Question 1

Which of the following is the weakest reducing agent?

Accepted Answer

A)   Br2(s) 
B)   ClO2-(aq) 
C)   Sn(s) 
D)   I⁻(aq) 
E)   Au(s)

Question 2

The standard emf for the cell using the overall cell reaction below is +0.48 V: Zn(s) + Ni2+(aq) → Zn2+(aq) + Ni(s) 
The emf generated by the cell when [Ni2+] = 2.50 M and [Zn2+] = 0.100 M is 2+(aq) → Zn2+(aq) + Ni(s)  The emf generated by the cell when [Ni2+] = 2.50 M and [Zn2+] = 0.100 M is   A)  0.40 B)  0.50 C)  0.52 D)  0.56 E)  0.44" class="answers-bank-image d-inline" rel="preload" >

Accepted Answer

A)   0.40
B)   0.50
C)   0.52
D)   0.56
E)   0.44

Question 3

Why,if we multiply a reaction by 2,don't we multiply its E°red by 2?

Accepted Answer

Half-cell potentials (E°_red)are a...

Question 4

What is the reaction at the cathode in a breathalyzer?

Accepted Answer

A)   Ethanol is oxidized to acetic acid.
B)   Acetic acid is reduced to ethanol.
C)   Oxygen is reduced.
D)   Hydrogen is oxidized.
E)   Ethanol is oxidized to acetaldehyde.

Question 5

Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. Pb2+(aq) + Cu(s) → Pb(s) + Cu2+(aq)

Accepted Answer

A)   7.9 × 10-8
B)   8.9 × 107
C)   7.9 × 1015
D)   1.3 × 10-16
E)   1.1 × 10-8

Question 6

The standard cell potential (E°) of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn(s) + 2 H+(aq) → Zn2+(aq) + H2(g) 
With +(aq) → Zn2+(aq) + H2(g)  With   = 1.0 atm and [Zn2+] = 1.0 M,the cell potential is 0.66 V.The concentration of   in the cathode compartment is ________ M. A)  2.0 × 10-2 B)  4.2 × 10-4 C)  1.4 × 10-1 D)  4.9 × 101 E)  1.0 × 10-12" class="answers-bank-image d-inline" rel="preload" > = 1.0 atm and [Zn2+] = 1.0 M,the cell potential is 0.66 V.The concentration of +(aq) → Zn2+(aq) + H2(g)  With   = 1.0 atm and [Zn2+] = 1.0 M,the cell potential is 0.66 V.The concentration of   in the cathode compartment is ________ M. A)  2.0 × 10-2 B)  4.2 × 10-4 C)  1.4 × 10-1 D)  4.9 × 101 E)  1.0 × 10-12" class="answers-bank-image d-inline" rel="preload" > in the cathode compartment is ________ M.

Accepted Answer

A)   2.0 × 10-2
B)   4.2 × 10-4
C)   1.4 × 10-1
D)   4.9 × 101
E)   1.0 × 10-12

Question 7

What element is being oxidized in the following redox reaction? H2O2(l) + ClO2(aq) → ClO2-(aq) + O2(g)

Accepted Answer

A)   H
B)   O
C)   Cl
D)   N
E)   C

Question 8

Determine the cell notation for the redox reaction given below. Sn(s) + 2 H⁺(aq) → Sn2+(aq) + H2(g)

Accepted Answer

A)   H+(aq)  ∣ H2(g)  ∣ Pt 2+(aq) + H2(g)  
A)   H+(aq)  ∣ H2(g)  ∣ Pt   Sn(s)  ∣ Sn2+(aq)  
B)   H2(g)  ∣ H+(aq)  ∣ Pt   Sn2+(aq)  ∣ Sn(s)  
C)   Sn2+(aq)  ∣ Sn(s)    H2(g)  ∣ H+(aq)  ∣ Pt 
D)   Sn(s)  ∣ Sn2+(aq)    H+(aq)  ∣ H2(g)  ∣ Pt 
E)   Sn(s)  ∣ H2(g)    Sn2+(aq)  ∣ H+(aq)  ∣ Pt" class="answers-bank-image d-inline" rel="preload" > Sn(s)  ∣ Sn2+(aq) 
B)   H2(g)  ∣ H+(aq)  ∣ Pt 2+(aq) + H2(g)  
A)   H+(aq)  ∣ H2(g)  ∣ Pt   Sn(s)  ∣ Sn2+(aq)  
B)   H2(g)  ∣ H+(aq)  ∣ Pt   Sn2+(aq)  ∣ Sn(s)  
C)   Sn2+(aq)  ∣ Sn(s)    H2(g)  ∣ H+(aq)  ∣ Pt 
D)   Sn(s)  ∣ Sn2+(aq)    H+(aq)  ∣ H2(g)  ∣ Pt 
E)   Sn(s)  ∣ H2(g)    Sn2+(aq)  ∣ H+(aq)  ∣ Pt" class="answers-bank-image d-inline" rel="preload" > Sn2+(aq)  ∣ Sn(s) 
C)   Sn2+(aq)  ∣ Sn(s)  2+(aq) + H2(g)  
A)   H+(aq)  ∣ H2(g)  ∣ Pt   Sn(s)  ∣ Sn2+(aq)  
B)   H2(g)  ∣ H+(aq)  ∣ Pt   Sn2+(aq)  ∣ Sn(s)  
C)   Sn2+(aq)  ∣ Sn(s)    H2(g)  ∣ H+(aq)  ∣ Pt 
D)   Sn(s)  ∣ Sn2+(aq)    H+(aq)  ∣ H2(g)  ∣ Pt 
E)   Sn(s)  ∣ H2(g)    Sn2+(aq)  ∣ H+(aq)  ∣ Pt" class="answers-bank-image d-inline" rel="preload" > H2(g)  ∣ H+(aq)  ∣ Pt
D)   Sn(s)  ∣ Sn2+(aq)  2+(aq) + H2(g)  
A)   H+(aq)  ∣ H2(g)  ∣ Pt   Sn(s)  ∣ Sn2+(aq)  
B)   H2(g)  ∣ H+(aq)  ∣ Pt   Sn2+(aq)  ∣ Sn(s)  
C)   Sn2+(aq)  ∣ Sn(s)    H2(g)  ∣ H+(aq)  ∣ Pt 
D)   Sn(s)  ∣ Sn2+(aq)    H+(aq)  ∣ H2(g)  ∣ Pt 
E)   Sn(s)  ∣ H2(g)    Sn2+(aq)  ∣ H+(aq)  ∣ Pt" class="answers-bank-image d-inline" rel="preload" > H+(aq)  ∣ H2(g)  ∣ Pt
E)   Sn(s)  ∣ H2(g)  2+(aq) + H2(g)  
A)   H+(aq)  ∣ H2(g)  ∣ Pt   Sn(s)  ∣ Sn2+(aq)  
B)   H2(g)  ∣ H+(aq)  ∣ Pt   Sn2+(aq)  ∣ Sn(s)  
C)   Sn2+(aq)  ∣ Sn(s)    H2(g)  ∣ H+(aq)  ∣ Pt 
D)   Sn(s)  ∣ Sn2+(aq)    H+(aq)  ∣ H2(g)  ∣ Pt 
E)   Sn(s)  ∣ H2(g)    Sn2+(aq)  ∣ H+(aq)  ∣ Pt" class="answers-bank-image d-inline" rel="preload" > Sn2+(aq)  ∣ H+(aq)  ∣ Pt

Question 9

Consider the following standard reduction potentials, Ni2+(aq) + 2 e- → Ni(s) E° = -0.26 V
I2(s) + 2 e- → 2 I-(aq) E° = +0.54 V
Under standard conditions,

Accepted Answer

A)   Ni2+(aq)  is a stronger oxidizing agent than I2(s)  and I-(aq)  is a stronger reducing agent than Ni(s) .
B)   I2(s)  is a stronger oxidizing agent than Ni2+(aq)  and Ni(s)  is a stronger reducing agent than I-(aq) .
C)   Ni(s)  is a stronger oxidizing agent than I-(aq)  and Ni2+(aq)  is a stronger reducing agent than I2(s) .
D)   I-(aq)  is a stronger oxidizing agent than Ni(s)  and I2(s)  is a stronger reducing agent than Ni2+(aq) .

Question 10

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 11

Use the tabulated half-cell potentials 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)

Accepted Answer

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

Exam 19: Electrochemistry

What element is being oxidized in the following redox reaction? H₂O₂(l) + ClO₂(aq) → ClO₂^-(aq) + O₂(g)

Correct Answer
verified

Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. Pb²⁺(aq) + Cu(s) → Pb(s) + Cu²⁺(aq)

Correct Answer
verified

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)

Correct Answer
verified

The standard cell potential (E°) of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn(s) + 2 H⁺(aq) → Zn²⁺(aq) + H₂(g) With = 1.0 atm and [Zn²⁺] = 1.0 M,the cell potential is 0.66 V.The concentration of in the cathode compartment is ________ M.

Correct Answer
verified

Why,if we multiply a reaction by 2,don't we multiply its E°_red by 2?

Correct Answer
verified
Half-cell potentials (E°_red)are a...
View Answer

Consider the following standard reduction potentials, Ni²⁺(aq) + 2 e^- → Ni(s) E° = -0.26 V I₂(s) + 2 e^- → 2 I^-(aq) E° = +0.54 V Under standard conditions,

Correct Answer
verified

Use the tabulated half-cell potentials 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

What is the reaction at the cathode in a breathalyzer?

Correct Answer
verified

Determine the cell notation for the redox reaction given below. Sn(s) + 2 H⁺(aq) → Sn²⁺(aq) + H₂(g)

Correct Answer
verified

The standard emf for the cell using the overall cell reaction below is +0.48 V: Zn(s) + Ni²⁺(aq) → Zn²⁺(aq) + Ni(s) The emf generated by the cell when [Ni²⁺] = 2.50 M and [Zn²⁺] = 0.100 M is

Correct Answer
verified

Which of the following is the weakest reducing agent?

Correct Answer
verified

Exam 19: Electrochemistry

What element is being oxidized in the following redox reaction? H2O2(l) + ClO2(aq) → ClO2-(aq) + O2(g)

Correct AnswerverifiedShow Answer

Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. Pb2+(aq) + Cu(s) → Pb(s) + Cu2+(aq)

Correct AnswerverifiedShow Answer

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)

Correct AnswerverifiedShow Answer

The standard cell potential (E°) of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn(s) + 2 H+(aq) → Zn2+(aq) + H2(g) With = 1.0 atm and [Zn2+] = 1.0 M,the cell potential is 0.66 V.The concentration of in the cathode compartment is ________ M.

Correct AnswerverifiedShow Answer

Why,if we multiply a reaction by 2,don't we multiply its E°red by 2?

Correct AnswerverifiedHalf-cell potentials (E°red)are a...View AnswerShow Answer

Consider the following standard reduction potentials, Ni2+(aq) + 2 e- → Ni(s) E° = -0.26 V I2(s) + 2 e- → 2 I-(aq) E° = +0.54 V Under standard conditions,

Correct AnswerverifiedShow Answer

Use the tabulated half-cell potentials 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

What is the reaction at the cathode in a breathalyzer?

Correct AnswerverifiedShow Answer

Determine the cell notation for the redox reaction given below. Sn(s) + 2 H⁺(aq) → Sn2+(aq) + H2(g)

Correct AnswerverifiedShow Answer

The standard emf for the cell using the overall cell reaction below is +0.48 V: Zn(s) + Ni2+(aq) → Zn2+(aq) + Ni(s) The emf generated by the cell when [Ni2+] = 2.50 M and [Zn2+] = 0.100 M is

Correct AnswerverifiedShow Answer

Which of the following is the weakest reducing agent?

Correct AnswerverifiedShow Answer

What element is being oxidized in the following redox reaction? H₂O₂(l) + ClO₂(aq) → ClO₂^-(aq) + O₂(g)

Correct Answer
verified

Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. Pb²⁺(aq) + Cu(s) → Pb(s) + Cu²⁺(aq)

Correct Answer
verified

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)

Correct Answer
verified

The standard cell potential (E°) of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn(s) + 2 H⁺(aq) → Zn²⁺(aq) + H₂(g) With = 1.0 atm and [Zn²⁺] = 1.0 M,the cell potential is 0.66 V.The concentration of in the cathode compartment is ________ M.

Correct Answer
verified

Why,if we multiply a reaction by 2,don't we multiply its E°_red by 2?

Correct Answer
verified
Half-cell potentials (E°_red)are a...
View Answer

Consider the following standard reduction potentials, Ni²⁺(aq) + 2 e^- → Ni(s) E° = -0.26 V I₂(s) + 2 e^- → 2 I^-(aq) E° = +0.54 V Under standard conditions,

Correct Answer
verified

Use the tabulated half-cell potentials 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

Correct Answer
verified

Determine the cell notation for the redox reaction given below. Sn(s) + 2 H⁺(aq) → Sn²⁺(aq) + H₂(g)

Correct Answer
verified

The standard emf for the cell using the overall cell reaction below is +0.48 V: Zn(s) + Ni²⁺(aq) → Zn²⁺(aq) + Ni(s) The emf generated by the cell when [Ni²⁺] = 2.50 M and [Zn²⁺] = 0.100 M is

Correct Answer
verified

Correct Answer
verified