydisulfate with iodide has been used for many years as part of the iodine clock reaction.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)→ 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.

Question 18

Two cells are connected in series,so that the same current flows through two electrodes,where the following half-reactions occur: Cu2+(aq)+ 2e- → Cu(s)and Ag+(aq)+ e- → Ag(s)
For every 1.00 g of copper produced in the first process,how many grams of silver will be produced in the second one?

Accepted Answer

A) 0.294 g Ag 
B) 0.588 g Ag 
C) 0.850 g Ag 
D) 1.70 g Ag 
E) 3.40 g Ag

Question 19

What is the purpose of a salt bridge in an electrochemical cell?

Accepted Answer

A) A salt bridge provides electrical contact between the electrodes that make up the cell. 
B) A salt bridge carries electrons between the cathode and anode. 
C) A salt bridge insulates the two electrodes. 
D) A salt bridge allows the electrolyte solution to siphon from one side of the cell to the other so the levels remain equal. 
E) A salt bridge allows electrolyte to flow from one half-cell to the other in order to maintain electroneutrality.

Question 20

What is E°cell for the reaction of nickel(II)ions with cadmium metal at 25°C? (R = 8.314 J/K • mol,F = 96,500 C • mol-1)
Ni2+(aq)+ Cd(s)  Cd2+(aq)+ Ni(s)K = 1.17 × 105

Accepted Answer

A) 0.0750 V 
B) 0.100 V 
C) 0.120 V 
D) 0.150 V 
E) 0.300 V

Exam 19: Electrochemistry

When the following redox equation is balanced with the smallest whole number coefficients,what is the coefficient of Sb³⁺(aq) ? BrO₃^-(aq) + Sb³⁺(aq) → Br^-(aq) + Sb⁵⁺(aq) (acidic solution)

Which equation is correct?

What mass of Cu may be deposited from a Cu²⁺ solution during electrolysis by a current of 3.00 A for 10.0 hours?

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 metal is not capable of acting as a sacrificial anode when used with iron pipe?

A voltaic cell is prepared using copper and silver.Its cell notation is shown below. Cu(s) | Cu²⁺(aq) || Ag⁺(aq) | Ag(s) Which reaction occurs at the cathode?

Which is the correct cell notation for the following reaction? Au³⁺(aq) + Al(s) → Al³⁺(aq) + Au(s)

A galvanic cell is constructed using the two hypothetical half-reactions A + e^- → B E° = +1.50 V and C + 2e^- → D E° = -0.50 V a.Calculate the standard potential of this cell,E°_cell . b.Calculate ΔG° for the cell reaction.(1 faraday = 96,500 C)

Given Cu²⁺(aq) + 2e^- → Cu(s) E° = +0.34 V Al³⁺(aq) + 3e^- → Al(s) E° = -1.66 V Na⁺(aq) + e^- → Na(s) E° = -2.71 V Which of the following reactions will occur?

Which is the correct cell diagram for the following electrochemical cell? Half-Reaction E° (V) Sn²⁺(aq) + 2e^- →Sn(s) -0.14 Fe²⁺(aq) + 2e^- →Fe(s) -0.44

Lithium-ion batteries can be recharged many times.

What is the cell potential at 25°C for the following reaction if [Zn²⁺] = 1.0 × 10^-4 M and [Sn²⁺] = 0.20 M ? (R = 8.314 J/K • mol,F = 96,500 C • mol^-1) Zn²⁺(aq) + Sn(s) → Zn(s) + Sn²⁺(aq) E°_cell = -0.62 V

What is E°_cell for the following reaction? 2Au(s) + 3Ca²⁺(aq) → 2Au³⁺(aq) + 3Ca(s) Au³⁺(aq) + 3e^- → Au(s) E° = 1.50 V Ca²⁺ (aq) + 2e^- → Ca(s) E° = -2.87 V

Consider the reaction CuO(s) + H₂(g) → Cu(s) + H₂O(l) In this reaction,which substances are the oxidizing agent and reducing agent, Respectively?

The redox reaction of peroxydisulfate with iodide has been used for many years as part of the iodine clock reaction.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? S₂O₈^2-(aq) + 2H⁺ + 2I^-(aq) → 2HSO₄^-(aq) + I₂(aq)

What is the purpose of a salt bridge in an electrochemical cell?

What is E°_cell for the reaction of nickel(II) ions with cadmium metal at 25°C? (R = 8.314 J/K • mol,F = 96,500 C • mol^-1) Ni²⁺(aq) + Cd(s) Cd²⁺(aq) + Ni(s) K = 1.17 × 10⁵

Exam 19: Electrochemistry

When the following redox equation is balanced with the smallest whole number coefficients,what is the coefficient of Sb3+(aq) ? BrO3-(aq) + Sb3+(aq) → Br-(aq) + Sb5+(aq) (acidic solution)

Which equation is correct?

What mass of Cu may be deposited from a Cu2+ solution during electrolysis by a current of 3.00 A for 10.0 hours?

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 metal is not capable of acting as a sacrificial anode when used with iron pipe?

A voltaic cell is prepared using copper and silver.Its cell notation is shown below. Cu(s) | Cu2+(aq) || Ag+(aq) | Ag(s) Which reaction occurs at the cathode?

Which is the correct cell notation for the following reaction? Au3+(aq) + Al(s) → Al3+(aq) + Au(s)

A galvanic cell is constructed using the two hypothetical half-reactions A + e- → B E° = +1.50 V and C + 2e- → D E° = -0.50 V a.Calculate the standard potential of this cell,E°cell . b.Calculate ΔG° for the cell reaction.(1 faraday = 96,500 C)

Given Cu2+(aq) + 2e- → Cu(s) E° = +0.34 V Al3+(aq) + 3e- → Al(s) E° = -1.66 V Na+(aq) + e- → Na(s) E° = -2.71 V Which of the following reactions will occur?

Based on the data presented below,which is the strongest oxidizing agent? [PtCl4]2-(aq) + 2e- Pt(s) + 4Cl-(aq) E° = 0.755V RuO4(s) + 8H+(aq) + 8e- Ru(s) + 4H2O(l) E° = 1.038V FeO42-(aq) + 8H+(aq) + 3e- Fe3+(aq) +4H2O(l) E° = 2.07 V H4XeO6(aq) + 2H+(aq) + 2e- XeO3(aq) +3H2O(l) E° = 2.42 V

Which is the correct cell diagram for the following electrochemical cell? Half-Reaction E° (V) Sn2+(aq) + 2e- →Sn(s) -0.14 Fe2+(aq) + 2e- →Fe(s) -0.44

Lithium-ion batteries can be recharged many times.

What is the cell potential at 25°C for the following reaction if [Zn2+] = 1.0 × 10-4 M and [Sn2+] = 0.20 M ? (R = 8.314 J/K • mol,F = 96,500 C • mol-1) Zn2+(aq) + Sn(s) → Zn(s) + Sn2+(aq) E°cell = -0.62 V

What is E°cell for the following reaction? 2Au(s) + 3Ca2+(aq) → 2Au3+(aq) + 3Ca(s) Au3+(aq) + 3e- → Au(s) E° = 1.50 V Ca2+ (aq) + 2e- → Ca(s) E° = -2.87 V

Consider the reaction CuO(s) + H2(g) → Cu(s) + H2O(l) In this reaction,which substances are the oxidizing agent and reducing agent, Respectively?

The redox reaction of peroxydisulfate with iodide has been used for many years as part of the iodine clock reaction.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) → 2HSO4-(aq) + I2(aq)

Two cells are connected in series,so that the same current flows through two electrodes,where the following half-reactions occur: Cu2+(aq) + 2e- → Cu(s) and Ag+(aq) + e- → Ag(s) For every 1.00 g of copper produced in the first process,how many grams of silver will be produced in the second one?

What is the purpose of a salt bridge in an electrochemical cell?

What is E°cell for the reaction of nickel(II) ions with cadmium metal at 25°C? (R = 8.314 J/K • mol,F = 96,500 C • mol-1) Ni2+(aq) + Cd(s) Cd2+(aq) + Ni(s) K = 1.17 × 105

When the following redox equation is balanced with the smallest whole number coefficients,what is the coefficient of Sb³⁺(aq) ? BrO₃^-(aq) + Sb³⁺(aq) → Br^-(aq) + Sb⁵⁺(aq) (acidic solution)

What mass of Cu may be deposited from a Cu²⁺ solution during electrolysis by a current of 3.00 A for 10.0 hours?

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?

A voltaic cell is prepared using copper and silver.Its cell notation is shown below. Cu(s) | Cu²⁺(aq) || Ag⁺(aq) | Ag(s) Which reaction occurs at the cathode?

Which is the correct cell notation for the following reaction? Au³⁺(aq) + Al(s) → Al³⁺(aq) + Au(s)

A galvanic cell is constructed using the two hypothetical half-reactions A + e^- → B E° = +1.50 V and C + 2e^- → D E° = -0.50 V a.Calculate the standard potential of this cell,E°_cell . b.Calculate ΔG° for the cell reaction.(1 faraday = 96,500 C)

Given Cu²⁺(aq) + 2e^- → Cu(s) E° = +0.34 V Al³⁺(aq) + 3e^- → Al(s) E° = -1.66 V Na⁺(aq) + e^- → Na(s) E° = -2.71 V Which of the following reactions will occur?

Which is the correct cell diagram for the following electrochemical cell? Half-Reaction E° (V) Sn²⁺(aq) + 2e^- →Sn(s) -0.14 Fe²⁺(aq) + 2e^- →Fe(s) -0.44

What is the cell potential at 25°C for the following reaction if [Zn²⁺] = 1.0 × 10^-4 M and [Sn²⁺] = 0.20 M ? (R = 8.314 J/K • mol,F = 96,500 C • mol^-1) Zn²⁺(aq) + Sn(s) → Zn(s) + Sn²⁺(aq) E°_cell = -0.62 V

What is E°_cell for the following reaction? 2Au(s) + 3Ca²⁺(aq) → 2Au³⁺(aq) + 3Ca(s) Au³⁺(aq) + 3e^- → Au(s) E° = 1.50 V Ca²⁺ (aq) + 2e^- → Ca(s) E° = -2.87 V

Consider the reaction CuO(s) + H₂(g) → Cu(s) + H₂O(l) In this reaction,which substances are the oxidizing agent and reducing agent, Respectively?

The redox reaction of peroxydisulfate with iodide has been used for many years as part of the iodine clock reaction.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? S₂O₈^2-(aq) + 2H⁺ + 2I^-(aq) → 2HSO₄^-(aq) + I₂(aq)

What is E°_cell for the reaction of nickel(II) ions with cadmium metal at 25°C? (R = 8.314 J/K • mol,F = 96,500 C • mol^-1) Ni²⁺(aq) + Cd(s) Cd²⁺(aq) + Ni(s) K = 1.17 × 10⁵