Question 1

The standard emf for the cell using the overall cell reaction below is +2.20 V:
2Al(s) + 3I2(s) → 2Al3+(aq) + 6I-(aq) 
The emf generated by the cell when [Al3+] = 4.5 × 10-3 M and [I-] = 0.15 M is
2(s) → 2Al3+(aq) + 6I-(aq)  The emf generated by the cell when [Al3+] = 4.5 × 10-3 M and [I-] = 0.15 M is   A) 2.20 B) 2.32 C) 2.10 D) 2.39 E) 2.23" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  2.20
B)  2.32
C)  2.10
D)  2.39
E)  2.23

Question 2

What element is being oxidized in the following redox reaction?
Mg2+(aq) + NH4+(aq) → Mg(s) + NO3⁻(aq)

Accepted Answer

A)  Mg
B)  N
C)  H
D)  O

Question 3

Which of the following metal cations is the best oxidizing agent?

Accepted Answer

A)  Co2+
B)  Fe2+
C)  Fe3+
D)  Zn2+

Question 4

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C.
Fe(s) ∣ Fe3+(aq,0.0011 M) ∣∣ Fe3+(aq,2.33 M) ∣ Fe(s) 
3+(aq,0.0011 M) ∣∣ Fe3+(aq,2.33 M) ∣ Fe(s)    A) 0.066 V B) -0.036 V C) 0.00 V D) -0.099 V E) 0.20 V" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  0.066 V
B)  -0.036 V
C)  0.00 V
D)  -0.099 V
E)  0.20 V

Question 5

Balance the following redox reaction if it occurs in basic solution.What are the coefficients in front of Cr(OH) 4⁻ and ClO⁻ in the balanced reaction?
Cr(OH) 4⁻(aq) + ClO⁻(aq) → CrO42-(aq) + Cl⁻(aq)

Accepted Answer

A)  Cr(OH) 4⁻ = 2,ClO⁻ = 3
B)  Cr(OH) 4⁻ = 1,ClO⁻ = 1
C)  Cr(OH) 4⁻ = 1,ClO⁻ = 2
D)  Cr(OH) 4⁻ = 2,ClO⁻ = 6
E)  Cr(OH) 4⁻ = 6,ClO⁻ = 5

Question 6

What is the oxidizing agent in the redox reaction represented by the following cell notation?
Fe(s) ∣ Fe3+(aq) 3+(aq)  Cl2(g) ∣ Cl⁻(aq) ∣ Pt A) Fe(s)  B) Fe3+(aq)  C) Cl2(g)  D) Cl⁻(aq)  E) Pt" class="answers-bank-image d-inline" rel="preload" >Cl2(g) ∣ Cl⁻(aq) ∣ Pt

Accepted Answer

A)  Fe(s) 
B)  Fe3+(aq) 
C)  Cl2(g) 
D)  Cl⁻(aq) 
E)  Pt

Question 7

What element is being oxidized in the following redox reaction?
Cr(OH) 4⁻(aq) + ClO⁻(aq) → CrO42-(aq) + Cl⁻(aq)

Accepted Answer

A)  Cr
B)  O
C)  H
D)  Cl

Question 8

Consider the galvanic cell,Zn(s) ∣ Zn2+(aq) ∣∣ Pb2+(aq) ∣ Pb(s) .Which one of the following changes to the cell would cause the cell potential to increase (i.e. ,become more positive) ?

Accepted Answer

A)  increase the [Zn2+] concentration
B)  increase the [Pb2+] concentration
C)  increase the mass of Zn(s) 
D)  decrease the mass of Zn(s)

Question 9

Which of the following is the strongest oxidizing agent? 2(l)  B) Au3+(aq)  C) Ag(s)  D) Br⁻(aq)  E) Au(s) " class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

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

Question 10

Determine the cell notation for the redox reaction given below.
Pb(s) + 2 H⁺(aq) → Pb2+(aq) + H2(g)

Accepted Answer

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

Question 11

Balance the following redox reaction if it occurs in acidic solution.What are the coefficients in front of H⁺ and Fe3+ in the balanced reaction?
Fe2+(aq) + MnO4⁻(aq) → Fe3+(aq) + Mn2+(aq)

Accepted Answer

A)  H+ = 2,Fe3+ = 3
B)  H+ = 8,Fe3+ = 5
C)  H+ = 3,Fe3+ = 2
D)  H+ = 5,Fe3+ = 1
E)  H+ = 8,Fe3+ = 1

Question 12

A galvanic cell consists of one half-cell that contains Ag(s) and Ag+(aq) ,and one half-cell that contains Cu(s) and Cu2+(aq) .What species are produced at the electrodes under standard conditions?
Ag+(aq) + e- → Ag(s) E° = +0.80 V
Cu2+(aq) + 2 e- → Cu(s) E° = +0.34 V

Accepted Answer

A)  Ag(aq) is formed at the cathode and,Cu(s) is formed at the anode.
B)  Ag(s) is formed at the cathode,and Cu2+(aq) is formed at the anode.
C)  Cu(s) is formed at the cathode,and Ag+(aq) is formed at the anode.
D)  Cu2+(aq) is formed at the cathode,and Cu(s) is formed at the anode.

Question 13

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. ) 
Pb(s) + Br2(l) → Pb2+(aq) + 2 Br⁻(aq) 
2(l) → Pb2+(aq) + 2 Br⁻(aq)    A) 1.20 V B) 0.94 V C) -0.94 V D) -1.20 V E) -0.60 V" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  1.20 V
B)  0.94 V
C)  -0.94 V
D)  -1.20 V
E)  -0.60 V

Question 14

What is the difference between a voltaic cell and an electrolytic cell?

Accepted Answer

A voltaic cell contains a redox reaction...

Question 15

How many electrons are transferred in the following reaction? (The reaction is unbalanced. ) 
Mg(s) + Al3+(aq) → Al(s) + Mg2+(aq)

Accepted Answer

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

Question 16

Balance the following redox reaction if it occurs in basic solution.What are the coefficients in front of ClO2 and H2O in the balanced reaction?
H2O2(l) + ClO2(aq) → ClO2⁻(aq) + O2(g)

Accepted Answer

A)  ClO2 = 1,H2O = 1
B)  ClO2 = 1,H2O = 2
C)  ClO2 = 4,H2O = 3
D)  ClO2 = 4,H2O = 2
E)  ClO2 = 2,H2O = 2

Question 17

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

Accepted Answer

A)  Cd
B)  Cr
C)  Mn
D)  Ag
E)  Al

Question 18

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

Accepted Answer

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

Question 19

Which of the following is the weakest oxidizing agent? 2O2(aq)  B) Fe3+(aq)  C) ClO2(g)  D) I2(s)  E) Fe(s) " class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  H2O2(aq) 
B)  Fe3+(aq) 
C)  ClO2(g) 
D)  I2(s) 
E)  Fe(s)

Question 20

Use the tabulated half-cell potentials below to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C.
2 Al(s) + 3 Mg2+(aq) → 2 Al3+(aq) + 3 Mg(s) 
2+(aq) → 2 Al3+(aq) + 3 Mg(s)    A) 1.1 × 1072 B) 8.9 × 10-73 C) 1.1 × 10-72 D) 1.0 × 1024 E) 4.6 × 1031" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)  1.1 × 1072
B)  8.9 × 10-73
C)  1.1 × 10-72
D)  1.0 × 1024
E)  4.6 × 1031

Exam 18: Electrochemistry

How many electrons are transferred in the following reaction? (The reaction is unbalanced. ) Mg(s) + Al3+(aq) → Al(s) + Mg2+(aq)

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

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Balance the following redox reaction if it occurs in basic solution.What are the coefficients in front of Cr(OH) 4⁻ and ClO⁻ in the balanced reaction? Cr(OH) 4⁻(aq) + ClO⁻(aq) → CrO42-(aq) + Cl⁻(aq)

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What element is being oxidized in the following redox reaction? Cr(OH) 4⁻(aq) + ClO⁻(aq) → CrO42-(aq) + Cl⁻(aq)

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Which of the following is the strongest oxidizing agent?

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The standard emf for the cell using the overall cell reaction below is +2.20 V: 2Al(s) + 3I2(s) → 2Al3+(aq) + 6I-(aq) The emf generated by the cell when [Al3+] = 4.5 × 10-3 M and [I-] = 0.15 M is

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Which of the following is the weakest oxidizing agent?

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Balance the following redox reaction if it occurs in basic solution.What are the coefficients in front of ClO2 and H2O in the balanced reaction? H2O2(l) + ClO2(aq) → ClO2⁻(aq) + O2(g)

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What element is being oxidized in the following redox reaction? Mg2+(aq) + NH4+(aq) → Mg(s) + NO3⁻(aq)

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A galvanic cell consists of one half-cell that contains Ag(s) and Ag+(aq) ,and one half-cell that contains Cu(s) and Cu2+(aq) .What species are produced at the electrodes under standard conditions? Ag+(aq) + e- → Ag(s) E° = +0.80 V Cu2+(aq) + 2 e- → Cu(s) E° = +0.34 V

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Consider the galvanic cell,Zn(s) ∣ Zn2+(aq) ∣∣ Pb2+(aq) ∣ Pb(s) .Which one of the following changes to the cell would cause the cell potential to increase (i.e. ,become more positive) ?

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Determine the cell notation for the redox reaction given below. Pb(s) + 2 H⁺(aq) → Pb2+(aq) + H2(g)

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Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Fe(s) ∣ Fe3+(aq,0.0011 M) ∣∣ Fe3+(aq,2.33 M) ∣ Fe(s)

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

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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. ) Pb(s) + Br2(l) → Pb2+(aq) + 2 Br⁻(aq)

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Use the tabulated half-cell potentials below to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. 2 Al(s) + 3 Mg2+(aq) → 2 Al3+(aq) + 3 Mg(s)

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Which of the following metal cations is the best oxidizing agent?

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Balance the following redox reaction if it occurs in acidic solution.What are the coefficients in front of H⁺ and Fe3+ in the balanced reaction? Fe2+(aq) + MnO4⁻(aq) → Fe3+(aq) + Mn2+(aq)

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What is the oxidizing agent in the redox reaction represented by the following cell notation? Fe(s) ∣ Fe3+(aq) Cl2(g) ∣ Cl⁻(aq) ∣ Pt

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What is the difference between a voltaic cell and an electrolytic cell?

Correct AnswerverifiedA voltaic cell contains a redox reaction...View AnswerShow Answer

How many electrons are transferred in the following reaction? (The reaction is unbalanced. ) Mg(s) + Al³⁺(aq) → Al(s) + Mg²⁺(aq)

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

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Balance the following redox reaction if it occurs in basic solution.What are the coefficients in front of Cr(OH) ₄^⁻and ClO^⁻ in the balanced reaction? Cr(OH) ₄⁻(aq) + ClO⁻(aq) → CrO₄^2-(aq) + Cl⁻(aq)

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What element is being oxidized in the following redox reaction? Cr(OH) ₄⁻(aq) + ClO⁻(aq) → CrO₄^2-(aq) + Cl⁻(aq)

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Correct Answer
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The standard emf for the cell using the overall cell reaction below is +2.20 V: 2Al(s) + 3I₂(s) → 2Al³⁺(aq) + 6I^-(aq) The emf generated by the cell when [Al³⁺] = 4.5 × 10^-³ M and [I^-] = 0.15 M is

Correct Answer
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Correct Answer
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Balance the following redox reaction if it occurs in basic solution.What are the coefficients in front of ClO₂and H₂O in the balanced reaction? H₂O₂(l) + ClO₂(aq) → ClO₂⁻(aq) + O₂(g)

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What element is being oxidized in the following redox reaction? Mg²⁺(aq) + NH₄⁺(aq) → Mg(s) + NO₃⁻(aq)

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A galvanic cell consists of one half-cell that contains Ag(s) and Ag⁺(aq) ,and one half-cell that contains Cu(s) and Cu²⁺(aq) .What species are produced at the electrodes under standard conditions? Ag⁺(aq) + e^- → Ag(s) E° = +0.80 V Cu²⁺(aq) + 2 e^- → Cu(s) E° = +0.34 V

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Consider the galvanic cell,Zn(s) ∣ Zn²⁺(aq) ∣∣ Pb²⁺(aq) ∣ Pb(s) .Which one of the following changes to the cell would cause the cell potential to increase (i.e. ,become more positive) ?

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Determine the cell notation for the redox reaction given below. Pb(s) + 2 H⁺(aq) → Pb²⁺(aq) + H₂(g)

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Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Fe(s) ∣ Fe³⁺(aq,0.0011 M) ∣∣ Fe³⁺(aq,2.33 M) ∣ Fe(s)

Correct Answer
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Correct Answer
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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. ) Pb(s) + Br₂(l) → Pb²⁺(aq) + 2 Br⁻(aq)

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Use the tabulated half-cell potentials below to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. 2 Al(s) + 3 Mg²⁺(aq) → 2 Al³⁺(aq) + 3 Mg(s)

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Correct Answer
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Balance the following redox reaction if it occurs in acidic solution.What are the coefficients in front of H⁺and Fe³⁺ in the balanced reaction? Fe²⁺(aq) + MnO₄⁻(aq) → Fe³⁺(aq) + Mn²⁺(aq)

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What is the oxidizing agent in the redox reaction represented by the following cell notation? Fe(s) ∣ Fe³⁺(aq) Cl₂(g) ∣ Cl⁻(aq) ∣ Pt

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Correct Answer
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A voltaic cell contains a redox reaction...
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