Question 1

Identify the battery that is used as a common flashlight battery.

Accepted Answer

A)   dry-cell battery
B)   lithium-ion battery
C)   lead-acid storage battery
D)   NiCad battery
E)   fuel cellF) A) and D)
G) B) and E)

Question 2

What is undergoing reduction in the redox reaction represented by the following cell notation? Pb(s)  ∣ Pb2+(aq)  2+(aq)    H+(aq)  ∣ H2(g)  ∣ Pt(s)  A)  H2(g)  B)  H+(aq)  C)  Pb2+(aq)  D)  Pb(s)  E)  Pt(s) " class="answers-bank-image d-inline" rel="preload" > H+(aq)  ∣ H2(g)  ∣ Pt(s)

Accepted Answer

A)   H2(g) 
B)   H+(aq) 
C)   Pb2+(aq) 
D)   Pb(s) 
E)   Pt(s) F) D) and E)
G) B) and E)

Question 3

Which of the following is the strongest oxidizing agent?

Accepted Answer

A)   Br2(l) 
B)   Au3+(aq) 
C)   Ag(s) 
D)   Br⁻(aq) 
E)   Au(s) F) D) and E)
G) A) and D)

Question 4

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 2 5°C. (The equation is balanced.)  Pb(s)  + Br2(l)  → Pb2+(aq)  + 2 Br⁻(aq) 
Pb2+(aq)  + 2 e⁻ → Pb(s)  E° = -0.13 V
Br2(l)  + 2 e⁻ → 2 Br⁻(aq)  E° = +1.07 V

Accepted Answer

A)   +1.20 V
B)   +0.94 V
C)   -0.94 V
D)   -1.20 V
E)   -0.60 VF) A) and B)
G) B) and D)

Question 5

What is the reducing agent in the redox reaction represented by the following cell notation? 
Ni(s)  ∣ Ni2+(aq)  2+(aq)    Ag+(aq)  ∣ Ag(s)  A)  Ni(s)  B)  Ni2+(aq)  C)  Ag+(aq)  D)  Ag(s)  E)  Pt(s) " class="answers-bank-image d-inline" rel="preload" > Ag+(aq)  ∣ Ag(s)

Accepted Answer

A)   Ni(s) 
B)   Ni2+(aq) 
C)   Ag+(aq) 
D)   Ag(s) 
E)   Pt(s) F) A) and E)
G) A) and D)

Question 6

Which of the following is TRUE about standard electrode potentials?

Accepted Answer

A)   E°cell is negative for spontaneous reactions.
B)   Electrons will flow from a more positive electrode to a more negative electrode.
C)   The electrode potential of the standard hydrogen electrode is exactly zero.
D)   E°cell is the sum between standard reduction potentials of the anode and the cathode.
E)   The electrode in any half-cell with a greater tendency to undergo reduction is negatively charged relative to the standard hydrogen electrode and therefore has E° < 0.F) B) and E)
G) D) and E)

Question 7

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.)  Br2(l)  + 2Cl-(aq)  → 2Br-(aq)  + Cl2 (g) 
Br2(l)  + 2 e → 2Br-(aq)  E°= 1.09 V
2Cl- (aq)  → Cl2(g)  + 2 e - E°= -1.36 V

Accepted Answer

A)   +0.93 V
B)   +2.24 V
C)   +2.45 V
D)   +5.47 V
E)   +0.67 VF) A) and D)
G) None of the above

Question 8

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25 °C. (The equation is balanced.)  Sn(s)  + 2Ag⁺(aq)  → Sn2+(aq)  + 2Ag(s) 
Sn2+(aq)  + 2 e⁻ → Sn(s)  E° = -0.14 V
Ag⁺(aq)  + e⁻ → Ag(s)  E° = +0.80 V

Accepted Answer

A)   +1.74 V
B)   +0.94 V
C)   +1.08 V
D)   -1.08 V
E)   -1.74 VF) None of the above
G) A) and B)

Question 9

Which of the following reactions would be the most spontaneous at 298 K?

Accepted Answer

A)   A + 2 B → C; E°cell = +0.98 V
B)   A + B → 2 C; E°cell = -0.030 V
C)   A + B → 3 C; E°cell = +0.15 V
D)   A + B → C; E°cell = +1.22 V
E)   A + B → C; E°cell = -1.22 VF) C) and D)
G) A) and B)

Question 10

Explain the significance of the standard hydrogen electrode (SHE) in the tabulation of standard reduction potentials of other species.

Accepted Answer

The SHE is used to construct an electroc...

Question 11

Determine which of the following pairs of reactants will result in a spontaneous reaction at 25 °C.

Accepted Answer

A)   Pb2+(aq)  + Cu(s) ; if E°(Pb2+/Pb)  = -0.13V and E°(Cu2+/Cu)  = +0.16V
B)   Ag+(aq)  + Br⁻(aq) ; if E°(Ag+/Ag)  = 0.80V and E°(Br2/Br-)  = +1.09V
C)   Li+(aq)  + Al(s) ; if E°(Li+/Li)  = -3.04V and E°(Al3+/Al)  = -1.66V
D)   Fe3+(aq)  + Ni(s) ; if E°(Fe3+/Fe)  = -0.04V and E°(Ni2+/Ni)  = -0.23V
E)   Cd2+(aq)  + I-(aq) ; if E°(Cd2+/Cd)  = -0.40V and E°(I2/I-)  = + 0.54VF) A) and B)
G) B) and D)

Question 12

Identify the battery that is in most automobiles.

Accepted Answer

A)   dry-cell battery
B)   lithium-ion battery
C)   lead-acid storage battery
D)   NiCad battery
E)   fuel cellF) A) and D)
G) All of the above

Question 13

A galvanic cell consists of a Zn2+/ Zn half-cell and a standard hydrogen electrode. If the Zn2+/ Zn half-cell standard cell functions as the anode, and the standard cell potential is 0.76 V, what is the standard reduction potential for the Zn2+/ Zn half-cell?

Accepted Answer

A)   -0.76 V
B)   -0.38 V
C)   +0.38 V
D)   +0.76 VE) A) and B)
F) All of the above

Question 14

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °: Cu(s)  ∣ Cu2+(aq, 0.0032 mol L-1)  2+(aq, 0.0032 mol L-1)    Cu2+(aq, 4.48 mol L-1)  ∣ Cu(s)  E°(Cu2+/Cu)  = +0.34 V A)  0.00 V B)  +0.093 V C)  +0.34 V D)  +0.186 V E)  +0.052 V" class="answers-bank-image d-inline" rel="preload" > Cu2+(aq, 4.48 mol L-1)  ∣ Cu(s) 
E°(Cu2+/Cu)  = +0.34 V

Accepted Answer

A)   0.00 V
B)   +0.093 V
C)   +0.34 V
D)   +0.186 V
E)   +0.052 VF) A) and E)
G) D) and E)

Question 15

Determine the redox reaction represented by the following cell notation: 
Mg(s)  ∣ Mg2+(aq)  2+(aq)    Cu2+(aq)  ∣ Cu(s)  A)  Cu(s)  + Mg2+(aq)  → Mg(s)  + Cu2+(aq)  B)  Mg(s)  + Cu2+(aq)  → Cu(s)  + Mg2+(aq)  C)  2Mg(s)  + Cu2+(aq)  → Cu(s)  + 2Mg2+(aq)  D)  2Cu(s)  + Mg2+(aq)  → Mg(s)  + 2Cu2+(aq)  E)  3Mg(s)  + 2Cu2+(aq)  → 2Cu(s)  + 3Mg2+(aq) " class="answers-bank-image d-inline" rel="preload" > Cu2+(aq)  ∣ Cu(s)

Accepted Answer

A)   Cu(s)  + Mg2+(aq)  → Mg(s)  + Cu2+(aq) 
B)   Mg(s)  + Cu2+(aq)  → Cu(s)  + Mg2+(aq) 
C)   2Mg(s)  + Cu2+(aq)  → Cu(s)  + 2Mg2+(aq) 
D)   2Cu(s)  + Mg2+(aq)  → Mg(s)  + 2Cu2+(aq) 
E)   3Mg(s)  + 2Cu2+(aq)  → 2Cu(s)  + 3Mg2+(aq) F) None of the above
G) A) and D)

Question 16

Which of the following metals will dissolve in nitric acid but not hydrochloric acid?

Accepted Answer

A)   Cd; E°(Cd2+/Cd)  = -0.40V
B)   Cr; E°(Cr3+/Cr)  = -0.73V
C)   Mn; E°(Mn2+/Mn)  = -1.18V
D)   Ag; E°(Ag+/Ag)  = +0.80V
E)   Al; E°(Al3+/Al)  = -1.66VF) B) and D)
G) D) and E)

Question 17

Use the provided reduction potentials to calculate ΔrG° for the following redox reaction: 2Al(s)  + 3Mg2+(aq)  → 2Al3+(aq)  + 3Mg(s) 
E°(Al3+/Al)  = -1.66 V and E°(Mg2+/Mg)  = -2.37 V

Accepted Answer

A)   +4.1 × 102 kJ mol-1
B)   +1.4 × 102 kJ mol-1
C)   -2.3 × 102 kJ mol-1
D)   -7.8 × 102 kJ mol-1
E)   +6.8 × 102 kJ mol-1F) A) and B)
G) A) and C)

Question 18

For the galvanic cell reaction, expressed below using shorthand notation, what half-reaction occurs at the cathode? Zn(s)  ∣ Zn2+(aq)  ∣∣ Ni2+(aq)  ∣ Ni(s)

Accepted Answer

A)   Zn(s)  → Zn2+(aq)  + 2 e-
B)   Zn2+(aq)  + 2 e- → Zn(s) 
C)   Ni(s)  → Ni2+(aq)  + 2 e-
D)   Ni2+(aq)  + 2 e- → Ni(s) E) C) and D)
F) A) and B)

Question 19

Describe how water can be made to be a good conductor of electrical current.

Accepted Answer

A)   use pure water
B)   heat the water
C)   add salt
D)   chill the water
E)   vaporize the waterF) C) and D)
G) A) and B)

Question 20

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: Al(s)  ∣ Al3+(aq, 0.115 mol L-1)  3+(aq, 0.115 mol L-1)    Al3+(aq, 3.89 mol L-1)  ∣ Al(s)  E°(Al3+/Al)  = -1.66 V A)  +1.66 V B)  +0.060 V C)  0.00 V D)  +0.090 V E)  +0.030 V" class="answers-bank-image d-inline" rel="preload" > Al3+(aq, 3.89 mol L-1)  ∣ Al(s) 
E°(Al3+/Al)  = -1.66 V

Accepted Answer

A)   +1.66 V
B)   +0.060 V
C)   0.00 V
D)   +0.090 V
E)   +0.030 VF) A) and E)
G) B) and E)

Exam 18: Electrochemistry

Which of the following is the strongest oxidizing agent?

Correct Answer
verified

Determine the redox reaction represented by the following cell notation: Mg(s) ∣ Mg²⁺(aq) Cu²⁺(aq) ∣ Cu(s)

Correct Answer
verified

Identify the battery that is used as a common flashlight battery.

Correct Answer
verified

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: Al(s) ∣ Al³⁺(aq, 0.115 mol L^-1) Al³⁺(aq, 3.89 mol L^-1) ∣ Al(s) E°(Al³⁺/Al) = -1.66 V

Correct Answer
verified

Correct Answer
verified

Describe how water can be made to be a good conductor of electrical current.

Correct Answer
verified

Use the provided reduction potentials to calculate Δ_rG° for the following redox reaction: 2Al(s) + 3Mg²⁺(aq) → 2Al³⁺(aq) + 3Mg(s) E°(Al³⁺/Al) = -1.66 V and E°(Mg²⁺/Mg) = -2.37 V

Correct Answer
verified

Which of the following reactions would be the most spontaneous at 298 K?

Correct Answer
verified

Identify the battery that is in most automobiles.

Correct Answer
verified

Which of the following metals will dissolve in nitric acid but not hydrochloric acid?

Correct Answer
verified

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °: Cu(s) ∣ Cu²⁺(aq, 0.0032 mol L^-1) Cu²⁺(aq, 4.48 mol L^-1) ∣ Cu(s) E°(Cu²⁺/Cu) = +0.34 V

Correct Answer
verified

Correct Answer
verified

Determine which of the following pairs of reactants will result in a spontaneous reaction at 25 °C.

Correct Answer
verified

For the galvanic cell reaction, expressed below using shorthand notation, what half-reaction occurs at the cathode? Zn(s) ∣ Zn²⁺(aq) ∣∣ Ni²⁺(aq) ∣ Ni(s)

Correct Answer
verified

What is the reducing agent in the redox reaction represented by the following cell notation? Ni(s) ∣ Ni²⁺(aq) Ag⁺(aq) ∣ Ag(s)

Correct Answer
verified

Correct Answer
verified

A galvanic cell consists of a Zn²⁺/ Zn half-cell and a standard hydrogen electrode. If the Zn²⁺/ Zn half-cell standard cell functions as the anode, and the standard cell potential is 0.76 V, what is the standard reduction potential for the Zn²⁺/ Zn half-cell?

Correct Answer
verified

Explain the significance of the standard hydrogen electrode (SHE) in the tabulation of standard reduction potentials of other species.

Correct Answer
verified
The SHE is used to construct an electroc...
View Answer

Which of the following is TRUE about standard electrode potentials?

Correct Answer
verified

What is undergoing reduction in the redox reaction represented by the following cell notation? Pb(s) ∣ Pb²⁺(aq) H⁺(aq) ∣ H₂(g) ∣ Pt(s)

Correct Answer
verified

Exam 18: Electrochemistry

Which of the following is the strongest oxidizing agent?

Correct AnswerverifiedShow Answer

Determine the redox reaction represented by the following cell notation: Mg(s) ∣ Mg2+(aq) Cu2+(aq) ∣ Cu(s)

Correct AnswerverifiedShow Answer

Identify the battery that is used as a common flashlight battery.

Correct AnswerverifiedShow Answer

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: Al(s) ∣ Al3+(aq, 0.115 mol L-1) Al3+(aq, 3.89 mol L-1) ∣ Al(s) E°(Al3+/Al) = -1.66 V

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Describe how water can be made to be a good conductor of electrical current.

Correct AnswerverifiedShow Answer

Use the provided reduction potentials to calculate ΔrG° for the following redox reaction: 2Al(s) + 3Mg2+(aq) → 2Al3+(aq) + 3Mg(s) E°(Al3+/Al) = -1.66 V and E°(Mg2+/Mg) = -2.37 V

Correct AnswerverifiedShow Answer

Which of the following reactions would be the most spontaneous at 298 K?

Correct AnswerverifiedShow Answer

Identify the battery that is in most automobiles.

Correct AnswerverifiedShow Answer

Which of the following metals will dissolve in nitric acid but not hydrochloric acid?

Correct AnswerverifiedShow Answer

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °: Cu(s) ∣ Cu2+(aq, 0.0032 mol L-1) Cu2+(aq, 4.48 mol L-1) ∣ Cu(s) E°(Cu2+/Cu) = +0.34 V

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Determine which of the following pairs of reactants will result in a spontaneous reaction at 25 °C.

Correct AnswerverifiedShow Answer

For the galvanic cell reaction, expressed below using shorthand notation, what half-reaction occurs at the cathode? Zn(s) ∣ Zn2+(aq) ∣∣ Ni2+(aq) ∣ Ni(s)

Correct AnswerverifiedShow Answer

What is the reducing agent in the redox reaction represented by the following cell notation? Ni(s) ∣ Ni2+(aq) Ag+(aq) ∣ Ag(s)

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

A galvanic cell consists of a Zn2+/ Zn half-cell and a standard hydrogen electrode. If the Zn2+/ Zn half-cell standard cell functions as the anode, and the standard cell potential is 0.76 V, what is the standard reduction potential for the Zn2+/ Zn half-cell?

Correct AnswerverifiedShow Answer

Explain the significance of the standard hydrogen electrode (SHE) in the tabulation of standard reduction potentials of other species.

Correct AnswerverifiedThe SHE is used to construct an electroc...View AnswerShow Answer

Which of the following is TRUE about standard electrode potentials?

Correct AnswerverifiedShow Answer

What is undergoing reduction in the redox reaction represented by the following cell notation? Pb(s) ∣ Pb2+(aq) H+(aq) ∣ H2(g) ∣ Pt(s)

Correct AnswerverifiedShow Answer

Correct Answer
verified

Determine the redox reaction represented by the following cell notation: Mg(s) ∣ Mg²⁺(aq) Cu²⁺(aq) ∣ Cu(s)

Correct Answer
verified

Correct Answer
verified

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: Al(s) ∣ Al³⁺(aq, 0.115 mol L^-1) Al³⁺(aq, 3.89 mol L^-1) ∣ Al(s) E°(Al³⁺/Al) = -1.66 V

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Use the provided reduction potentials to calculate Δ_rG° for the following redox reaction: 2Al(s) + 3Mg²⁺(aq) → 2Al³⁺(aq) + 3Mg(s) E°(Al³⁺/Al) = -1.66 V and E°(Mg²⁺/Mg) = -2.37 V

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °: Cu(s) ∣ Cu²⁺(aq, 0.0032 mol L^-1) Cu²⁺(aq, 4.48 mol L^-1) ∣ Cu(s) E°(Cu²⁺/Cu) = +0.34 V

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

For the galvanic cell reaction, expressed below using shorthand notation, what half-reaction occurs at the cathode? Zn(s) ∣ Zn²⁺(aq) ∣∣ Ni²⁺(aq) ∣ Ni(s)

Correct Answer
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What is the reducing agent in the redox reaction represented by the following cell notation? Ni(s) ∣ Ni²⁺(aq) Ag⁺(aq) ∣ Ag(s)

Correct Answer
verified

Correct Answer
verified

A galvanic cell consists of a Zn²⁺/ Zn half-cell and a standard hydrogen electrode. If the Zn²⁺/ Zn half-cell standard cell functions as the anode, and the standard cell potential is 0.76 V, what is the standard reduction potential for the Zn²⁺/ Zn half-cell?

Correct Answer
verified

Correct Answer
verified
The SHE is used to construct an electroc...
View Answer

Correct Answer
verified

What is undergoing reduction in the redox reaction represented by the following cell notation? Pb(s) ∣ Pb²⁺(aq) H⁺(aq) ∣ H₂(g) ∣ Pt(s)

Correct Answer
verified