What mass of Cu may be deposited from a Cu2+ solution during electrolysis by a current of 3.00 A for 10.0 hours?

A) 63.6 g Cu B) 35.6 g Cu C) 6.4 g Cu D) 3.6 g Cu E) 71.2 g Cu A) 63.6 g Cu B) 35.6 g Cu C) 6.4 g Cu D) 3.6 g Cu E) 71.2 g Cu

Consider the following balanced redox reaction. Mn2+(aq)+ S2O82-(aq)+ 2H2O(l)→ MnO2(s)+ 4H+(aq)+ 2SO42-(aq) Which of the following statements is true?

A) Mn2+(aq)is the oxidizing agent and is reduced. B) Mn2+ (aq)is the oxidizing agent and is oxidized. C) Mn2+ (aq)is the reducing agent and is oxidized. D) Mn2+ (aq)is the reducing agent and is reduced. E) Manganese does not change its oxidation number in this reaction. A) Mn2+(aq)is the oxidizing agent and is reduced. B) Mn2+ (aq)is the oxidizing agent and is oxidized. C) Mn2+ (aq)is the reducing agent and is oxidized. D) Mn2+ (aq)is the reducing agent and is reduced. E) Manganese does not change its oxidation number in this reaction.

A voltaic cell is prepared using copper and silver.Its cell notation is shown below. Cu(s)| Cu2+(aq)|| Ag+(aq)| Ag(s) Which reaction occurs at the cathode?

A) Cu(s)→ Cu2+(aq)+ 2e- B) Cu2+(aq)+ 2e- → Cu(s) C) Ag(s)→ Ag+(aq)+ e- D) Ag+(aq)+ e- → Ag(s) E) Cu(s)+ 2Ag+(aq)→ Cu2+(aq)+ 2Ag(s) A) Cu(s)→ Cu2+(aq)+ 2e- B) Cu2+(aq)+ 2e- → Cu(s) C) Ag(s)→ Ag+(aq)+ e- D) Ag+(aq)+ e- → Ag(s) E) Cu(s)+ 2Ag+(aq)→ Cu2+(aq)+ 2Ag(s)

Given Cu2+(aq)+ 2e- → Cu(s)E° = +0.34 V Al3+(aq)+ 3e- → Al(s)E° = -1.66 V Na+(aq)+ e- → Na(s)E° = -2.71 V Which of the following reactions will occur?

A) 2Na+(aq)+ Cu(s)→ Cu2+(aq)+ 2Na(s) B) Al(s)+ 3Na+(aq)→ Al3+(aq)+ 3Na(s) C) 2Na(s)+ Cu2+(aq)→ Cu(s)+ 2Na+(aq) D) 2Al3+(aq)+ 3Cu(s)→ 3Cu2+(aq)+ 2Al(s) E) None of the will occur. A) 2Na+(aq)+ Cu(s)→ Cu2+(aq)+ 2Na(s) B) Al(s)+ 3Na+(aq)→ Al3+(aq)+ 3Na(s) C) 2Na(s)+ Cu2+(aq)→ Cu(s)+ 2Na+(aq) D) 2Al3+(aq)+ 3Cu(s)→ 3Cu2+(aq)+ 2Al(s) E) None of the will occur.

Based on the data presented below,which is the strongest oxidizing agent? [PtCl4]2-(aq)+ 2e- Pt(s)+ 4Cl-(aq)E° = 0.755V RuO4(s)+ 8H+(aq)+ 8e- Ru(s)+ 4H2O(l)E° = 1.038V FeO42-(aq)+ 8H+(aq)+ 3e- Fe3+(aq)+4H2O(l)E° = 2.07 V H4XeO6(aq)+ 2H+(aq)+ 2e- XeO3(aq)+3H2O(l)E° = 2.42 V

A) [PtCl4]2-(aq) B) RuO4(s) C) HFeO4-(aq) D) H4XeO6(aq) E) Cl-(aq) A) [PtCl4]2-(aq) B) RuO4(s) C) HFeO4-(aq) D) H4XeO6(aq) E) Cl-(aq)

What is the cell potential at 25°C for the following reaction if [Zn2+] = 1.0 × 10-4 M and [Sn2+] = 0.20 M ? (R = 8.314 J/K • mol,F = 96,500 C • mol-1) Zn2+(aq)+ Sn(s)→ Zn(s)+ Sn2+(aq)E°cell = -0.62 V

A) -0.62 V B) +0.52 V C) -0.52 V D) -0.72 V E) +0.72 V A) -0.62 V B) +0.52 V C) -0.52 V D) -0.72 V E) +0.72 V

What is E°cell for the following reaction? 2Au(s)+ 3Ca2+(aq)→ 2Au3+(aq)+ 3Ca(s) Au3+(aq)+ 3e- → Au(s)E° = 1.50 V Ca2+ (aq)+ 2e- → Ca(s)E° = -2.87 V

A) -4.37 V B) -1.37 V C) -11.6 V D) 1.37 V E) 4.37 V A) -4.37 V B) -1.37 V C) -11.6 V D) 1.37 V E) 4.37 V

Two cells are connected in series,so that the same current flows through two electrodes,where the following half-reactions occur: Cu2+(aq)+ 2e- → Cu(s)and Ag+(aq)+ e- → Ag(s) For every 1.00 g of copper produced in the first process,how many grams of silver will be produced in the second one?

A) 0.294 g Ag B) 0.588 g Ag C) 0.850 g Ag D) 1.70 g Ag E) 3.40 g Ag A) 0.294 g Ag B) 0.588 g Ag C) 0.850 g Ag D) 1.70 g Ag E) 3.40 g Ag

Exam 19: Electrochemistry

When the following redox equation is balanced with the smallest whole number coefficients,what is the coefficient of Sb³⁺(aq)? BrO₃^-(aq)+ Sb³⁺(aq)→ Br^-(aq)+ Sb⁵⁺(aq) (acidic solution)

(Multiple Choice)

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Question 81

Which equation is correct?

(Multiple Choice)

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Question 82

What mass of Cu may be deposited from a Cu²⁺ solution during electrolysis by a current of 3.00 A for 10.0 hours?

(Multiple Choice)

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Question 83

Consider the following balanced redox reaction. Mn²⁺(aq)+ S₂O8^2-(aq)+ 2H₂O(l)→ MnO₂(s)+ 4H⁺(aq)+ 2SO₄^2-(aq) Which of the following statements is true?

(Multiple Choice)

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Question 84

Which metal is not capable of acting as a sacrificial anode when used with iron pipe?

(Multiple Choice)

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Question 85

A voltaic cell is prepared using copper and silver.Its cell notation is shown below. Cu(s)| Cu²⁺(aq)|| Ag⁺(aq)| Ag(s) Which reaction occurs at the cathode?

(Multiple Choice)

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Question 86

Which is the correct cell notation for the following reaction? Au³⁺(aq)+ Al(s)→ Al³⁺(aq)+ Au(s)

(Multiple Choice)

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Question 87

A galvanic cell is constructed using the two hypothetical half-reactions A + e^- → B E° = +1.50 V and C + 2e^- → D E° = -0.50 V a.Calculate the standard potential of this cell,E°_cell . b.Calculate ΔG° for the cell reaction.(1 faraday = 96,500 C)

(Short Answer)

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Question 88

Given Cu²⁺(aq)+ 2e^- → Cu(s)E° = +0.34 V Al³⁺(aq)+ 3e^- → Al(s)E° = -1.66 V Na⁺(aq)+ e^- → Na(s)E° = -2.71 V Which of the following reactions will occur?

(Multiple Choice)

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Question 89

Based on the data presented below,which is the strongest oxidizing agent? [PtCl₄]^2-(aq)+ 2e^- Pt(s)+ 4Cl^-(aq)E° = 0.755V RuO₄(s)+ 8H⁺(aq)+ 8e^- Ru(s)+ 4H₂O(l)E° = 1.038V FeO₄^2-(aq)+ 8H⁺(aq)+ 3e^- Fe³⁺(aq)+4H₂O(l)E° = 2.07 V H₄XeO₆(aq)+ 2H⁺(aq)+ 2e^- XeO₃(aq)+3H₂O(l)E° = 2.42 V

(Multiple Choice)

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Question 90

Complete and balance the following redox equation.Now sum the coefficients of all species in the balanced equation.(Remember to add the coefficients that are equal to one,and to add the coefficients of any species added to the equation.)The sum of the smallest whole number coefficients is Bi(OH)₃ + SnO₂^2- → Bi + SnO₃^2- (basic solution)

(Multiple Choice)

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Question 91

Which is the correct cell diagram for the following electrochemical cell? Half-Reaction E° (V) Sn²⁺(aq)+ 2e^- →Sn(s)-0.14 Fe²⁺(aq)+ 2e^- →Fe(s)-0.44

(Multiple Choice)

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Question 92

Lithium-ion batteries can be recharged many times.

(True/False)

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Question 93

What is the cell potential at 25°C for the following reaction if [Zn²⁺] = 1.0 × 10^-4 M and [Sn²⁺] = 0.20 M ? (R = 8.314 J/K • mol,F = 96,500 C • mol^-1) Zn²⁺(aq)+ Sn(s)→ Zn(s)+ Sn²⁺(aq)E°_cell = -0.62 V

(Multiple Choice)

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Question 94

What is E°_cell for the following reaction? 2Au(s)+ 3Ca²⁺(aq)→ 2Au³⁺(aq)+ 3Ca(s) Au³⁺(aq)+ 3e^- → Au(s)E° = 1.50 V Ca²⁺ (aq)+ 2e^- → Ca(s)E° = -2.87 V

(Multiple Choice)

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Question 95

Consider the reaction CuO(s)+ H₂(g)→ Cu(s)+ H₂O(l) In this reaction,which substances are the oxidizing agent and reducing agent, Respectively?

(Multiple Choice)

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Question 96

The redox reaction of peroxydisulfate with iodide has been used for many years as part of the iodine clock reaction.If E°_cell = 1.587 V and E° of the cathode half-cell is 0.536 V, what is E° of the anode half-cell? S₂O₈^2-(aq)+ 2H⁺ + 2I^-(aq)→ 2HSO₄^-(aq)+ I₂(aq)

(Multiple Choice)

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Question 97

Two cells are connected in series,so that the same current flows through two electrodes,where the following half-reactions occur: Cu²⁺(aq)+ 2e^- → Cu(s)and Ag⁺(aq)+ e^- → Ag(s) For every 1.00 g of copper produced in the first process,how many grams of silver will be produced in the second one?

(Multiple Choice)

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Question 98

What is the purpose of a salt bridge in an electrochemical cell?

(Multiple Choice)

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Question 99

What is E°_cell for the reaction of nickel(II)ions with cadmium metal at 25°C? (R = 8.314 J/K • mol,F = 96,500 C • mol^-1) Ni²⁺(aq)+ Cd(s) Cd²⁺(aq)+ Ni(s)K = 1.17 × 10⁵

(Multiple Choice)

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Question 100

Showing 81 - 100 of 122

Exam 19: Electrochemistry

When the following redox equation is balanced with the smallest whole number coefficients,what is the coefficient of Sb3+(aq)? BrO3-(aq)+ Sb3+(aq)→ Br-(aq)+ Sb5+(aq) (acidic solution)

Which equation is correct?

What mass of Cu may be deposited from a Cu2+ solution during electrolysis by a current of 3.00 A for 10.0 hours?

Consider the following balanced redox reaction. Mn2+(aq)+ S2O82-(aq)+ 2H2O(l)→ MnO2(s)+ 4H+(aq)+ 2SO42-(aq) Which of the following statements is true?

Which metal is not capable of acting as a sacrificial anode when used with iron pipe?

A voltaic cell is prepared using copper and silver.Its cell notation is shown below. Cu(s)| Cu2+(aq)|| Ag+(aq)| Ag(s) Which reaction occurs at the cathode?

Which is the correct cell notation for the following reaction? Au3+(aq)+ Al(s)→ Al3+(aq)+ Au(s)

A galvanic cell is constructed using the two hypothetical half-reactions A + e- → B E° = +1.50 V and C + 2e- → D E° = -0.50 V a.Calculate the standard potential of this cell,E°cell . b.Calculate ΔG° for the cell reaction.(1 faraday = 96,500 C)

Given Cu2+(aq)+ 2e- → Cu(s)E° = +0.34 V Al3+(aq)+ 3e- → Al(s)E° = -1.66 V Na+(aq)+ e- → Na(s)E° = -2.71 V Which of the following reactions will occur?

Based on the data presented below,which is the strongest oxidizing agent? [PtCl4]2-(aq)+ 2e- Pt(s)+ 4Cl-(aq)E° = 0.755V RuO4(s)+ 8H+(aq)+ 8e- Ru(s)+ 4H2O(l)E° = 1.038V FeO42-(aq)+ 8H+(aq)+ 3e- Fe3+(aq)+4H2O(l)E° = 2.07 V H4XeO6(aq)+ 2H+(aq)+ 2e- XeO3(aq)+3H2O(l)E° = 2.42 V

Which is the correct cell diagram for the following electrochemical cell? Half-Reaction E° (V) Sn2+(aq)+ 2e- →Sn(s)-0.14 Fe2+(aq)+ 2e- →Fe(s)-0.44

Lithium-ion batteries can be recharged many times.

What is the cell potential at 25°C for the following reaction if [Zn2+] = 1.0 × 10-4 M and [Sn2+] = 0.20 M ? (R = 8.314 J/K • mol,F = 96,500 C • mol-1) Zn2+(aq)+ Sn(s)→ Zn(s)+ Sn2+(aq)E°cell = -0.62 V

What is E°cell for the following reaction? 2Au(s)+ 3Ca2+(aq)→ 2Au3+(aq)+ 3Ca(s) Au3+(aq)+ 3e- → Au(s)E° = 1.50 V Ca2+ (aq)+ 2e- → Ca(s)E° = -2.87 V

Consider the reaction CuO(s)+ H2(g)→ Cu(s)+ H2O(l) In this reaction,which substances are the oxidizing agent and reducing agent, Respectively?

The redox reaction of peroxydisulfate with iodide has been used for many years as part of the iodine clock reaction.If E°cell = 1.587 V and E° of the cathode half-cell is 0.536 V, what is E° of the anode half-cell? S2O82-(aq)+ 2H+ + 2I-(aq)→ 2HSO4-(aq)+ I2(aq)

Two cells are connected in series,so that the same current flows through two electrodes,where the following half-reactions occur: Cu2+(aq)+ 2e- → Cu(s)and Ag+(aq)+ e- → Ag(s) For every 1.00 g of copper produced in the first process,how many grams of silver will be produced in the second one?

What is the purpose of a salt bridge in an electrochemical cell?

What is E°cell for the reaction of nickel(II)ions with cadmium metal at 25°C? (R = 8.314 J/K • mol,F = 96,500 C • mol-1) Ni2+(aq)+ Cd(s) Cd2+(aq)+ Ni(s)K = 1.17 × 105

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When the following redox equation is balanced with the smallest whole number coefficients,what is the coefficient of Sb³⁺(aq)? BrO₃^-(aq)+ Sb³⁺(aq)→ Br^-(aq)+ Sb⁵⁺(aq) (acidic solution)

What mass of Cu may be deposited from a Cu²⁺ solution during electrolysis by a current of 3.00 A for 10.0 hours?

Consider the following balanced redox reaction. Mn²⁺(aq)+ S₂O8^2-(aq)+ 2H₂O(l)→ MnO₂(s)+ 4H⁺(aq)+ 2SO₄^2-(aq) Which of the following statements is true?

A voltaic cell is prepared using copper and silver.Its cell notation is shown below. Cu(s)| Cu²⁺(aq)|| Ag⁺(aq)| Ag(s) Which reaction occurs at the cathode?

Which is the correct cell notation for the following reaction? Au³⁺(aq)+ Al(s)→ Al³⁺(aq)+ Au(s)

A galvanic cell is constructed using the two hypothetical half-reactions A + e^- → B E° = +1.50 V and C + 2e^- → D E° = -0.50 V a.Calculate the standard potential of this cell,E°_cell . b.Calculate ΔG° for the cell reaction.(1 faraday = 96,500 C)

Given Cu²⁺(aq)+ 2e^- → Cu(s)E° = +0.34 V Al³⁺(aq)+ 3e^- → Al(s)E° = -1.66 V Na⁺(aq)+ e^- → Na(s)E° = -2.71 V Which of the following reactions will occur?

Which is the correct cell diagram for the following electrochemical cell? Half-Reaction E° (V) Sn²⁺(aq)+ 2e^- →Sn(s)-0.14 Fe²⁺(aq)+ 2e^- →Fe(s)-0.44

What is the cell potential at 25°C for the following reaction if [Zn²⁺] = 1.0 × 10^-4 M and [Sn²⁺] = 0.20 M ? (R = 8.314 J/K • mol,F = 96,500 C • mol^-1) Zn²⁺(aq)+ Sn(s)→ Zn(s)+ Sn²⁺(aq)E°_cell = -0.62 V

What is E°_cell for the following reaction? 2Au(s)+ 3Ca²⁺(aq)→ 2Au³⁺(aq)+ 3Ca(s) Au³⁺(aq)+ 3e^- → Au(s)E° = 1.50 V Ca²⁺ (aq)+ 2e^- → Ca(s)E° = -2.87 V

Consider the reaction CuO(s)+ H₂(g)→ Cu(s)+ H₂O(l) In this reaction,which substances are the oxidizing agent and reducing agent, Respectively?

The redox reaction of peroxydisulfate with iodide has been used for many years as part of the iodine clock reaction.If E°_cell = 1.587 V and E° of the cathode half-cell is 0.536 V, what is E° of the anode half-cell? S₂O₈^2-(aq)+ 2H⁺ + 2I^-(aq)→ 2HSO₄^-(aq)+ I₂(aq)

What is E°_cell for the reaction of nickel(II)ions with cadmium metal at 25°C? (R = 8.314 J/K • mol,F = 96,500 C • mol^-1) Ni²⁺(aq)+ Cd(s) Cd²⁺(aq)+ Ni(s)K = 1.17 × 10⁵