Question 1

Which of the following is the strongest reducing agent?

Accepted Answer

A)   Al(s) 
B)   Zn(s) 
C)   Mg(s) 
D)   Al3+(aq) 
E)   Mg2+(aq)

Question 2

For a galvanic cell that uses the following two half-reactions, Cr2O72-(aq)  + 14H+(aq)  + 6 e- → 2Cr3+(aq)  + 7H2O(l) 
Pb(s)  → Pb2+(aq)  + 2 e-
How many moles of Pb(s)  are oxidized by three mol es of Cr2O72-?

Accepted Answer

A)   3
B)   6
C)   9
D)   18

Question 3

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) 
E°(Pb2+/Pb)  = -0.13 V and E°(Cu2+/Cu)  = +0.34 V

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 4

Which of the following reactions would have the smallest value of K at 298 K?

Accepted Answer

A)   A + B → C; E°cell = +1.22 V
B)   A + 2 B → C; E°cell = +0.98 V
C)   A + B → 2 C; E°cell = -0.030 V
D)   A + B → 3 C; E°cell = +0.15 V
E)   A + B → C; E°cell = -0.015 V

Question 5

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

Accepted Answer

A)   I-(aq)  + Zn2+(aq) ; if E°(I2/I-)  = + 0.54V and E°(Zn2+/Zn)  = -0.76V
B)   Ca(s)  + Mg2+(aq) ; if E°(Ca2+/Ca)  = -2.76V and E°(Mg2+/Mg)  = -2.37V
C)   H2(g)  + Cd2+(aq) ; if E°(Cd2+/Cd)  = -0.40V
D)   Ag(s)  + Sn2+(aq) ; if E°(Ag+/Ag)  = + 0.80V and E°(Sn2+/Sn)  = -0.14V
E)   Ag+(aq)  + Mn2+(aq) ; if E°(Ag+/Ag)  = + 0.80V and E°(MnO4-/Mn2+)  = +1.51V

Question 6

Calculate the cell potential for the following unbalanced reaction that takes place in an electrochemical cell at 25 °C when [ 2+/Mg)  = -2.37 V and E°(Fe3+/Fe)  = -0.036 V A)  +2.09 V B)  -3.18 V C)  +2.35 V D)  +0.36 V E)  -1.51 V" class="answers-bank-image d-inline" rel="preload" > ] = 0.500 M and [ 2+/Mg)  = -2.37 V and E°(Fe3+/Fe)  = -0.036 V A)  +2.09 V B)  -3.18 V C)  +2.35 V D)  +0.36 V E)  -1.51 V" class="answers-bank-image d-inline" rel="preload" > ] = 2.00 M Mg(s)  + 2+/Mg)  = -2.37 V and E°(Fe3+/Fe)  = -0.036 V A)  +2.09 V B)  -3.18 V C)  +2.35 V D)  +0.36 V E)  -1.51 V" class="answers-bank-image d-inline" rel="preload" > (aq)  → 2+/Mg)  = -2.37 V and E°(Fe3+/Fe)  = -0.036 V A)  +2.09 V B)  -3.18 V C)  +2.35 V D)  +0.36 V E)  -1.51 V" class="answers-bank-image d-inline" rel="preload" > (aq)  + Fe(s) 
E°(Mg2+/Mg)  = -2.37 V and E°(Fe3+/Fe)  = -0.036 V

Accepted Answer

A)   +2.09 V
B)   -3.18 V
C)   +2.35 V
D)   +0.36 V
E)   -1.51 V

Question 7

Calculate the cell potential for the following unbalanced reaction that takes place in an electrochemical cell at 25 °C when [ 2+/Mg)  = -2.37 V and E°(Fe3+/Fe)  = -0.036 V A)  +2.32 V B)  +2.30 V C)  -2.32 V D)  -2.30 V E)  +1.23 V" class="answers-bank-image d-inline" rel="preload" > ] = 0.914 M and [ 2+/Mg)  = -2.37 V and E°(Fe3+/Fe)  = -0.036 V A)  +2.32 V B)  +2.30 V C)  -2.32 V D)  -2.30 V E)  +1.23 V" class="answers-bank-image d-inline" rel="preload" > ] = 0.0230 M Mg(s)  + 2+/Mg)  = -2.37 V and E°(Fe3+/Fe)  = -0.036 V A)  +2.32 V B)  +2.30 V C)  -2.32 V D)  -2.30 V E)  +1.23 V" class="answers-bank-image d-inline" rel="preload" > (aq)  → 2+/Mg)  = -2.37 V and E°(Fe3+/Fe)  = -0.036 V A)  +2.32 V B)  +2.30 V C)  -2.32 V D)  -2.30 V E)  +1.23 V" class="answers-bank-image d-inline" rel="preload" > (aq)  + Fe(s) 
E°(Mg2+/Mg)  = -2.37 V and E°(Fe3+/Fe)  = -0.036 V

Accepted Answer

A)   +2.32 V
B)   +2.30 V
C)   -2.32 V
D)   -2.30 V
E)   +1.23 V

Question 8

Which of the following is the strongest oxidizing agent?

Accepted Answer

A)   MnO2(s) 
B)   Cl⁻(aq) 
C)   Cu⁺(aq) 
D)   SO42-(aq) 
E)   MnO4⁻(aq)

Question 9

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 10

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.)  2 Ag+(aq)  + Pb(s)  → 2Ag(s)  + Pb2+(aq) 
Ag+(aq)  + e- → Ag(s)  E°= 0.80 V
Pb2+(aq)  + 2 e- → Pb(s)  E°= -0.13 V

Accepted Answer

A)   +0.93 V
B)   +1.85 V
C)   -5.32 V
D)   +5.47 V
E)   +0.67 V

Question 11

If the standard reduction potential of Zn is -0.76 V, which of the following statements about a cell whose half-cells are Zn2+/Zn and SHE is correct?

Accepted Answer

A)   SHE will be the cell's cathode, Zn(s)  will be the cell's anode, and the measured cell potential will be 0.76 V.
B)   SHE will be the cell's anode, Zn(s)  will be the cell's cathode, and the measured cell potential will be 0.76 V.
C)   SHE will be the cell's cathode, Zn(s)  will be the cell's anode, and the measured cell potential will be -0.76 V.
D)   SHE will be the cell's cathode, Zn2+(aq)  will be the cell's anode, and the measured cell potential will be 0.76 V.
E)   H+(aq)  will be the cell's cathode, Zn2+(aq)  will be the cell's anode, and the measured cell potential will be 0.76 V.

Question 12

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

Accepted Answer

A)   H+(aq)  ∣ H2(g)  ∣ Pt(s)  2+(aq)  + H2(g)  
A)   H+(aq)  ∣ H2(g)  ∣ Pt(s)    Pb(s)  ∣ Pb2+(aq)  
B)   H2(g)  ∣ H+(aq)  ∣ Pt(s)    Pb2+(aq)  ∣ Pb(s)  
C)   Pb2+(aq)  ∣ Pb(s)    H2(g)  ∣ H+(aq)  ∣ Pt(s)  
D)   Pb(s)  ∣ Pb2+(aq)    H+(aq)  ∣ H2(g)  ∣ Pt(s)  
E)   Pb(s)  ∣ H2(g)    Pb2+(aq)  ∣ H+(aq)  ∣ Pt(s) " class="answers-bank-image d-inline" rel="preload" > Pb(s)  ∣ Pb2+(aq) 
B)   H2(g)  ∣ H+(aq)  ∣ Pt(s)  2+(aq)  + H2(g)  
A)   H+(aq)  ∣ H2(g)  ∣ Pt(s)    Pb(s)  ∣ Pb2+(aq)  
B)   H2(g)  ∣ H+(aq)  ∣ Pt(s)    Pb2+(aq)  ∣ Pb(s)  
C)   Pb2+(aq)  ∣ Pb(s)    H2(g)  ∣ H+(aq)  ∣ Pt(s)  
D)   Pb(s)  ∣ Pb2+(aq)    H+(aq)  ∣ H2(g)  ∣ Pt(s)  
E)   Pb(s)  ∣ H2(g)    Pb2+(aq)  ∣ H+(aq)  ∣ Pt(s) " class="answers-bank-image d-inline" rel="preload" > Pb2+(aq)  ∣ Pb(s) 
C)   Pb2+(aq)  ∣ Pb(s)  2+(aq)  + H2(g)  
A)   H+(aq)  ∣ H2(g)  ∣ Pt(s)    Pb(s)  ∣ Pb2+(aq)  
B)   H2(g)  ∣ H+(aq)  ∣ Pt(s)    Pb2+(aq)  ∣ Pb(s)  
C)   Pb2+(aq)  ∣ Pb(s)    H2(g)  ∣ H+(aq)  ∣ Pt(s)  
D)   Pb(s)  ∣ Pb2+(aq)    H+(aq)  ∣ H2(g)  ∣ Pt(s)  
E)   Pb(s)  ∣ H2(g)    Pb2+(aq)  ∣ H+(aq)  ∣ Pt(s) " class="answers-bank-image d-inline" rel="preload" > H2(g)  ∣ H+(aq)  ∣ Pt(s) 
D)   Pb(s)  ∣ Pb2+(aq)  2+(aq)  + H2(g)  
A)   H+(aq)  ∣ H2(g)  ∣ Pt(s)    Pb(s)  ∣ Pb2+(aq)  
B)   H2(g)  ∣ H+(aq)  ∣ Pt(s)    Pb2+(aq)  ∣ Pb(s)  
C)   Pb2+(aq)  ∣ Pb(s)    H2(g)  ∣ H+(aq)  ∣ Pt(s)  
D)   Pb(s)  ∣ Pb2+(aq)    H+(aq)  ∣ H2(g)  ∣ Pt(s)  
E)   Pb(s)  ∣ H2(g)    Pb2+(aq)  ∣ H+(aq)  ∣ Pt(s) " class="answers-bank-image d-inline" rel="preload" > H+(aq)  ∣ H2(g)  ∣ Pt(s) 
E)   Pb(s)  ∣ H2(g)  2+(aq)  + H2(g)  
A)   H+(aq)  ∣ H2(g)  ∣ Pt(s)    Pb(s)  ∣ Pb2+(aq)  
B)   H2(g)  ∣ H+(aq)  ∣ Pt(s)    Pb2+(aq)  ∣ Pb(s)  
C)   Pb2+(aq)  ∣ Pb(s)    H2(g)  ∣ H+(aq)  ∣ Pt(s)  
D)   Pb(s)  ∣ Pb2+(aq)    H+(aq)  ∣ H2(g)  ∣ Pt(s)  
E)   Pb(s)  ∣ H2(g)    Pb2+(aq)  ∣ H+(aq)  ∣ Pt(s) " class="answers-bank-image d-inline" rel="preload" > Pb2+(aq)  ∣ H+(aq)  ∣ Pt(s)

Question 13

Use the provided reduction potentials to calculate ΔrG° for the following balanced redox reaction: Pb2+(aq)  + Cu(s)  → Pb(s)  + Cu2+(aq) 
E°(Pb2+/Pb)  = -0.13 V and E°(Cu2+/Cu)  = +0.34 V

Accepted Answer

A)   -41 kJ mol-1
B)   -0.47 kJ mol-1
C)   +46 kJ mol-1
D)   +91 kJ mol-1
E)   -21 kJ mol-1

Question 14

The standard cell potential (E°)  of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn(s)  + -1, the cell potential is 0.45 V. The concentration of   in the cathode compartment is ________ mol L-1. A)  3.3 × 10-11 B)  2.4 × 10-3 C)  1.1 × 10-21 D)  0.73 E)  5.8 × 10-6" class="answers-bank-image d-inline" rel="preload" > (aq)  → -1, the cell potential is 0.45 V. The concentration of   in the cathode compartment is ________ mol L-1. A)  3.3 × 10-11 B)  2.4 × 10-3 C)  1.1 × 10-21 D)  0.73 E)  5.8 × 10-6" class="answers-bank-image d-inline" rel="preload" > (aq)  + -1, the cell potential is 0.45 V. The concentration of   in the cathode compartment is ________ mol L-1. A)  3.3 × 10-11 B)  2.4 × 10-3 C)  1.1 × 10-21 D)  0.73 E)  5.8 × 10-6" class="answers-bank-image d-inline" rel="preload" > (g) 
With -1, the cell potential is 0.45 V. The concentration of   in the cathode compartment is ________ mol L-1. A)  3.3 × 10-11 B)  2.4 × 10-3 C)  1.1 × 10-21 D)  0.73 E)  5.8 × 10-6" class="answers-bank-image d-inline" rel="preload" > = 1.0 atm and [ -1, the cell potential is 0.45 V. The concentration of   in the cathode compartment is ________ mol L-1. A)  3.3 × 10-11 B)  2.4 × 10-3 C)  1.1 × 10-21 D)  0.73 E)  5.8 × 10-6" class="answers-bank-image d-inline" rel="preload" > ] = 1.0 mol L-1, the cell potential is 0.45 V. The concentration of -1, the cell potential is 0.45 V. The concentration of   in the cathode compartment is ________ mol L-1. A)  3.3 × 10-11 B)  2.4 × 10-3 C)  1.1 × 10-21 D)  0.73 E)  5.8 × 10-6" class="answers-bank-image d-inline" rel="preload" > in the cathode compartment is ________ mol L-1.

Accepted Answer

A)   3.3 × 10-11
B)   2.4 × 10-3
C)   1.1 × 10-21
D)   0.73
E)   5.8 × 10-6

Question 15

What is undergoing oxidation 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)

Question 16

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 17

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.)  Pb2+(aq)  + Mg(s)  → Pb(s)  + Mg2+(aq) 
Mg2+(aq)  +2 e- →Mg(s)  E°= -2.37 V
Pb2+(aq)  + 2e- → Pb(s)  E°= -0.13 V

Accepted Answer

A)   +0.93 V
B)   +2.24 V
C)   -5.32 V
D)   +5.47 V
E)   +0.67 V

Question 18

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) 
Mg2+(aq)  + 2 e⁻ → Mg(s)  E° = -2.38 V
Cu2+(aq)  + 2 e⁻ → Cu(s)  E° = +0.34 V

Accepted Answer

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

Question 19

Match the following.
-Q = K

Accepted Answer

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

Question 20

The electrolysis of molten -3 B)  107 C)  321 D)  1.32 E)  35.7" class="answers-bank-image d-inline" rel="preload" > for 4.25 hr with an electrical current of 25.0 A produces -3 B)  107 C)  321 D)  1.32 E)  35.7" class="answers-bank-image d-inline" rel="preload" > of aluminum metal.

Accepted Answer

A)   9.90 × 10-3
B)   107
C)   321
D)   1.32
E)   35.7

Exam 18: Electrochemistry

Which of the following is the strongest oxidizing agent?

Correct Answer
verified

The electrolysis of molten for 4.25 hr with an electrical current of 25.0 A produces of aluminum metal.

Correct Answer
verified

Correct Answer
verified

Calculate the cell potential for the following unbalanced reaction that takes place in an electrochemical cell at 25 °C when [ ] = 0.500 M and [ ] = 2.00 M Mg(s) + (aq) → (aq) + Fe(s) E°(Mg²⁺/Mg) = -2.37 V and E°(Fe³⁺/Fe) = -0.036 V

Correct Answer
verified

Use the provided reduction potentials to calculate Δ_rG° for the following balanced redox reaction: Pb²⁺(aq) + Cu(s) → Pb(s) + Cu²⁺(aq) E°(Pb²⁺/Pb) = -0.13 V and E°(Cu²⁺/Cu) = +0.34 V

Correct Answer
verified

If the standard reduction potential of Zn is -0.76 V, which of the following statements about a cell whose half-cells are Zn²⁺/Zn and SHE is correct?

Correct Answer
verified

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

Correct Answer
verified

Correct Answer
verified

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

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

Correct Answer
verified

Which of the following is the strongest reducing agent?

Correct Answer
verified

Calculate the cell potential for the following unbalanced reaction that takes place in an electrochemical cell at 25 °C when [ ] = 0.914 M and [ ] = 0.0230 M Mg(s) + (aq) → (aq) + Fe(s) E°(Mg²⁺/Mg) = -2.37 V and E°(Fe³⁺/Fe) = -0.036 V

Correct Answer
verified

Match the following. -Q = K

Correct Answer
verified

For a galvanic cell that uses the following two half-reactions, Cr₂O₇^2-(aq) + 14H⁺(aq) + 6 e^- → 2Cr³⁺(aq) + 7H₂O(l) Pb(s) → Pb²⁺(aq) + 2 e^- How many moles of Pb(s) are oxidized by three mol es of Cr₂O₇^2-?

Correct Answer
verified

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

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) E°(Pb²⁺/Pb) = -0.13 V and E°(Cu²⁺/Cu) = +0.34 V

Correct Answer
verified

Which of the following reactions would have the smallest value of K at 298 K?

Correct Answer
verified

The standard cell potential (E°) of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn(s) + (aq) → (aq) + (g) With = 1.0 atm and [ ] = 1.0 mol L^-1, the cell potential is 0.45 V. The concentration of in the cathode compartment is ________ mol L^-1.

Correct Answer
verified

Correct Answer
verified

Exam 18: Electrochemistry

Which of the following is the strongest oxidizing agent?

Correct AnswerverifiedShow Answer

The electrolysis of molten for 4.25 hr with an electrical current of 25.0 A produces of aluminum metal.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Calculate the cell potential for the following unbalanced reaction that takes place in an electrochemical cell at 25 °C when [ ] = 0.500 M and [ ] = 2.00 M Mg(s) + (aq) → (aq) + Fe(s) E°(Mg2+/Mg) = -2.37 V and E°(Fe3+/Fe) = -0.036 V

Correct AnswerverifiedShow Answer

Use the provided reduction potentials to calculate ΔrG° for the following balanced redox reaction: Pb2+(aq) + Cu(s) → Pb(s) + Cu2+(aq) E°(Pb2+/Pb) = -0.13 V and E°(Cu2+/Cu) = +0.34 V

Correct AnswerverifiedShow Answer

If the standard reduction potential of Zn is -0.76 V, which of the following statements about a cell whose half-cells are Zn2+/Zn and SHE is correct?

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

Correct AnswerverifiedShow Answer

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

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

Correct AnswerverifiedShow Answer

Which of the following is the strongest reducing agent?

Correct AnswerverifiedShow Answer

Calculate the cell potential for the following unbalanced reaction that takes place in an electrochemical cell at 25 °C when [ ] = 0.914 M and [ ] = 0.0230 M Mg(s) + (aq) → (aq) + Fe(s) E°(Mg2+/Mg) = -2.37 V and E°(Fe3+/Fe) = -0.036 V

Correct AnswerverifiedShow Answer

Match the following. -Q = K

Correct AnswerverifiedShow Answer

For a galvanic cell that uses the following two half-reactions, Cr2O72-(aq) + 14H+(aq) + 6 e- → 2Cr3+(aq) + 7H2O(l) Pb(s) → Pb2+(aq) + 2 e- How many moles of Pb(s) are oxidized by three mol es of Cr2O72-?

Correct AnswerverifiedShow Answer

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

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) E°(Pb2+/Pb) = -0.13 V and E°(Cu2+/Cu) = +0.34 V

Correct AnswerverifiedShow Answer

Which of the following reactions would have the smallest value of K at 298 K?

Correct AnswerverifiedShow Answer

The standard cell potential (E°) of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn(s) + (aq) → (aq) + (g) With = 1.0 atm and [ ] = 1.0 mol L-1, the cell potential is 0.45 V. The concentration of in the cathode compartment is ________ mol L-1.

Correct AnswerverifiedShow Answer

Correct AnswerverifiedShow Answer

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

Calculate the cell potential for the following unbalanced reaction that takes place in an electrochemical cell at 25 °C when [ ] = 0.500 M and [ ] = 2.00 M Mg(s) + (aq) → (aq) + Fe(s) E°(Mg²⁺/Mg) = -2.37 V and E°(Fe³⁺/Fe) = -0.036 V

Correct Answer
verified

Use the provided reduction potentials to calculate Δ_rG° for the following balanced redox reaction: Pb²⁺(aq) + Cu(s) → Pb(s) + Cu²⁺(aq) E°(Pb²⁺/Pb) = -0.13 V and E°(Cu²⁺/Cu) = +0.34 V

Correct Answer
verified

If the standard reduction potential of Zn is -0.76 V, which of the following statements about a cell whose half-cells are Zn²⁺/Zn and SHE is correct?

Correct Answer
verified

Correct Answer
verified

Correct Answer
verified

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

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

Correct Answer
verified

Correct Answer
verified

Calculate the cell potential for the following unbalanced reaction that takes place in an electrochemical cell at 25 °C when [ ] = 0.914 M and [ ] = 0.0230 M Mg(s) + (aq) → (aq) + Fe(s) E°(Mg²⁺/Mg) = -2.37 V and E°(Fe³⁺/Fe) = -0.036 V

Correct Answer
verified

Correct Answer
verified

For a galvanic cell that uses the following two half-reactions, Cr₂O₇^2-(aq) + 14H⁺(aq) + 6 e^- → 2Cr³⁺(aq) + 7H₂O(l) Pb(s) → Pb²⁺(aq) + 2 e^- How many moles of Pb(s) are oxidized by three mol es of Cr₂O₇^2-?

Correct Answer
verified

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) E°(Pb²⁺/Pb) = -0.13 V and E°(Cu²⁺/Cu) = +0.34 V

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The standard cell potential (E°) of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn(s) + (aq) → (aq) + (g) With = 1.0 atm and [ ] = 1.0 mol L^-1, the cell potential is 0.45 V. The concentration of in the cathode compartment is ________ mol L^-1.

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