Deck 18: Electrochemistry

Question 1

Identify the location of reduction in an electrochemical cell.

A)the anode
B)the cathode
C)the electrode
D)the salt bridge
E)the socket

Answer 1

the cathode

Question 2

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

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

Answer 2

O

Question 3

Balance the following redox reaction if it occurs in basic solution. What are the coefficients in front of Br₂ and OH⁻ in the balanced reaction? Br₂(l)→ BrO₃⁻(aq)+ Br⁻(aq)

A) Br₂ = 1, OH⁻ = 2
B) Br₂ = 2, OH⁻ = 5
C) Br₂ = 3, OH⁻ = 3
D) Br₂ = 3, OH⁻ = 6
E) Br₂ = 1, OH⁻ = 6

Answer 3

Br₂ = 3, OH⁻ = 6

Question 4

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

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

Question 5

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

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

Question 6

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

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

Question 7

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)

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 8

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)

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 9

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)

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 10

Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of Cd and Ag⁺ in the balanced reaction? Cd(s)+ Ag⁺(aq)→ Ag(s)+ Cd²⁺(aq)

A)Cd = 1, Ag⁺ = 2
B)Cd = 1, Ag⁺ = 1
C)Cd = 2, Ag⁺ = 1
D)Cd = 2, Ag⁺ = 2
E)Cd = 3, Ag⁺ = 1

Question 11

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

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

Question 12

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)

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 13

Which of the following statements is TRUE?

A)A reduction process corresponds to an increase in oxidation state as a result of loss of electrons.
B)An oxidation process involves the loss of electrons resulting in an increase in oxidation state.
C)An oxidation process corresponds to a decrease in oxidation state as a result of a gain of electrons.
D)During a reduction process electrons are lost, while during an oxidation they are gained.
E)During a reduction process an oxidation state increases, while in an oxidation process an oxidation state decreases.

Question 14

Determine the redox reaction represented by the following cell notation: Mg(s)∣ Mg²⁺(aq) Cu²⁺(aq)∣ Cu(s)

A)Cu(s)+ Mg²⁺(aq)→ Mg(s)+ Cu²⁺(aq)
B)Mg(s)+ Cu²⁺(aq)→ Cu(s)+ Mg²⁺(aq)
C)2Mg(s)+ Cu²⁺(aq)→ Cu(s)+ 2Mg²⁺(aq)
D)2Cu(s)+ Mg²⁺(aq)→ Mg(s)+ 2Cu²⁺(aq)
E)3Mg(s)+ 2Cu²⁺(aq)→ 2Cu(s)+ 3Mg²⁺(aq)

Question 15

Define a salt bridge.

A)A pathway, composed of salt water, that ions pass through.
B)A pathway in which no ions flow.
C)A pathway between the cathode and anode in which ions are reduced.
D)A pathway between the cathode and anode in which ions are oxidized.
E)A pathway through which counterions can flow between the half-cells without the solutions in the half-cell totally mixing.

Question 16

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)

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 17

Balance the following redox reaction if it occurs in basic solution. What are the coefficients in front of Al and F₂ in the balanced reaction? Al(s)+ F₂(g)→ Al³⁺(aq)+ F^-(aq)

A)Al = 2, F₂ = 3
B)Al = 2, F₂ = 6
C)Al = 1, F₂ = 1
D)Al = 2, F₂ = 1
E)Al = 3, F₂ = 2

Question 18

What element is being reduced in the following (unbalanced)redox reaction? MnO₄⁻ (aq)+ H₂C₂O₄(aq)→ Mn²⁺(aq)+ CO₂(g)

A)C
B)O
C)Mn
D)H

Question 19

Identify the location of oxidation in an electrochemical cell.

A)the anode
B)the cathode
C)the electrode
D)the salt bridge
E)the socket

Question 20

What element is being oxidized in the following (unbalanced)redox reaction? MnO₄⁻ (aq)+ H₂C₂O₄(aq)→ Mn²⁺(aq)+ CO₂(g)

A)C
B)O
C)Mn
D)H

Question 21

Which of the following is the weakest oxidizing agent?

A)Sn²⁺(aq)
B)Cr³⁺(aq)
C)Sn⁴⁺(aq)
D)Cr(s)
E)Sn(s)

Question 22

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

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

Question 23

Which of the following is the strongest oxidizing agent?

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

Question 24

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

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

Question 25

Which of the following is the weakest reducing agent?

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

Question 26

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

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

Question 27

Which of the following is the strongest reducing agent?

A)Sn²⁺(aq)
B)Cr³⁺(aq)
C)Sn⁴⁺(aq)
D)Cr(s)
E)Sn(s)

Question 28

Which of the following is the weakest reducing agent?

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

Question 29

Which of the following is the strongest reducing agent?

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

Question 30

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

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

Question 31

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

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

Question 32

Which of the following is the strongest reducing agent?

A)Na(s)
B)Li⁺(aq)
C)Ca(s)
D)Ca²⁺(aq)
E)Li(s)

Question 33

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

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 34

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

Question 35

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

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

Question 36

Which of the following is TRUE about standard electrode potentials?

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.

Question 37

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

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

Question 38

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

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

Question 39

Determine the cell notation for the redox reaction given below: 3Cl₂(g)+ 2Fe(s)→ 6Cl⁻(aq)+ 2Fe³⁺(aq)

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

Question 40

Which of the following is the strongest oxidizing agent?

A)MnO₂(s)
B)Cl⁻(aq)
C)Cu⁺(aq)
D)SO₄^2-(aq)
E)MnO₄⁻(aq)

Question 41

How many electrons are transferred in the following reaction? (The reaction is unbalanced.) Fe²⁺(aq)+ K(s)→ Fe(s)+ K⁺(aq)

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

Question 42

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

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

Question 43

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

A)Cd; E^o(Cd²⁺/Cd)= -0.40V
B)Cr; E^o(Cr³⁺/Cr)= -0.73V
C)Mn; E^o(Mn²⁺/Mn)= -1.18V
D)Ag; E^o(Ag⁺/Ag)= +0.80V
E)Al; E^o(Al³⁺/Al)= -1.66V

Question 44

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

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 45

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?

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 46

Identify the characteristics of a spontaneous reaction.

A)Δ_rG° > 0
B)ΔE°_cell < 0
C)K < 0
D)ΔE°_cell > 0
E)K = 0

Question 47

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

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

Question 48

Which of the following metals will dissolve in HCl?

A)Au; E^o(Au³⁺/Au)= -1.50V
B)Ag; E^o(Ag⁺/Ag)= +0.80V
C)Cu; E^o(Cu²⁺/Cu)= +0.34V
D)Al; E^o(Al³⁺/Al)= -1.66V
E)Pt; E^o(Pt²⁺/Pt)= +1.19V

Question 49

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.) 3Cl₂(g)+ 2Fe(s)→ 6Cl⁻(aq)+ 2Fe³⁺(aq)
Cl₂(g)+ 2 e⁻ → 2Cl⁻(aq)E° = +1.36 V
Fe³⁺(aq)+ 3 e⁻ → Fe(s)E° = -0.04 V

A)+4.16 V
B)-1.40 V
C)-1.32 V
D)+1.32 V
E)+1.40 V

Question 50

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

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

Question 51

Which of the following statements is true for the cell diagram below? Zn(s)∣ Zn²⁺(aq) Cu²⁺(aq)∣ Cu(s)

A)Zn is oxidized, Cu is reduced; the single vertical lines represent phase boundaries while the two vertical lines represent a salt bridge.
B)Zn²⁺is oxidized, Cu is reduced; the single vertical lines represent phase boundaries while the two vertical lines represent a salt bridge.
C)Zn is oxidized, Cu²⁺ is reduced; the single vertical lines represent phase boundaries while the two vertical lines represent a salt bridge.
D)Zn is oxidized, Cu²⁺ is reduced; the single vertical lines represent salt bridges while the two vertical lines represent a phase boundary.
E)Zn is reduced, Cu²⁺ is oxidized; the single vertical lines represent phase boundaries while the two vertical lines represent a salt bridge.

Question 52

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

A)Fe; E^o(Fe²⁺/Fe)= -0.45V
B)Pb; E^o(Pb²⁺/Pb)= -0.13V
C)Cu; E^o(Cu²⁺/Cu)= +0.34V
D)Sn; E^o(Sn²⁺/Sn)= -0.14V
E)Ni; E^o(Ni²⁺/Ni)= -0.23V

Question 53

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

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

Question 54

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

A)Sn⁴⁺(aq)+ Mg(s); if E^o(Sn⁴⁺/Sn²⁺)= +0.15V and E^o(Mg²⁺/Mg)= -2.37V
B)Cr³⁺(aq)+ Ni(s); if E^o(Cr³⁺/Cr)= -0.73V and E^o(Ni²⁺/Ni)= -0.23V
C)Zn(s)+ Na⁺(aq); if E^o(Zn²⁺/Zn)= -0.76V and E^o(Na⁺/Na)= -2.71V
D)Fe(s)+ Ba²⁺(aq); if E^o(Fe³⁺/Fe)= -0.04V and E^o(Ba²⁺/Ba)= -2.90V
E)Ni²⁺(aq)+ NO(g); if E^o(Ni²⁺/Ni)= -0.23V and E^o(NO₃^-/NO)= +0.96V

Question 55

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.) 2K(s)+ I₂(s)→ 2K⁺(aq)+ 2I⁻(aq)
K⁺(aq)+ e⁻ → K (s) E° = -2.93 V
I₂(s)+ 2 e⁻ → 2 I⁻(aq) E° = +0.54 V

A)+6.40 V
B)+1.85 V
C)-5.32 V
D)+3.47 V
E)+5.32 V

Question 56

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

A)Pb²⁺(aq)+ Cu(s); if E^o(Pb²⁺/Pb)= -0.13V and E^o(Cu²⁺/Cu)= +0.16V
B)Ag⁺(aq)+ Br⁻(aq); if E^o(Ag⁺/Ag)= 0.80V and E^o(Br₂/Br^-)= +1.09V
C)Li⁺(aq)+ Al(s); if E^o(Li⁺/Li)= -3.04V and E^o(Al³⁺/Al)= -1.66V
D)Fe³⁺(aq)+ Ni(s); if E^o(Fe³⁺/Fe)= -0.04V and E^o(Ni²⁺/Ni)= -0.23V
E)Cd²⁺(aq)+ I^-(aq); if E^o(Cd²⁺/Cd)= -0.40V and E^o(I₂/I^-)= + 0.54V

Question 57

Which of the following is the weakest oxidizing agent?

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

Question 58

Which of the following is the strongest oxidizing agent?

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

Question 59

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 2 5°C. (The equation is balanced.) Pb(s)+ Br₂(l)→ Pb²⁺(aq)+ 2 Br⁻(aq)
Pb²⁺(aq)+ 2 e⁻ → Pb(s) E° = -0.13 V
Br₂(l)+ 2 e⁻ → 2 Br⁻(aq)E° = +1.07 V

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

Question 60

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.) Sn(s)+ 2Ag⁺(aq)→ Sn²⁺(aq)+ 2Ag(s)
Sn²⁺(aq)+ 2 e⁻ → Sn(s) E° = -0.14 V
Ag⁺(aq)+ e⁻ → Ag(s) E° = +0.80 V

A)+1.74 V
B)+0.94 V
C)+1.08 V
D)-1.08 V
E)-1.74 V

Question 61

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

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 62

Identify the battery type that has a high overcharge tolerance.

A)NiCad battery
B)lithium-ion battery
C)nickel-metal hydride battery
D)lead-acid storage battery
E)zinc-manganese battery

Question 63

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C:
Sn(s)∣ Sn²⁺(aq, 0.022 mol L^-1) Ag⁺(aq, 2.7 mol L^-1)∣ Ag(s)
E°(Sn²⁺/Sn)= -0.14 V and E°(Ag⁺/Ag)= +0.80 V

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

Question 64

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C:
Mg(s)∣ Mg²⁺(aq, 2.74 mol L^-1) Cu²⁺(aq, 0.0033 mol L^-1)∣ Cu(s)
E°(Mg²⁺/Mg)= -2.37 V and E°(Cu²⁺/Cu)= +0.34 V

A)-2.80 V
B)+2.62 V
C)+2.71 V
D)+2.12 V
E)-1.94 V

Question 65

What is the reaction at the cathode in a breathalyzer?

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 66

Use the provided reduction potentials to calculate the equilibrium constant (K)for the following balanced redox reaction at 25 °C: 2Al(s)+ 3Mg²⁺(aq)→ 2Al³⁺(aq)+ 3Mg(s)
E°(Al³⁺/Al)= -1.66 V and E°(Mg²⁺/Mg)= -2.37 V

A)1.1 × 10⁷²
B)8.9 × 10^-70
C)9.7 × 10^-73
D)1.0 × 10²⁴
E)4.6 × 10³¹

Question 67

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

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

Question 68

Describe how water can be made to be a good conductor of electrical current.

A)use pure water
B)heat the water
C)add salt
D)chill the water
E)vaporize the water

Question 69

Identify the battery that is in most automobiles.

A)dry-cell battery
B)lithium-ion battery
C)lead-acid storage battery
D)NiCad battery
E)fuel cell

Question 70

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C:
Al(s)∣ Al³⁺(aq, 0.115 mol L^-1) Al³⁺(aq, 3.89 mol L^-1)∣ Al(s)
E°(Al³⁺/Al)= -1.66 V

A)+1.66 V
B)+0.060 V
C)0.00 V
D)+0.090 V
E)+0.030 V

Question 71

Identify the battery that is used as a common flashlight battery.

A)dry-cell battery
B)lithium-ion battery
C)lead-acid storage battery
D)NiCad battery
E)fuel cell

Question 72

Use the provided reduction potentials to calculate Δ_rG° for the following balanced redox reaction: 3I₂(s)+ 2Fe(s)→ 2Fe³⁺(aq)+ 6I⁻(aq)
E°(I₂/I^-)= + 0.54 V and E°(Fe³⁺/Fe)= -0.036 V

A)-1.1 × 10² kJ mol^-1
B)+4.9 × 10¹ kJ mol^-1
C)-9.7 × 10¹ kJ mol^-1
D)+2.3 × 10² kJ mol^-1
E)-3.3 × 10² kJ mol^-1

Question 73

Use the tabulated half-cell potentials to calculate the equilibrium constant (K)for the following balanced redox reaction at 25 °C: 3I₂(s)+ 2Fe(s)→ 2Fe³⁺(aq)+ 6I⁻(aq)
E°(I₂/I^-)= + 0.54 V and E°(Fe³⁺/Fe)= -0.036 V

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

Question 74

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °:
Fe(s)∣ Fe³⁺(aq, 0.0011 mol L^-1) Fe³⁺(aq, 2.33 mol L^-1)∣ Fe(s)
E°(Fe³⁺/Fe)= -0.036 V

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

Question 75

Identify the components of a fuel cell.

A)nickel-metal hydride
B)lithium-ion
C)hydrogen-oxygen
D)nickel-cadmium
E)zinc-manganese

Question 76

Which of the following reactions would be the most spontaneous at 298 K?

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

Question 77

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

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

Question 78

What is the reaction at the anode in a breathalyzer?

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 79

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

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 80

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

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