Deck 18: Electrochemistry

Question 1

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

Answer 1

Cr(OH)₄^⁻ = 2,ClO⁻ = 3

Question 2

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

Answer 2

Ni(s)

Question 3

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

Answer 3

Al = 2,F₂ = 3

Question 4

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 5

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

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

Question 6

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

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

Question 7

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

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

Question 8

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 9

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 10

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

Question 11

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

Question 12

Identify oxidation.

A)increase in oxidation number
B)loss of electrons
C)gain of electrons
D)decrease in oxidation number
E)both A and B

Question 13

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

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

Question 14

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 15

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 16

Determine the cell notation for the redox reaction given below.
Sn(s)+ 2 Ag⁺(aq)→ Sn²⁺(aq)+ 2 Ag(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 17

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

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

Question 18

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

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

Question 19

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

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 20

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 21

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)+ 2 Ag⁺(aq)→ Sn²⁺(aq)+ 2 Ag(s)

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

Question 22

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

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

Question 23

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

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

Question 24

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

A)Pb²⁺(aq)+ Cu(s)
B)Ag⁺(aq)+ Br⁻(aq)
C)Li⁺(aq)+ Al(s)
D)Fe³⁺(aq)+ Ni(s)
E)None of the above pairs will react.

Question 25

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 26

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 27

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. )
3 Cl₂(g)+ 2 Fe(s)→ 6 Cl⁻(aq)+ 2 Fe³⁺(aq)

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

Question 28

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 K(s)+ I₂(s)→ 2 K⁺(aq)+ 2 I⁻(aq)

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

Question 29

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)

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

Question 30

What statement is not true about standard electrode potentials?

A)E°_cell is positive for spontaneous reactions.
B)Electrons will flow from more negative electrode to more positive electrode.
C)The electrode potential of the standard hydrogen electrode is exactly zero.
D)E°_cell is the difference in voltage between the anode and the cathode.
E)The electrode in any half-cell with a greater tendency to undergo reduction is positively charged relative to the standard hydrogen electrode and therefore has a positive E°.

Question 31

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 32

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)

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

Question 33

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

A)I^-(aq)+ Zn²⁺(aq)
B)Ca(s)+ Mg²⁺(aq)
C)H₂(g)+ Cd²⁺(aq)
D)Ag(s)+ Sn²⁺(aq)
E)All of the above pairs will react.

Question 34

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 35

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

Question 36

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 37

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 38

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 39

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

A)Sn⁴⁺(aq)+ Mg(s)
B)Cr³⁺(aq)+ Ni(s)
C)Zn(s)+ Na⁺(aq)
D)Fe(s)+ Ba²⁺(aq)
E)None of the above pairs will react.

Question 40

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 41

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C.
Sn(s)∣ Sn²⁺(aq,0.022 M)Ag⁺(aq,2.7 M)∣ Ag(s)

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

Question 42

Give the criteria for a nonspontaneous reaction.

A)ΔG° < 0,E°_cell > 0,K > 1
B)ΔG° > 0,E°_cell > 0,K > 1
C)ΔG° > 0,E°_cell < 0,K > 1
D)ΔG° < 0,E°_cell > 0,K < 1
E)ΔG° > 0,E°_cell < 0,K < 1

Question 43

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C.
Sn(s)∣ Sn²⁺(aq,1.8 M)∣∣ Ag⁺(aq,0.055 M)∣ Ag(s)

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

Question 44

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 45

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)

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

Question 46

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)More information is needed to determine.

Question 47

Give the criteria for a spontaneous reaction.

A)ΔG° < 0,E°_cell > 0,K > 1
B)ΔG° > 0,E°_cell > 0,K > 1
C)ΔG° > 0,E°_cell < 0,K > 1
D)ΔG° < 0,E°_cell > 0,K < 1
E)ΔG° > 0,E°_cell < 0,K < 1

Question 48

Use the tabulated half-cell potentials below to calculate ΔG° for the following redox reaction.
2 Al(s)+ 3 Mg²⁺(aq)→ 2 Al³⁺(aq)+ 3 Mg(s)

A)4.1 × 10² kJ
B)1.4 × 10² kJ
C)-2.3 × 10² kJ
D)-7.8 × 10² kJ
E)6.8 × 10² kJ

Question 49

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

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

Question 50

Which of the following metals will dissolve in HCl?

A)Ba
B)Na
C)Mg
D)Al
E)All of the above

Question 51

Use the tabulated half-cell potentials below to calculate ΔG° for the following balanced redox reaction.
3 I₂(s)+ 2 Fe(s)→ 2 Fe³⁺(aq)+ 6 I⁻(aq)

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

Question 52

Use the tabulated half-cell potentials below to calculate ΔG° for the following balanced redox reaction.
Pb²⁺(aq)+ Cu(s)→ Pb(s)+ Cu²⁺(aq)

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

Question 53

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)

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

Question 54

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

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

Question 55

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C.
Mg(s)∣ Mg²⁺(aq,2.74 M)∣∣ Cu²⁺(aq,0.0033 M)∣ Cu(s)

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

Question 56

Use the tabulated half-cell potentials below 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)

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

Question 57

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

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

Question 58

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 59

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)More information is needed to determine.

Question 60

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

A)Fe
B)Pb
C)Cu
D)Sn
E)Ni

Question 61

Explain the use of a salt bridge.

Question 62

Match the following.
Q > K

A)E_cell = E°_cell
B)E_cell = 0
C)E°_cell < 0
D)E_cell < 0
E)E°_cell > 0
F)E_cell > 0

Question 63

For the galvanic cell reaction,expressed below using shorthand notation,what half-reaction occurs at the cathode?
Zn(s)∣ Zn²⁺(aq)∣∣ Ni²⁺(aq)∣ Ni(s)

A)Zn(s)→ Zn²⁺(aq)+ 2 e^-
B)Zn²⁺(aq)+ 2 e^- → Zn(s)
C)Ni(s)→ Ni²⁺(aq)+ 2 e^-
D)Ni²⁺(aq)+ 2 e^- → Ni(s)

Question 64

What is the shorthand notation that represents the following galvanic cell reaction?
Pb(s)+ Cu(NO₃)₂(aq)→ Pb(NO₃)₂(aq)+ Cu(s)

A)Pb(s)∣ Pb²⁺(aq)∣∣ Cu²⁺(aq)∣ Cu(s)
B)Cu(s)∣ Cu²⁺(aq)∣∣ Pb²⁺(aq)∣ Pb(s)
C)Pb(s)∣ NO₃^-(aq)∣∣ NO₃^-(aq)∣ Cu(s)
D)Cu(s)∣ Cu(NO₃)₂(aq)∣∣ Pb(NO₃)₂(aq)∣ Pb(s)

Question 65

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

A)73.5 g
B)24.5 g
C)220.g
D)147 g
E)8.17 g

Question 66

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C.
Al(s)∣ Al³⁺(aq,0.115 M)∣∣ Al³⁺(aq,3.89 M)∣ Al(s)

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

Question 67

Explain the significance of the standard hydrogen electrode (SHE)in the tabulation of standard reduction potentials of other species.

Question 68

What is the reduction half-reaction for the following overall galvanic cell reaction?
Zn²⁺(aq)+ 2 Ag(s)→ Zn(s)+ 2 Ag⁺(aq)

A)Ag(s)+ e^- → Ag⁺(aq)
B)Ag⁺(aq)+ e^- → Ag(s)
C)Zn²⁺(aq)+ 2 e^- → Zn(s)
D)Zn²⁺(aq)+ e^- → Zn(s)

Question 69

Match the following.
Q = 1

A)E_cell = E°_cell
B)E_cell = 0
C)E°_cell < 0
D)E_cell < 0
E)E°_cell > 0
F)E_cell > 0

Question 70

Match the following.
Q < K

A)E_cell = E°_cell
B)E_cell = 0
C)E°_cell < 0
D)E_cell < 0
E)E°_cell > 0
F)E_cell > 0

Question 71

Match the following.
ΔG° > 0

A)E_cell = E°_cell
B)E_cell = 0
C)E°_cell < 0
D)E_cell < 0
E)E°_cell > 0
F)E_cell > 0

Question 72

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

Question 73

Give the type of battery that most cars contain.

A)lead-acid battery
B)dry-cell battery
C)alkaline battery
D)nickel-cadmium battery
E)nickel-metal hydride battery

Question 74

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

Question 75

Match the following.
ΔG° < 0

A)E_cell = E°_cell
B)E_cell = 0
C)E°_cell < 0
D)E_cell < 0
E)E°_cell > 0
F)E_cell > 0

Question 76

Nickel can be plated from aqueous solution according to the following half reaction.How long would it take (in minutes)to plate 29.6 g of nickel at 4.7 A?
Ni²⁺(aq)+ 2 e⁻ → Ni(s)

A)1.7 × 10² minutes
B)5.9 × 10² minutes
C)3.5 × 10² minutes
D)4.8 × 10² minutes
E)6.2 × 10² minutes

Question 77

Match the following.
Q = K

A)E_cell = E°_cell
B)E_cell = 0
C)E°_cell < 0
D)E_cell < 0
E)E°_cell > 0
F)E_cell > 0

Question 78

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C.
Cu(s)∣ Cu²⁺(aq,0.0032 M)∣∣ Cu²⁺(aq,4.48 M)∣ Cu(s)

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

Question 79

What mass of silver can be plated onto an object in 33.5 minutes at 8.70 A of current?
Ag⁺(aq)+ e⁻ → Ag(s)

A)19.6 g
B)0.326 g
C)9.78 g
D)3.07 g
E)0.102 g

Question 80

Why are iron nails coated with zinc?