Question 1

What is the oxidizing agent in the redox reaction represented by the following cell notation?
Sn(s) ∣ Sn2+(aq) ∣∣ Ag+(aq) ∣ Ag(s)

Accepted Answer

A)  Sn(s) 
B)  Ag+(aq) 
C)  Sn2+(aq) 
D)  Ag(s) 
E)  Pt

Question 2

What mass of aluminum can be plated onto an object in 755 minutes at 5.80 A of current?

Accepted Answer

A)  73.5 g
B)  24.5 g
C)  220.g
D)  147 g
E)  8.17 g

Question 3

Based on the following information,
Cl2(g) + 2 e- → 2 Cl-(aq) E° = +1.36 V
Mg2+(aq) + 2 e- → 2 Mg(s) E° = -2.37 V
Which of the following chemical species is the strongest reducing agent?

Accepted Answer

A)  Cl2(g) 
B)  Mg2+(aq) 
C)  Cl-(aq) 
D)  Mg(s)

Question 4

Match the following.
-Q < K

Accepted Answer

A)  Ecell = E°cell
B)  Ecell = 0
C)  E°cell 
D)  Ecell 
E)  E°cell > 0F) Ecell > 0

Question 5

Identify oxidation.

Accepted Answer

A)  increase in oxidation number
B)  loss of electrons
C)  gain of electrons
D)  decrease in oxidation number
E)  both A and B

Question 6

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. ) 
Mg(s) + Cu2+(aq) → Cu(s) + Mg2+(aq) 
2+(aq) → Cu(s) + Mg2+(aq)    A) 2.04 V B) -2.04 V C) 2.72 V D) -1.36 V E) 1.36 V" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  2.04 V
B)  -2.04 V
C)  2.72 V
D)  -1.36 V
E)  1.36 V

Question 7

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C.
Sn(s) ∣ Sn2+(aq,0.022 M) 2+(aq,0.022 M)  Ag+(aq,2.7 M) ∣ Ag(s)    A) 1.01 V B) -0.83 V C) 1.31 V D) 0.01 V E) -0.66 V" class="answers-bank-image d-inline" rel="preload" >Ag+(aq,2.7 M) ∣ Ag(s) 
2+(aq,0.022 M)  Ag+(aq,2.7 M) ∣ Ag(s)    A) 1.01 V B) -0.83 V C) 1.31 V D) 0.01 V E) -0.66 V" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  1.01 V
B)  -0.83 V
C)  1.31 V
D)  0.01 V
E)  -0.66 V

Question 8

Use the tabulated half-cell potentials below to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C.
3 I2(s) + 2 Fe(s) → 2 Fe3+(aq) + 6 I⁻(aq) 
2(s) + 2 Fe(s) → 2 Fe3+(aq) + 6 I⁻(aq)    A) 3.5 × 10-59 B) 1.1 × 1017 C) 2.4 × 1058 D) 8.9 × 10-18 E) 1.7 × 1029" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  3.5 × 10-59
B)  1.1 × 1017
C)  2.4 × 1058
D)  8.9 × 10-18
E)  1.7 × 1029

Question 9

Give the type of battery that most cars contain.

Accepted Answer

A)  lead-acid battery
B)  dry-cell battery
C)  alkaline battery
D)  nickel-cadmium battery
E)  nickel-metal hydride battery

Question 10

What is the balanced equation for the galvanic cell reaction expressed using shorthand notation below?
Ni(s) ∣ Ni2+(aq) ∣∣ Cl2(g) ∣ Cl-(aq) ∣ C(s)

Accepted Answer

A)  Ni(s) + 2 Cl-(aq) → Ni2+(aq) + Cl2(g) 
B)  Ni(s) + Cl2(g) → Ni2+(aq) + 2 Cl-(aq) 
C)  Ni2+(aq) + 2 Cl-(aq) → Ni(s) + Cl2(g) 
D)  Ni2+(aq) + 2 Cl-(aq) → NiCl2(s)

Question 11

A voltaic cell is constructed with two Zn2+-Zn electrodes,where the half-reaction is
Zn2+(aq) + 2e- → Zn(s) E° = -0.763 V
The concentrations of zinc ion in the two compartments are 5.50 M and 1.11 × 10-2 M,respectively.The cell emf is ________ V.

Accepted Answer

A)  -1.54 × 10-3
B)  -378
C)  0.0798
D)  0.160
E)  -0.761

Question 12

Which of the following metals,if coated onto iron,would prevent the corrosion (oxidation) of iron?

Accepted Answer

A)  Zn
B)  Cu
C)  Ag
D)  Au

Question 13

How many seconds are required to produce 4.00 g of aluminum metal from the electrolysis of molten AlCl3 with an electrical current of 12.0 A?

Accepted Answer

A)  27.0
B)  9.00
C)  1.19 × 103
D)  2.90 × 105
E)  3.57 × 103

Question 14

Match the following.
-ΔG° < 0

Accepted Answer

A)  Ecell = E°cell
B)  Ecell = 0
C)  E°cell 
D)  Ecell 
E)  E°cell > 0F) Ecell > 0

Question 15

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C.
Cu(s) ∣ Cu2+(aq,0.0032 M) ∣∣ Cu2+(aq,4.48 M) ∣ Cu(s) 
2+(aq,0.0032 M) ∣∣ Cu2+(aq,4.48 M) ∣ Cu(s)    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" >

Accepted Answer

A)  0.00 V
B)  0.093 V
C)  0.34 V
D)  0.186 V
E)  0.052 V

Question 16

Balance the following redox reaction if it occurs in acidic solution.What are the coefficients in front of H2C2O4 and H2O in the balanced reaction?
MnO4⁻(aq) + H2C2O4(aq) → Mn2+(aq) + CO2(g)

Accepted Answer

A)  H2C2O4 = 5,H2O = 8
B)  H2C2O4 = 1,H2O = 1
C)  H2C2O4 = 5,H2O = 1
D)  H2C2O4 = 1,H2O = 4
E)  H2C2O4 = 3,H2O = 2

Question 17

Given that E°red = -1.66 V for Al3+/Al at 25°C,find E° and E for the concentration cell expressed using shorthand notation below.
Al(s) ∣ Al3+(1.0 × 10-5 M) ∣∣ Al3+(0.100 M) ∣ Al(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° = -1.66 V and E = -1.42 V
D)  E° = -1.66 V and E = -1.54 V

Question 18

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

Accepted Answer

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

Question 19

Use the tabulated half-cell potentials below to calculate ΔG° for the following redox reaction.
2 Al(s) + 3 Mg2+(aq) → 2 Al3+(aq) + 3 Mg(s) 
2+(aq) → 2 Al3+(aq) + 3 Mg(s)    A) 4.1 × 102 kJ B) 1.4 × 102 kJ C) -2.3 × 102 kJ D) -7.8 × 102 kJ E) 6.8 × 102 kJ" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  4.1 × 102 kJ
B)  1.4 × 102 kJ
C)  -2.3 × 102 kJ
D)  -7.8 × 102 kJ
E)  6.8 × 102 kJ

Question 20

Give the criteria for a nonspontaneous reaction.

Accepted Answer

A) ΔG° cell > 0,K > 1 B) ΔG° > 0,E°cell > 0,K > 1 C) ΔG° > 0,E°cell 1 D) ΔG° cell > 0,K E) ΔG° > 0,E°cell < 0,K < 1

Exam 18: Electrochemistry

How many seconds are required to produce 4.00 g of aluminum metal from the electrolysis of molten AlCl3 with an electrical current of 12.0 A?

Correct AnswerverifiedShow Answer

Which of the following metals,if coated onto iron,would prevent the corrosion (oxidation) of iron?

Correct AnswerverifiedShow Answer

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Cu(s) ∣ Cu2+(aq,0.0032 M) ∣∣ Cu2+(aq,4.48 M) ∣ Cu(s)

Correct AnswerverifiedShow Answer

What is the oxidizing agent in the redox reaction represented by the following cell notation? Sn(s) ∣ Sn2+(aq) ∣∣ Ag+(aq) ∣ Ag(s)

Correct AnswerverifiedShow Answer

What is the balanced equation for the galvanic cell reaction expressed using shorthand notation below? Ni(s) ∣ Ni2+(aq) ∣∣ Cl2(g) ∣ Cl-(aq) ∣ C(s)

Correct AnswerverifiedShow Answer

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. ) Mg(s) + Cu2+(aq) → Cu(s) + Mg2+(aq)

Correct AnswerverifiedShow Answer

Given that E°red = -1.66 V for Al3+/Al at 25°C,find E° and E for the concentration cell expressed using shorthand notation below. Al(s) ∣ Al3+(1.0 × 10-5 M) ∣∣ Al3+(0.100 M) ∣ Al(s)

Correct AnswerverifiedShow Answer

What mass of aluminum can be plated onto an object in 755 minutes at 5.80 A of current?

Correct AnswerverifiedShow Answer

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Sn(s) ∣ Sn2+(aq,0.022 M) Ag+(aq,2.7 M) ∣ Ag(s)

Correct AnswerverifiedShow Answer

Match the following. -Q < K

Correct AnswerverifiedShow Answer

Give the criteria for a nonspontaneous reaction.

Correct AnswerverifiedShow Answer

Use the tabulated half-cell potentials below to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. 3 I2(s) + 2 Fe(s) → 2 Fe3+(aq) + 6 I⁻(aq)

Correct AnswerverifiedShow Answer

Use the tabulated half-cell potentials below to calculate ΔG° for the following redox reaction. 2 Al(s) + 3 Mg2+(aq) → 2 Al3+(aq) + 3 Mg(s)

Correct AnswerverifiedShow Answer

Give the type of battery that most cars contain.

Correct AnswerverifiedShow Answer

Balance the following redox reaction if it occurs in acidic solution.What are the coefficients in front of H2C2O4 and H2O in the balanced reaction? MnO4⁻(aq) + H2C2O4(aq) → Mn2+(aq) + CO2(g)

Correct AnswerverifiedShow Answer

Based on the following information, Cl2(g) + 2 e- → 2 Cl-(aq) E° = +1.36 V Mg2+(aq) + 2 e- → 2 Mg(s) E° = -2.37 V Which of the following chemical species is the strongest reducing agent?

Correct AnswerverifiedShow Answer

Identify oxidation.

Correct AnswerverifiedShow Answer

Match the following. -ΔG° < 0

Correct AnswerverifiedShow Answer

A voltaic cell is constructed with two Zn2+-Zn electrodes,where the half-reaction is Zn2+(aq) + 2e- → Zn(s) E° = -0.763 V The concentrations of zinc ion in the two compartments are 5.50 M and 1.11 × 10-2 M,respectively.The cell emf is ________ V.

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

How many seconds are required to produce 4.00 g of aluminum metal from the electrolysis of molten AlCl₃ with an electrical current of 12.0 A?

Correct Answer
verified

Correct Answer
verified

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Cu(s) ∣ Cu²⁺(aq,0.0032 M) ∣∣ Cu²⁺(aq,4.48 M) ∣ Cu(s)

Correct Answer
verified

What is the oxidizing agent in the redox reaction represented by the following cell notation? Sn(s) ∣ Sn²⁺(aq) ∣∣ Ag⁺(aq) ∣ Ag(s)

Correct Answer
verified

What is the balanced equation for the galvanic cell reaction expressed using shorthand notation below? Ni(s) ∣ Ni²⁺(aq) ∣∣ Cl₂(g) ∣ Cl^-(aq) ∣ C(s)

Correct Answer
verified

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. ) Mg(s) + Cu²⁺(aq) → Cu(s) + Mg²⁺(aq)

Correct Answer
verified

Given that E°_red = -1.66 V for Al³⁺/Al at 25°C,find E° and E for the concentration cell expressed using shorthand notation below. Al(s) ∣ Al³⁺(1.0 × 10^-5 M) ∣∣ Al³⁺(0.100 M) ∣ Al(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. Sn(s) ∣ Sn²⁺(aq,0.022 M) Ag⁺(aq,2.7 M) ∣ Ag(s)

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Use the tabulated half-cell potentials below to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. 3 I₂(s) + 2 Fe(s) → 2 Fe³⁺(aq) + 6 I⁻(aq)

Correct Answer
verified

Use the tabulated half-cell potentials below to calculate ΔG° for the following redox reaction. 2 Al(s) + 3 Mg²⁺(aq) → 2 Al³⁺(aq) + 3 Mg(s)

Correct Answer
verified

Correct Answer
verified

Balance the following redox reaction if it occurs in acidic solution.What are the coefficients in front of H₂C₂O₄and H₂O in the balanced reaction? MnO₄⁻(aq) + H₂C₂O₄(aq) → Mn²⁺(aq) + CO₂(g)

Correct Answer
verified

Based on the following information, Cl₂(g) + 2 e^- → 2 Cl^-(aq) E° = +1.36 V Mg²⁺(aq) + 2 e^- → 2 Mg(s) E° = -2.37 V Which of the following chemical species is the strongest reducing agent?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

A voltaic cell is constructed with two Zn²⁺-Zn electrodes,where the half-reaction is Zn²⁺(aq) + 2e^- → Zn(s) E° = -0.763 V The concentrations of zinc ion in the two compartments are 5.50 M and 1.11 × 10^-² M,respectively.The cell emf is ________ V.

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