What is E of the following cell reaction at 25°C? E°cell = 0.460 V.Cu(s)| Cu2+(0.020M)|| Ag+(0.16M)| Ag(s)

A) 0.463 V B) 0.282 V C) 0.460 V D) 0.487 V E) 0.467 V A) 0.463 V B) 0.282 V C) 0.460 V D) 0.487 V E) 0.467 V

In order to determine the identity of a particular transition metal (M),a voltaic cell is constructed at 25°C with the anode consisting of the transition metal as the electrode immersed in a solution of 0.0977 M M(NO3)2,and the cathode consisting of a copper electrode immersed in a 0.0724M Cu(NO3)2 solution.The two half-reactions are as follows: M(s) M2+(aq)+ 2e- Cu2+(aq)+ 2e- Cu(s) The potential measured across the cell is 1.13 V.What is the identity of the metal M? Reduction Half-Reaction E° (V) Cu2+(aq)+ 2e- Cu(s) +0.34 Ni2+(aq)+ 2e- Ni(s) -0.23 Cd2+(aq)+ 2e- Cd(s) - 0.40 Zn2+(aq)+ 2e- Zn(s)-0.76 Mn2+(aq)+ 2e- Mn(s) -1.18

A) Zn B) Ni C) Cu D) Cd E) Mn A) Zn B) Ni C) Cu D) Cd E) Mn

In order to determine the identity of a particular lanthanide metal (M),a voltaic cell is constructed at 25°C with the anode consisting of the lanthanide metal as the electrode immersed in a solution of 0.0467 M MCl3,and the cathode consisting of a copper electrode immersed in a 1.00 M Cu(NO3)2 solution.The two half-reactions are as follows: M(s) M3+(aq)+ 3e- Cu2+(aq)+ 2e- Cu(s) The potential measured across the cell is 2.70 V.What is the identity of the metal? Reduction Half-Reaction E° (V) Cu2+(aq)+ 2e- Cu(s)0.34 Ce3+(aq)+ 3e- Ce(s)-2.336 Tm3+(aq)+ 3e- Tm(s)-2.319 Eu3+(aq)+ 3e- Eu(s)-1.991 Gd3+(aq)+ 3e- Gd(s)-2.279 Sm3+(aq)+ 3e- Sm(s)-2.304

A) Tm B) Gd C) Ce D) Eu E) Sm A) Tm B) Gd C) Ce D) Eu E) Sm

Given: What is the cell potential at 25°C for the following cell? Cr(s)| Cr3+(0.010 M)|| Ag+(0.00025 M)| Ag(s)

A) 0.95 V B) 2.09 V C) 1.51 V D) 1.37 V E) 1.71 V A) 0.95 V B) 2.09 V C) 1.51 V D) 1.37 V E) 1.71 V

If the value of E°cell is 2.10 V for the reaction F2 (g)+ 2Fe2+ (aq)→ 2Fe3+ (aq)+ 2F- (aq), What is the value of E°cell for F- (aq)+ Fe3+ (aq)→ Fe2+ (aq)+ 1/2 F2(g)?

A) -4.20 V B) -1.05 V C) 2.10V D) 1.05 V E) -2.10V A) -4.20 V B) -1.05 V C) 2.10V D) 1.05 V E) -2.10V

Given: Ni2+(aq)+ 2e- Ni(s); E° = -0.23 V 2H+(aq)+ 2e- H2(g); E° = 0.00 VAg+(aq)+ e- Ag(s); E° = 0.80 V NO3-(aq)+ 4H+(aq)+ 3e- NO(g)+ 2H2O(l); E° = 0.96 V Which of the following statements is true?

A) Ni2+ reacts spontaneously with 1 M H+(aq)to form H2. B) Ni2+ reacts spontaneously with H2(g). C) Ag(s)reacts spontaneously with Ni2+. D) Ag(s)reacts spontaneously with 1 M NO3- in 1 M H+(aq). E) Ag(s)reacts spontaneously with 1 M H+(aq). A) Ni2+ reacts spontaneously with 1 M H+(aq)to form H2. B) Ni2+ reacts spontaneously with H2(g). C) Ag(s)reacts spontaneously with Ni2+. D) Ag(s)reacts spontaneously with 1 M NO3- in 1 M H+(aq). E) Ag(s)reacts spontaneously with 1 M H+(aq).

Given: Zn2+(aq)+ 2e- Zn(s); E° = -0.76 V 2H+(aq)+ 2e- H2(g); E° = 0.00 V I2(s)+ 2e- 2I-(aq); E° = 0.54 V Br2(l)+ 2e- 2Br-(aq); E° = 1.07 V Ni2+(aq)+ 2e- Ni(s); E° = -0.23 V Cu2+(aq)+ 2e- Cu(s); E° = 0.34 V Which of the following species will oxidize Ni but not Cu?

A) Zn2+ B) Br- C) H+ D) I2 E) Zn A) Zn2+ B) Br- C) H+ D) I2 E) Zn

Given: Zn2+(aq)+ 2e- Zn(s); E° = -0.76 V Co2+(aq)+ 2e- Co(s); E° = -0.28 V Sn2+(aq)+ 2e- Sn(s); E° = -0.15 V Pb2+(aq)+ 2e- Pb(s); E° = -0.13 V Fe3+(aq)+ e- Fe2+(aq); E° = 0.77 V Under standard-state conditions,which of the following pairs of elements or ions is capable of reducing Sn2+(aq)to Sn(s)?

A) Zn(s)or Co(s) B) Pb(s)or Fe2+(aq) C) Co(s)or Pb(s) D) Fe2+(aq)or Zn(s) E) Zn2+(aq)or Co2+(aq) A) Zn(s)or Co(s) B) Pb(s)or Fe2+(aq) C) Co(s)or Pb(s) D) Fe2+(aq)or Zn(s) E) Zn2+(aq)or Co2+(aq)

Exam 19: Electrochemistry

When the following oxidation-reduction reaction in basic solution is balanced,what is the lowest whole-number coefficient for OH^-,and on which side of the balanced equation should it appear? Cr₂O₃(s)→ Cr(OH)₂(aq)+ CrO₄^2-(aq)

(Multiple Choice)

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Question 81

Given: Pb²⁺ (aq)+ 2e^- Pb(s); Eº = -0.13 V What is the standard cell potential for the following reaction? 2Cr(s)+ 3Pb²⁺ (aq)→ 3Pb(s)+ 2Cr³⁺ (aq)

(Multiple Choice)

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Question 82

What is E of the following cell reaction at 25°C? E°_cell = 0.460 V.Cu(s)| Cu²⁺(0.020M)|| Ag⁺(0.16M)| Ag(s)

(Multiple Choice)

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Question 83

In a table of standard reduction potentials,the strongest reducing agents are the _ species in the half-reactions with the _ E° values.

(Multiple Choice)

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Question 84

For a reaction in a voltaic cell,both ΔH° and ΔS° are positive.Which of the following statements is true?

(Multiple Choice)

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Question 85

Which of the following statements is true concerning the hypthetical electrochemical cell depicted below? (M1 and M2 are differing metals) M1 | M1²⁺(aq)|| M2⁺(aq)| M2 M1²⁺(aq)+ 2e− M1(s); E° = -2.91 V M2²⁺(aq)+ e− M2(s); E° = -2.98 V

(Multiple Choice)

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Question 86

In order to determine the identity of a particular transition metal (M),a voltaic cell is constructed at 25°C with the anode consisting of the transition metal as the electrode immersed in a solution of 0.0977 M M(NO₃)₂,and the cathode consisting of a copper electrode immersed in a 0.0724M Cu(NO₃)₂ solution.The two half-reactions are as follows: M(s) M²⁺(aq)+ 2e^- Cu²⁺(aq)+ 2e^- Cu(s) The potential measured across the cell is 1.13 V.What is the identity of the metal M? Reduction Half-Reaction E° (V) Cu²⁺(aq)+ 2e^- Cu(s) +0.34 Ni²⁺(aq)+ 2e^- Ni(s) -0.23 Cd²⁺(aq)+ 2e^- Cd(s) - 0.40 Zn²⁺(aq)+ 2e^- Zn(s)-0.76 Mn²⁺(aq)+ 2e^- Mn(s) -1.18

(Multiple Choice)

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Question 87

Which of the following statements is true concerning the electrolysis of a 1.0 M aqueous solution of NaI? Reduction Half-Reaction E° (V) Na⁺(aq)+ e^- Na(s) -2.71 2H₂O(l)+ 2e^- H₂(g)+ 2OH^-(aq) -0.83 2H⁺(aq)+ 2e^- H₂(g) 0.00 I₂(s)+ 2e^- 2I^-(aq) 0.54 O₂(g)+ 4H⁺(aq)+ 4e^- 2H₂O(l) 1.23

(Multiple Choice)

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Question 88

In order to determine the identity of a particular lanthanide metal (M),a voltaic cell is constructed at 25°C with the anode consisting of the lanthanide metal as the electrode immersed in a solution of 0.0467 M MCl₃,and the cathode consisting of a copper electrode immersed in a 1.00 M Cu(NO₃)₂ solution.The two half-reactions are as follows: M(s) M³⁺(aq)+ 3e^- Cu²⁺(aq)+ 2e^- Cu(s) The potential measured across the cell is 2.70 V.What is the identity of the metal? Reduction Half-Reaction E° (V) Cu²⁺(aq)+ 2e^- Cu(s)0.34 Ce³⁺(aq)+ 3e^- Ce(s)-2.336 Tm³⁺(aq)+ 3e^- Tm(s)-2.319 Eu³⁺(aq)+ 3e^- Eu(s)-1.991 Gd³⁺(aq)+ 3e^- Gd(s)-2.279 Sm³⁺(aq)+ 3e^- Sm(s)-2.304

(Multiple Choice)

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Question 89

Given: What is the cell potential at 25°C for the following cell? Cr(s)| Cr³⁺(0.010 M)|| Ag⁺(0.00025 M)| Ag(s)

(Multiple Choice)

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Question 90

What is the balanced spontaneous reaction and standard cell potential of an electrochemical cell constructed from half cells with the following half reactions? Cu²⁺(aq)+ 2e¯ → Cu(s)E° = 0.337 V E° = -0.130 V

(Multiple Choice)

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Question 91

A _____ is a commercial electrochemical cell used to obtain sodium metal by the electrolysis of molten sodium chloride.

(Multiple Choice)

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Question 92

If the value of E°_cell is 2.10 V for the reaction F₂ (g)+ 2Fe²⁺ (aq)→ 2Fe³⁺ (aq)+ 2F^- (aq), What is the value of E°_cell for F^- (aq)+ Fe³⁺ (aq)→ Fe²⁺(aq)+ 1/2 F₂(g)?

(Multiple Choice)

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Question 93

If E°_cell for a certain reaction is 1 V (n = 4),and ΔS° is 11.2 J/(K⋅mol),what is ΔH° in units of J/mol at 25°C?

(Multiple Choice)

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Question 94

Balance the following oxidation-reduction occurring in acidic solution. MnO₄^-(aq)+ Co²⁺(aq)→ Mn²⁺(aq)+ Co³⁺(aq)

(Multiple Choice)

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Question 95

What is the cell reaction for the following electrochemical cell? Pt | Fe²⁺(aq),Fe³⁺(aq)|| Cr³⁺(aq)| Cr

(Multiple Choice)

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Question 96

Given: Ni²⁺(aq)+ 2e^- Ni(s); E° = -0.23 V 2H⁺(aq)+ 2e^- H₂(g); E° = 0.00 VAg⁺(aq)+ e^- Ag(s); E° = 0.80 V NO₃^-(aq)+ 4H⁺(aq)+ 3e^- NO(g)+ 2H₂O(l); E° = 0.96 V Which of the following statements is true?

(Multiple Choice)

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Question 97

Given: Zn²⁺(aq)+ 2e^- Zn(s); E° = -0.76 V 2H⁺(aq)+ 2e^- H₂(g); E° = 0.00 V I₂(s)+ 2e^- 2I^-(aq); E° = 0.54 V Br₂(l)+ 2e^- 2Br^-(aq); E° = 1.07 V Ni²⁺(aq)+ 2e^- Ni(s); E° = -0.23 V Cu²⁺(aq)+ 2e^- Cu(s); E° = 0.34 V Which of the following species will oxidize Ni but not Cu?

(Multiple Choice)

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Question 98

What is the cell notation for the voltaic cell shown below?

(Multiple Choice)

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Question 99

Given: Zn²⁺(aq)+ 2e^- Zn(s); E° = -0.76 V Co²⁺(aq)+ 2e^- Co(s); E° = -0.28 V Sn²⁺(aq)+ 2e^- Sn(s); E° = -0.15 V Pb²⁺(aq)+ 2e^- Pb(s); E° = -0.13 V Fe³⁺(aq)+ e^- Fe²⁺(aq); E° = 0.77 V Under standard-state conditions,which of the following pairs of elements or ions is capable of reducing Sn²⁺(aq)to Sn(s)?

(Multiple Choice)

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Question 100

Showing 81 - 100 of 122

When the following oxidation-reduction reaction in basic solution is balanced,what is the lowest whole-number coefficient for OH^-,and on which side of the balanced equation should it appear? Cr₂O₃(s)→ Cr(OH)₂(aq)+ CrO₄^2-(aq)

Given: Pb²⁺ (aq)+ 2e^- Pb(s); Eº = -0.13 V What is the standard cell potential for the following reaction? 2Cr(s)+ 3Pb²⁺ (aq)→ 3Pb(s)+ 2Cr³⁺ (aq)

What is E of the following cell reaction at 25°C? E°_cell = 0.460 V.Cu(s)| Cu²⁺(0.020M)|| Ag⁺(0.16M)| Ag(s)

In a table of standard reduction potentials,the strongest reducing agents are the _ species in the half-reactions with the _ E° values.

For a reaction in a voltaic cell,both ΔH° and ΔS° are positive.Which of the following statements is true?

Which of the following statements is true concerning the hypthetical electrochemical cell depicted below? (M1 and M2 are differing metals) M1 | M1²⁺(aq)|| M2⁺(aq)| M2 M1²⁺(aq)+ 2e− M1(s); E° = -2.91 V M2²⁺(aq)+ e− M2(s); E° = -2.98 V

Given: What is the cell potential at 25°C for the following cell? Cr(s)| Cr³⁺(0.010 M)|| Ag⁺(0.00025 M)| Ag(s)

What is the balanced spontaneous reaction and standard cell potential of an electrochemical cell constructed from half cells with the following half reactions? Cu²⁺(aq)+ 2e¯ → Cu(s)E° = 0.337 V E° = -0.130 V

A _____ is a commercial electrochemical cell used to obtain sodium metal by the electrolysis of molten sodium chloride.

If the value of E°_cell is 2.10 V for the reaction F₂ (g)+ 2Fe²⁺ (aq)→ 2Fe³⁺ (aq)+ 2F^- (aq), What is the value of E°_cell for F^- (aq)+ Fe³⁺ (aq)→ Fe²⁺(aq)+ 1/2 F₂(g)?

If E°_cell for a certain reaction is 1 V (n = 4),and ΔS° is 11.2 J/(K⋅mol),what is ΔH° in units of J/mol at 25°C?

Balance the following oxidation-reduction occurring in acidic solution. MnO₄^-(aq)+ Co²⁺(aq)→ Mn²⁺(aq)+ Co³⁺(aq)

What is the cell reaction for the following electrochemical cell? Pt | Fe²⁺(aq),Fe³⁺(aq)|| Cr³⁺(aq)| Cr

Given: Ni²⁺(aq)+ 2e^- Ni(s); E° = -0.23 V 2H⁺(aq)+ 2e^- H₂(g); E° = 0.00 VAg⁺(aq)+ e^- Ag(s); E° = 0.80 V NO₃^-(aq)+ 4H⁺(aq)+ 3e^- NO(g)+ 2H₂O(l); E° = 0.96 V Which of the following statements is true?

Given: Zn²⁺(aq)+ 2e^- Zn(s); E° = -0.76 V 2H⁺(aq)+ 2e^- H₂(g); E° = 0.00 V I₂(s)+ 2e^- 2I^-(aq); E° = 0.54 V Br₂(l)+ 2e^- 2Br^-(aq); E° = 1.07 V Ni²⁺(aq)+ 2e^- Ni(s); E° = -0.23 V Cu²⁺(aq)+ 2e^- Cu(s); E° = 0.34 V Which of the following species will oxidize Ni but not Cu?

What is the cell notation for the voltaic cell shown below?

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Exam 19: Electrochemistry

When the following oxidation-reduction reaction in basic solution is balanced,what is the lowest whole-number coefficient for OH-,and on which side of the balanced equation should it appear? Cr2O3(s)→ Cr(OH)2(aq)+ CrO42-(aq)

Given: Pb2+ (aq​)+ 2e- Pb(s); E​º = -0.13 V What is the standard cell potential for the following reaction? 2Cr(s)+ 3Pb2+ (​aq​)→ 3Pb(s​)+ 2Cr3+ (aq)

What is E of the following cell reaction at 25°C? E°cell = 0.460 V.Cu(s)| Cu2+(0.020M)|| Ag+(0.16M)| Ag(s)

In a table of standard reduction potentials,the strongest reducing agents are the _______ species in the half-reactions with the _______ E° values.

For a reaction in a voltaic cell,both ΔH° and ΔS° are positive.Which of the following statements is true?

Which of the following statements is true concerning the hypthetical electrochemical cell depicted below? (M1 and M2 are differing metals) M1 | M12+(aq)|| M2+(aq)| M2 M12+(aq)+ 2e− M1(s); E° = -2.91 V M22+(aq)+ e− M2(s); E° = -2.98 V

Which of the following statements is true concerning the electrolysis of a 1.0 M aqueous solution of NaI? Reduction Half-Reaction E° (V) Na+(aq)+ e- Na(s) -2.71 2H2O(l)+ 2e- H2(g)+ 2OH-(aq) -0.83 2H+(aq)+ 2e- H2(g) 0.00 I2(s)+ 2e- 2I-(aq) 0.54 O2(g)+ 4H+(aq)+ 4e- 2H2O(l) 1.23

Given: What is the cell potential at 25°C for the following cell? Cr(s)| Cr3+(0.010 M)|| Ag+(0.00025 M)| Ag(s)

What is the balanced spontaneous reaction and standard cell potential of an electrochemical cell constructed from half cells with the following half reactions? Cu2+(aq​)+ 2e¯ → Cu(s)E° = 0.337 V E° = -0.130 V

A _____ is a commercial electrochemical cell used to obtain sodium metal by the electrolysis of molten sodium chloride.

If the value of E°cell is 2.10 V for the reaction F2 (g)+ 2Fe2+ (aq​)→ 2Fe3+ (aq)+ 2F- (aq), What is the value of E°cell for F- (aq)+ Fe3+ (aq)→ Fe2+ (aq​)+ 1/2 F2(g)?

If E°cell for a certain reaction is 1 V (n = 4),and ΔS° is 11.2 J/(K⋅mol),what is ΔH° in units of J/mol at 25°C?

Balance the following oxidation-reduction occurring in acidic solution. MnO4-(aq)+ Co2+(aq)→ Mn2+(aq)+ Co3+(aq)

What is the cell reaction for the following electrochemical cell? Pt | Fe2+(aq),Fe3+(aq)|| Cr3+(aq)| Cr

Given: Ni2+(aq)+ 2e- Ni(s); E° = -0.23 V 2H+(aq)+ 2e- H2(g); E° = 0.00 VAg+(aq)+ e- Ag(s); E° = 0.80 V NO3-(aq)+ 4H+(aq)+ 3e- NO(g)+ 2H2O(l); E° = 0.96 V Which of the following statements is true?

Given: Zn2+(aq)+ 2e- Zn(s); E° = -0.76 V 2H+(aq)+ 2e- H2(g); E° = 0.00 V I2(s)+ 2e- 2I-(aq); E° = 0.54 V Br2(l)+ 2e- 2Br-(aq); E° = 1.07 V Ni2+(aq)+ 2e- Ni(s); E° = -0.23 V Cu2+(aq)+ 2e- Cu(s); E° = 0.34 V Which of the following species will oxidize Ni but not Cu?

What is the cell notation for the voltaic cell shown below?

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When the following oxidation-reduction reaction in basic solution is balanced,what is the lowest whole-number coefficient for OH^-,and on which side of the balanced equation should it appear? Cr₂O₃(s)→ Cr(OH)₂(aq)+ CrO₄^2-(aq)

Given: Pb²⁺ (aq)+ 2e^- Pb(s); Eº = -0.13 V What is the standard cell potential for the following reaction? 2Cr(s)+ 3Pb²⁺ (aq)→ 3Pb(s)+ 2Cr³⁺ (aq)

What is E of the following cell reaction at 25°C? E°_cell = 0.460 V.Cu(s)| Cu²⁺(0.020M)|| Ag⁺(0.16M)| Ag(s)

In a table of standard reduction potentials,the strongest reducing agents are the _ species in the half-reactions with the _ E° values.

Which of the following statements is true concerning the hypthetical electrochemical cell depicted below? (M1 and M2 are differing metals) M1 | M1²⁺(aq)|| M2⁺(aq)| M2 M1²⁺(aq)+ 2e− M1(s); E° = -2.91 V M2²⁺(aq)+ e− M2(s); E° = -2.98 V

Given: What is the cell potential at 25°C for the following cell? Cr(s)| Cr³⁺(0.010 M)|| Ag⁺(0.00025 M)| Ag(s)

What is the balanced spontaneous reaction and standard cell potential of an electrochemical cell constructed from half cells with the following half reactions? Cu²⁺(aq)+ 2e¯ → Cu(s)E° = 0.337 V E° = -0.130 V

If the value of E°_cell is 2.10 V for the reaction F₂ (g)+ 2Fe²⁺ (aq)→ 2Fe³⁺ (aq)+ 2F^- (aq), What is the value of E°_cell for F^- (aq)+ Fe³⁺ (aq)→ Fe²⁺(aq)+ 1/2 F₂(g)?

If E°_cell for a certain reaction is 1 V (n = 4),and ΔS° is 11.2 J/(K⋅mol),what is ΔH° in units of J/mol at 25°C?

Balance the following oxidation-reduction occurring in acidic solution. MnO₄^-(aq)+ Co²⁺(aq)→ Mn²⁺(aq)+ Co³⁺(aq)

What is the cell reaction for the following electrochemical cell? Pt | Fe²⁺(aq),Fe³⁺(aq)|| Cr³⁺(aq)| Cr

Given: Ni²⁺(aq)+ 2e^- Ni(s); E° = -0.23 V 2H⁺(aq)+ 2e^- H₂(g); E° = 0.00 VAg⁺(aq)+ e^- Ag(s); E° = 0.80 V NO₃^-(aq)+ 4H⁺(aq)+ 3e^- NO(g)+ 2H₂O(l); E° = 0.96 V Which of the following statements is true?

Given: Zn²⁺(aq)+ 2e^- Zn(s); E° = -0.76 V 2H⁺(aq)+ 2e^- H₂(g); E° = 0.00 V I₂(s)+ 2e^- 2I^-(aq); E° = 0.54 V Br₂(l)+ 2e^- 2Br^-(aq); E° = 1.07 V Ni²⁺(aq)+ 2e^- Ni(s); E° = -0.23 V Cu²⁺(aq)+ 2e^- Cu(s); E° = 0.34 V Which of the following species will oxidize Ni but not Cu?