Question 1

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. 
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 2

What is the reduction half-reaction for the following overall galvanic cell reaction? Co2+(aq)+ 2Ag(s)→ Co(s)+ 2 Ag+(aq)

Accepted Answer

A) Ag(s)+ e- → Ag+(aq) 
B) Ag+(aq)+ e- → Ag(s) 
C) Co2+(aq)+ 2 e- → Co(s) 
D) Co2+(aq)+ e- → Co(s) 
A) Ag(s)+ e- → Ag+(aq) 
B) Ag+(aq)+ e- → Ag(s) 
C) Co2+(aq)+ 2 e- → Co(s) 
D) Co2+(aq)+ e- → Co(s)

Question 3

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

Accepted Answer

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

Question 4

The standard cell potential (E°)of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn(s)+ 2H+(aq)→ Zn2+(aq)+ H2(g)
With   = 1.0 atm and [Zn2+] = 1.0 mol L-1, the cell potential is 0.66 V. The concentration of H+ in the cathode compartment is ________ mol L-1.

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 
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 5

How many electrons are transferred in the following reaction? (The reaction is unbalanced.) I2(s)+ Fe(s)→ Fe3+(aq)+ I⁻(aq)

Accepted Answer

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

Question 6

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-1 
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-1

Question 7

What element is being oxidized in the following (unbalanced)redox reaction? Zn2+(aq)+ NH4+(aq)→ Zn(s)+ NO3⁻(aq)

Accepted Answer

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

Question 8

Match the following.

-ΔrG° < 0

Accepted Answer

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

Question 9

Using the following standard reduction potentials, Fe3+(aq)+ e- →Fe2+(aq)E° = +0.77 V
Ni2+(aq)+ 2 e- →Ni(s)E° = -0.23 V
Calculate the standard cell potential for the galvanic cell reaction given below and determine whether or not this reaction is spontaneous under standard conditions.
Ni2+(aq)+ 2Fe2+(aq)→ 2Fe3+(aq)+ Ni(s)

Accepted Answer

A) E° = -1.00 V, nonspontaneous 
B) E° = -1.00 V, spontaneous 
C) E° = +1.00 V, nonspontaneous 
D) E° = +1.00 V, spontaneous 
A) E° = -1.00 V, nonspontaneous 
B) E° = -1.00 V, spontaneous 
C) E° = +1.00 V, nonspontaneous 
D) E° = +1.00 V, spontaneous

Question 10

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

Question 11

Predict the species that will be oxidized first if a mixture of molten salts containing the following ions undergoes electrolysis: Cu2+, Mg2+, Cl⁻, Br⁻, F⁻

Accepted Answer

A) Cl⁻ 
B) F⁻ 
C) Cu2+ 
D) Mg2+ 
E) Br⁻ 
A) Cl⁻ 
B) F⁻ 
C) Cu2+ 
D) Mg2+ 
E) Br⁻

Question 12

What is electrolysis?

Accepted Answer

An electrical curren

Question 13

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

Accepted Answer

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

Question 14

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C:
Sn(s)∣ Sn2+(aq, 1.8 mol L-1)   Ag+(aq, 0.055 mol L-1)∣ Ag(s)
E°(Sn2+/Sn)= -0.14 V and E°(Ag+/Ag)= +0.80 V

Accepted Answer

A) -0.94 V 
B) -0.85 V 
C) +1.02 V 
D) +0.98 V 
E) +0.86 V 
A) -0.94 V 
B) -0.85 V 
C) +1.02 V 
D) +0.98 V 
E) +0.86 V

Question 15

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 
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 16

Determine the cell notation for the redox reaction given below: Sn(s)+ 2Ag⁺(aq)→ Sn2+(aq)+ 2Ag(s)

Accepted Answer

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

Question 17

Sketch a voltaic cell that contains the following half reactions and label all relevant components.
Zn2+(aq)+ 2e⁻ → Zn(s) E°= -0.76 V
Cu2+(aq)+ 2e⁻ → Cu(s) E°= +0.34 V

Accepted Answer

The sketch

Question 18

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

Accepted Answer

Half-cell potentials (E°)are a

Question 19

Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of Zn and H+ in the balanced reaction? Zn2+(aq)+ NH4+(aq)→ Zn(s)+ NO3⁻(aq)

Accepted Answer

A) Zn = 1, H⁺ = 8 
B) Zn = 1, H⁺ = 4 
C) Zn = 4, H⁺ = 10 
D) Zn = 2, H⁺ = 4 
E) Zn = 3, H⁺ = 5 
A) Zn = 1, H⁺ = 8 
B) Zn = 1, H⁺ = 4 
C) Zn = 4, H⁺ = 10 
D) Zn = 2, H⁺ = 4 
E) Zn = 3, H⁺ = 5

Question 20

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 in voltage between 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. 
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 in voltage between 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.

Exam 18: Electrochemistry

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?

What is the reduction half-reaction for the following overall galvanic cell reaction? Co2+(aq)+ 2Ag(s)→ Co(s)+ 2 Ag+(aq)

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

The standard cell potential (E°)of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn(s)+ 2H+(aq)→ Zn2+(aq)+ H2(g) With = 1.0 atm and [Zn2+] = 1.0 mol L-1, the cell potential is 0.66 V. The concentration of H+ in the cathode compartment is ________ mol L-1.

How many electrons are transferred in the following reaction? (The reaction is unbalanced.) I2(s)+ Fe(s)→ Fe3+(aq)+ I⁻(aq)

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

What element is being oxidized in the following (unbalanced)redox reaction? Zn2+(aq)+ NH4+(aq)→ Zn(s)+ NO3⁻(aq)

Match the following. -ΔrG° < 0

Which of the following is the strongest oxidizing agent?

Predict the species that will be oxidized first if a mixture of molten salts containing the following ions undergoes electrolysis: Cu2+, Mg2+, Cl⁻, Br⁻, F⁻

What is electrolysis?

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

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: Sn(s)∣ Sn2+(aq, 1.8 mol L-1) Ag+(aq, 0.055 mol L-1)∣ Ag(s) E°(Sn2+/Sn)= -0.14 V and E°(Ag+/Ag)= +0.80 V

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)

Determine the cell notation for the redox reaction given below: Sn(s)+ 2Ag⁺(aq)→ Sn2+(aq)+ 2Ag(s)

Sketch a voltaic cell that contains the following half reactions and label all relevant components. Zn2+(aq)+ 2e⁻ → Zn(s) E°= -0.76 V Cu2+(aq)+ 2e⁻ → Cu(s) E°= +0.34 V

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

Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of Zn and H+ in the balanced reaction? Zn2+(aq)+ NH4+(aq)→ Zn(s)+ NO3⁻(aq)

Which of the following is TRUE about standard electrode potentials?

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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?

What is the reduction half-reaction for the following overall galvanic cell reaction? Co²⁺(aq)+ 2Ag(s)→ Co(s)+ 2 Ag⁺(aq)

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

The standard cell potential (E°)of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn(s)+ 2H⁺(aq)→ Zn²⁺(aq)+ H₂(g) With = 1.0 atm and [Zn²⁺] = 1.0 mol L^-1, the cell potential is 0.66 V. The concentration of H⁺ in the cathode compartment is ________ mol L^-1.

How many electrons are transferred in the following reaction? (The reaction is unbalanced.) I₂(s)+ Fe(s)→ Fe³⁺(aq)+ I⁻(aq)

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

What element is being oxidized in the following (unbalanced)redox reaction? Zn²⁺(aq)+ NH₄⁺(aq)→ Zn(s)+ NO₃⁻(aq)

Match the following. -Δ_rG° < 0

Predict the species that will be oxidized first if a mixture of molten salts containing the following ions undergoes electrolysis: Cu²⁺, Mg²⁺, Cl⁻, Br⁻, F⁻

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

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: Sn(s)∣ Sn²⁺(aq, 1.8 mol L^-1) Ag⁺(aq, 0.055 mol L^-1)∣ Ag(s) E°(Sn²⁺/Sn)= -0.14 V and E°(Ag⁺/Ag)= +0.80 V

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)

Determine the cell notation for the redox reaction given below: Sn(s)+ 2Ag⁺(aq)→ Sn²⁺(aq)+ 2Ag(s)

Sketch a voltaic cell that contains the following half reactions and label all relevant components. Zn²⁺(aq)+ 2e⁻ → Zn(s) E°= -0.76 V Cu²⁺(aq)+ 2e⁻ → Cu(s) E°= +0.34 V

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

Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of Znand H⁺ in the balanced reaction? Zn²⁺(aq)+ NH₄⁺(aq)→ Zn(s)+ NO₃⁻(aq)