Determine E°cell for the reaction: Cl2 + 2 F- → 2 Cl- + F2. The half reactions are: F2(s) + 2 e- → 2 F-(aq) &emsp; E° = +2.866 V Cl2(s) + 2 e- → 2 Cl-(aq) &emsp; E° = 1.358 V

A) 3.016 V B) -4.224 V C) 1.508 V D) 4.224 V E) -1.508 V A) 3.016 V B) -4.224 V C) 1.508 V D) 4.224 V E) -1.508 V

For the reaction: Mg(s) + AgNO3(aq) → Ag(s) + Mg(NO3)2(aq) Ag+(aq) + e- → Ag(s) E° = 0.800 V Mg2+(aq) + 2 e- → Mg(s) E° = -2.356 V For the reaction, determine E° for the cell.

A) 1.556 V B) -3.156 V C) 3.156 V D) 0.800 V E) 2.356 V A) 1.556 V B) -3.156 V C) 3.156 V D) 0.800 V E) 2.356 V

For the reaction: Mg(s) + AgNO3(aq) → Ag(s) + Mg(NO3)2(aq) Ag+(aq) + e- → Ag(s) E° = 0.800 V Mg2+(aq) + 2 e- → Mg(s) E° = -2.356 V Estimate Keq at 25°C.

A) 5.7 × 10106 B) 2.0 × 1053 C) 3.7 × 1052 D) 1.1 × 1027 E) 10-107 A) 5.7 × 10106 B) 2.0 × 1053 C) 3.7 × 1052 D) 1.1 × 1027 E) 10-107

What is the cell potential for the following cell at 25°C? Zn ∣ Zn2+ (0.0456 M) || Cu2+(0.120 M) ∣ Cu Cu2+ + 2 e- → Cu(s) &emsp; E° = 0.340 V Zn2+ + 2 e- → Zn(s) &emsp; E° = -0.763 V

A) 1.088 V B) 1.114 V C) 1.106 V D) 1.094 V E) 1.129 V A) 1.088 V B) 1.114 V C) 1.106 V D) 1.094 V E) 1.129 V

Which of the following are commonly used as alternate standard electrodes: I. Ag(s) | AgCl(s) | Cl- (1.0 M) II. Hg(l) | HgCl2(s) | Cl- (1.0 M) III. Ag(s) | AgCl(s) | Cl- (0.1 M) IV. Hg(l) | Hg2Cl2(s) | Cl- (1.0 M) V. Hg(s) | Hg2Cl2(s) | Cl- (1.0 M)

A) I) and V) B) II) and IV) C) I) and IV) D) II) and III) E) I) and III) A) I) and V) B) II) and IV) C) I) and IV) D) II) and III) E) I) and III)

What is the cell potential for the following cell at 25°C? Al ∣ Al3+(0.00212 M) || Sn2+(0.435 M) ∣ Sn Al3+ + 3 e- → Al(s) &emsp; E° = -1.676 V Sn2+ + 2 e- → Sn(s &emsp; E° = -0.137 V

A) 1.517 V B) 1.668 V C) 1.410 V D) 1.497 V E) 1.581 V A) 1.517 V B) 1.668 V C) 1.410 V D) 1.497 V E) 1.581 V

In a zinc-lead cell the reaction is: Pb2+ + Zn → Pb + Zn2+ &emsp; &emsp; E° = 0.637 V Which of the following statements about this cell is FALSE?

A) The zinc electrode is the cathode. B) The reaction will go in the direction indicated. C) The shorthand notation is Zn ∣ Zn2+ = Pb2+ ∣ Pb D) The actual cell voltage is less than +0.637 volts because of concentration polarization and possible other factors. E) The lead electrode is positively charged. A) The zinc electrode is the cathode. B) The reaction will go in the direction indicated. C) The shorthand notation is Zn ∣ Zn2+ = Pb2+ ∣ Pb D) The actual cell voltage is less than +0.637 volts because of concentration polarization and possible other factors. E) The lead electrode is positively charged.

What is E° of the spontaneous cell made from the Zn2+/Zn (-0.76 V) and Br2/2Br- (1.07 V) half cells?

A) -1.83 V B) 0.31 V C) 1.83 V D) -0.31 V E) -0.76 V A) -1.83 V B) 0.31 V C) 1.83 V D) -0.31 V E) -0.76 V

Determine E°cell for the reaction: Pb + Zn2+ → Pb2+ + Zn. The half reactions are: Pb2+(aq) + 2 e- → Pb(s) &emsp; E° = -0.125 V Zn2+(aq) + 2 e- → Zn(s) &emsp; E° = -0.763 V

A) 0.638 V B) -0.638 V C) 0.888 V D) -1.276 V E) -0.888 V A) 0.638 V B) -0.638 V C) 0.888 V D) -1.276 V E) -0.888 V

For the reaction: Mg(s) + AgNO3(aq) → Ag(s) + Mg(NO3)2(aq) Ag+(aq) + e- → Ag(s) E° = 0.800 V Mg2+(aq) + 2 e- → Mg(s) E° = -2.356 V Determine ΔG°.

A) -300.3 kJ/mol B) 304.5 kJ/mol C) 609.0 kJ/mol D) -304.5 kJ/mol E) -609.0 kJ/mol A) -300.3 kJ/mol B) 304.5 kJ/mol C) 609.0 kJ/mol D) -304.5 kJ/mol E) -609.0 kJ/mol

What is Keq at 25°C of the spontaneous cell made from the Zn2+/Zn (-0.76 V) and Br2/2Br- (1.07 V) half cells?

A) 10-6 B) 105 C) 1010 D) 10-11 E) 1061 A) 10-6 B) 105 C) 1010 D) 10-11 E) 1061

What is the Ecell for the following cell at 25°C? Pt ∣ Fe2+ (0.0562 M), Fe3+ (0.253 M) || Ag+ (0.334 M) ∣ Ag Ag+ + e- → Ag(s)&emsp; &emsp; E° = 0.800 V Fe3+ + e- → Fe2+ &emsp; &emsp; E° = -0.771 V

A) -0.038 V B) 1.500 V C) -0.004 V D) 0.096 V E) 0.039 V A) -0.038 V B) 1.500 V C) -0.004 V D) 0.096 V E) 0.039 V

Exam 20: Electrochemistry

Determine E°cell for the reaction: Cl₂ + 2 F- → 2 Cl- + F₂. The half reactions are: F₂(s) + 2 e- → 2 F-(aq) E° = +2.866 V Cl₂(s) + 2 e- → 2 Cl-(aq) E° = 1.358 V

(Multiple Choice)

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Question 61

For the reaction: Mg(s) + AgNO₃(aq) → Ag(s) + Mg(NO₃)₂(aq) Ag⁺(aq) + e- → Ag(s) E° = 0.800 V Mg²⁺(aq) + 2 e- → Mg(s) E° = -2.356 V For the reaction, determine E° for the cell.

(Multiple Choice)

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Question 62

For the reaction: Mg(s) + AgNO₃(aq) → Ag(s) + Mg(NO₃)₂(aq) Ag⁺(aq) + e- → Ag(s) E° = 0.800 V Mg₂+(aq) + 2 e- → Mg(s) E° = -2.356 V Estimate Keq at 25°C.

(Multiple Choice)

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Question 63

Determine E°cell for the reaction: 2 Ag+ + Mg → 2 Ag + Mg2+. The half reactions are: Mg2+(aq) + 2 e- → Mg(s) E° = -2.356 V Ag+(aq) + e- → Ag(s) E° = 0.800 V

(Multiple Choice)

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Question 64

What is the cell potential for the following cell at 25°C? Zn ∣ Zn²⁺ (0.0456 M) || Cu²⁺(0.120 M) ∣ Cu Cu²⁺ + 2 e- → Cu(s) E° = 0.340 V Zn²⁺ + 2 e- → Zn(s) E° = -0.763 V

(Multiple Choice)

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Question 65

Which of the following are commonly used as alternate standard electrodes: I. Ag(s) | AgCl(s) | Cl- (1.0 M) II. Hg(l) | HgCl₂(s) | Cl- (1.0 M) III. Ag(s) | AgCl(s) | Cl- (0.1 M) IV. Hg(l) | Hg₂Cl₂(s) | Cl- (1.0 M) V. Hg(s) | Hg₂Cl₂(s) | Cl- (1.0 M)

(Multiple Choice)

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Question 66

What is the cell potential for the following cell at 25°C? Al ∣ Al³⁺(0.00212 M) || Sn²⁺(0.435 M) ∣ Sn Al³⁺ + 3 e- → Al(s) E° = -1.676 V Sn²⁺ + 2 e- → Sn(s E° = -0.137 V

(Multiple Choice)

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Question 67

In a zinc-lead cell the reaction is: Pb²⁺ + Zn → Pb + Zn²⁺ E° = 0.637 V Which of the following statements about this cell is FALSE?

(Multiple Choice)

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Question 68

What is E° of the spontaneous cell made from the Zn²⁺/Zn (-0.76 V) and Br₂/2Br- (1.07 V) half cells?

(Multiple Choice)

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Question 69

Corrosion of metals is an oxidation-reduction process.

(True/False)

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Question 70

For the following voltaic cell, determine the [Cl-] when PCl₂ = 0.500 atm, [Zn²⁺] = 1.77 × 10^-2 M, and Ecell = 2.250 V. The half-reactions at 25°C are: Cl₂(g) + 2 e- → 2 Cl-(aq) E° = +1.358 V Zn²⁺(aq) + 2 e- → Zn(s) E° = -0.763 V Zn(s) ∣ Zn²⁺(aq) || Cl-(aq), Cl₂(g) ∣ Pt(s)

(Multiple Choice)

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Question 71

Determine E°cell for the reaction: Pb + Zn²⁺ → Pb²⁺ + Zn. The half reactions are: Pb2+(aq) + 2 e- → Pb(s) E° = -0.125 V Zn²⁺(aq) + 2 e- → Zn(s) E° = -0.763 V

(Multiple Choice)

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Question 72

For the reaction: Mg(s) + AgNO₃(aq) → Ag(s) + Mg(NO₃)₂(aq) Ag⁺(aq) + e- → Ag(s) E° = 0.800 V Mg²⁺(aq) + 2 e- → Mg(s) E° = -2.356 V Determine ΔG°.

(Multiple Choice)

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Question 73

The Ecell for the following concentration cell at 25°C is 0.006. Pt ∣ H₂ (g, 0.025 atm) ∣ H⁺(0.012 M) = H⁺ (1 M) ∣ H₂ (g, 1 atm) ∣ Pt 2 H⁺(aq) + 2 e- → H₂(g) E° = 0. V

(True/False)

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Question 74

Consider the following reaction: 2 Al + 3 Ni2+ → 2 Al3+ + 3 Ni E° = 1.410 v What would be the cell potential at 25°C as calculated from the Nernst equation if [Ni2+] = 0.020 M, [Al3+] = 3.60 M?

(Multiple Choice)

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Question 75

Determine the Ksp at 25°C of AgCl(s). The half-reactions are: Ag⁺(aq) + 1 e- → Ag(s) E° = +0.771 V AgCl(s) + 1 e- → Ag(s) + Cl- E° = +0.222 V

(Multiple Choice)

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Question 76

What is Keq at 25°C of the spontaneous cell made from the Zn²⁺/Zn (-0.76 V) and Br₂/2Br- (1.07 V) half cells?

(Multiple Choice)

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Question 77

What is the Ecell for the following cell at 25°C? Pt ∣ Fe²⁺ (0.0562 M), Fe³⁺ (0.253 M) || Ag⁺ (0.334 M) ∣ Ag Ag⁺ + e- → Ag(s) E° = 0.800 V Fe³⁺ + e- → Fe₂⁺ E° = -0.771 V

(Multiple Choice)

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Question 78

In a galvanic cell, oxidation occurs at the:

(Multiple Choice)

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Question 79

Cathodic protection is attaching a more active metal to the protected metal.

(True/False)

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Question 80

Showing 61 - 80 of 103

Exam 20: Electrochemistry

Determine E°cell for the reaction: Cl2 + 2 F- → 2 Cl- + F2. The half reactions are: F2(s) + 2 e- → 2 F-(aq) E° = +2.866 V Cl2(s) + 2 e- → 2 Cl-(aq) E° = 1.358 V

For the reaction: Mg(s) + AgNO3(aq) → Ag(s) + Mg(NO3)2(aq) Ag+(aq) + e- → Ag(s) E° = 0.800 V Mg2+(aq) + 2 e- → Mg(s) E° = -2.356 V For the reaction, determine E° for the cell.

For the reaction: Mg(s) + AgNO3(aq) → Ag(s) + Mg(NO3)2(aq) Ag+(aq) + e- → Ag(s) E° = 0.800 V Mg2+(aq) + 2 e- → Mg(s) E° = -2.356 V Estimate Keq at 25°C.

Determine E°cell for the reaction: 2 Ag+ + Mg → 2 Ag + Mg2+. The half reactions are: Mg2+(aq) + 2 e- → Mg(s) E° = -2.356 V Ag+(aq) + e- → Ag(s) E° = 0.800 V

What is the cell potential for the following cell at 25°C? Zn ∣ Zn2+ (0.0456 M) || Cu2+(0.120 M) ∣ Cu Cu2+ + 2 e- → Cu(s) E° = 0.340 V Zn2+ + 2 e- → Zn(s) E° = -0.763 V

Which of the following are commonly used as alternate standard electrodes: I. Ag(s) | AgCl(s) | Cl- (1.0 M) II. Hg(l) | HgCl2(s) | Cl- (1.0 M) III. Ag(s) | AgCl(s) | Cl- (0.1 M) IV. Hg(l) | Hg2Cl2(s) | Cl- (1.0 M) V. Hg(s) | Hg2Cl2(s) | Cl- (1.0 M)

What is the cell potential for the following cell at 25°C? Al ∣ Al3+(0.00212 M) || Sn2+(0.435 M) ∣ Sn Al3+ + 3 e- → Al(s) E° = -1.676 V Sn2+ + 2 e- → Sn(s E° = -0.137 V

In a zinc-lead cell the reaction is: Pb2+ + Zn → Pb + Zn2+ E° = 0.637 V Which of the following statements about this cell is FALSE?

What is E° of the spontaneous cell made from the Zn2+/Zn (-0.76 V) and Br2/2Br- (1.07 V) half cells?

Corrosion of metals is an oxidation-reduction process.

For the following voltaic cell, determine the [Cl-] when PCl2 = 0.500 atm, [Zn2+] = 1.77 × 10-2 M, and Ecell = 2.250 V. The half-reactions at 25°C are: Cl2(g) + 2 e- → 2 Cl-(aq) E° = +1.358 V Zn2+(aq) + 2 e- → Zn(s) E° = -0.763 V Zn(s) ∣ Zn2+(aq) || Cl-(aq), Cl2(g) ∣ Pt(s)

Determine E°cell for the reaction: Pb + Zn2+ → Pb2+ + Zn. The half reactions are: Pb2+(aq) + 2 e- → Pb(s) E° = -0.125 V Zn2+(aq) + 2 e- → Zn(s) E° = -0.763 V

For the reaction: Mg(s) + AgNO3(aq) → Ag(s) + Mg(NO3)2(aq) Ag+(aq) + e- → Ag(s) E° = 0.800 V Mg2+(aq) + 2 e- → Mg(s) E° = -2.356 V Determine ΔG°.

The Ecell for the following concentration cell at 25°C is 0.006. Pt ∣ H2 (g, 0.025 atm) ∣ H+ (0.012 M) = H+ (1 M) ∣ H2 (g, 1 atm) ∣ Pt 2 H+(aq) + 2 e- → H2(g) E° = 0. V

Consider the following reaction: 2 Al + 3 Ni2+ → 2 Al3+ + 3 Ni E° = 1.410 v What would be the cell potential at 25°C as calculated from the Nernst equation if [Ni2+] = 0.020 M, [Al3+] = 3.60 M?

Determine the Ksp at 25°C of AgCl(s). The half-reactions are: Ag+(aq) + 1 e- → Ag(s) E° = +0.771 V AgCl(s) + 1 e- → Ag(s) + Cl- E° = +0.222 V

What is Keq at 25°C of the spontaneous cell made from the Zn2+/Zn (-0.76 V) and Br2/2Br- (1.07 V) half cells?

What is the Ecell for the following cell at 25°C? Pt ∣ Fe2+ (0.0562 M), Fe3+ (0.253 M) || Ag+ (0.334 M) ∣ Ag Ag+ + e- → Ag(s) E° = 0.800 V Fe3+ + e- → Fe2+ E° = -0.771 V

In a galvanic cell, oxidation occurs at the:

Cathodic protection is attaching a more active metal to the protected metal.

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Determine E°cell for the reaction: Cl₂ + 2 F- → 2 Cl- + F₂. The half reactions are: F₂(s) + 2 e- → 2 F-(aq) E° = +2.866 V Cl₂(s) + 2 e- → 2 Cl-(aq) E° = 1.358 V

For the reaction: Mg(s) + AgNO₃(aq) → Ag(s) + Mg(NO₃)₂(aq) Ag⁺(aq) + e- → Ag(s) E° = 0.800 V Mg²⁺(aq) + 2 e- → Mg(s) E° = -2.356 V For the reaction, determine E° for the cell.

For the reaction: Mg(s) + AgNO₃(aq) → Ag(s) + Mg(NO₃)₂(aq) Ag⁺(aq) + e- → Ag(s) E° = 0.800 V Mg₂+(aq) + 2 e- → Mg(s) E° = -2.356 V Estimate Keq at 25°C.

What is the cell potential for the following cell at 25°C? Zn ∣ Zn²⁺ (0.0456 M) || Cu²⁺(0.120 M) ∣ Cu Cu²⁺ + 2 e- → Cu(s) E° = 0.340 V Zn²⁺ + 2 e- → Zn(s) E° = -0.763 V

Which of the following are commonly used as alternate standard electrodes: I. Ag(s) | AgCl(s) | Cl- (1.0 M) II. Hg(l) | HgCl₂(s) | Cl- (1.0 M) III. Ag(s) | AgCl(s) | Cl- (0.1 M) IV. Hg(l) | Hg₂Cl₂(s) | Cl- (1.0 M) V. Hg(s) | Hg₂Cl₂(s) | Cl- (1.0 M)

What is the cell potential for the following cell at 25°C? Al ∣ Al³⁺(0.00212 M) || Sn²⁺(0.435 M) ∣ Sn Al³⁺ + 3 e- → Al(s) E° = -1.676 V Sn²⁺ + 2 e- → Sn(s E° = -0.137 V

In a zinc-lead cell the reaction is: Pb²⁺ + Zn → Pb + Zn²⁺ E° = 0.637 V Which of the following statements about this cell is FALSE?

What is E° of the spontaneous cell made from the Zn²⁺/Zn (-0.76 V) and Br₂/2Br- (1.07 V) half cells?

Determine E°cell for the reaction: Pb + Zn²⁺ → Pb²⁺ + Zn. The half reactions are: Pb2+(aq) + 2 e- → Pb(s) E° = -0.125 V Zn²⁺(aq) + 2 e- → Zn(s) E° = -0.763 V

For the reaction: Mg(s) + AgNO₃(aq) → Ag(s) + Mg(NO₃)₂(aq) Ag⁺(aq) + e- → Ag(s) E° = 0.800 V Mg²⁺(aq) + 2 e- → Mg(s) E° = -2.356 V Determine ΔG°.

The Ecell for the following concentration cell at 25°C is 0.006. Pt ∣ H₂ (g, 0.025 atm) ∣ H⁺(0.012 M) = H⁺ (1 M) ∣ H₂ (g, 1 atm) ∣ Pt 2 H⁺(aq) + 2 e- → H₂(g) E° = 0. V

Determine the Ksp at 25°C of AgCl(s). The half-reactions are: Ag⁺(aq) + 1 e- → Ag(s) E° = +0.771 V AgCl(s) + 1 e- → Ag(s) + Cl- E° = +0.222 V

What is Keq at 25°C of the spontaneous cell made from the Zn²⁺/Zn (-0.76 V) and Br₂/2Br- (1.07 V) half cells?

What is the Ecell for the following cell at 25°C? Pt ∣ Fe²⁺ (0.0562 M), Fe³⁺ (0.253 M) || Ag⁺ (0.334 M) ∣ Ag Ag⁺ + e- → Ag(s) E° = 0.800 V Fe³⁺ + e- → Fe₂⁺ E° = -0.771 V