Calculate ΔrG° for the disproportionation reaction of copper(I)ion (Cu+)at 25 °C. 2 Cu+(aq)→ Cu2+(aq)+ Cu(s) The standard reduction potentials are as follows: Cu+(aq)+ e- → Cu(s) E° = +0.518 V Cu2+(aq)+ 2 e- → Cu(s) E° = +0.337 V

A) -165 kJ/mol⋅rxn B) -135 kJ/mol⋅rxn C) -34.9 kJ/mol⋅rxn D) +17.5 kJ/mol⋅rxn E) +135 kJ/mol⋅rxn A) -165 kJ/mol⋅rxn B) -135 kJ/mol⋅rxn C) -34.9 kJ/mol⋅rxn D) +17.5 kJ/mol⋅rxn E) +135 kJ/mol⋅rxn C

Calculate Ecell for the following electrochemical cell at 25 °C. Pt(s)| Fe3+(aq,0.100 M),Fe2+(aq,0.040 M)|| Cl-(aq,0.50 M)| AgCl(s)| Ag(s) The standard reduction potentials are as follows: AgCl(s)+ e- → Ag(s)+ Cl-(aq) E° = +0.222 V Fe3+(aq)+ e- → Fe2+(aq) E° = +0.771 V

A) -1.034 V B) -0.590 V C) -0.508 V D) -0.555 V E) +1.034 V A) -1.034 V B) -0.590 V C) -0.508 V D) -0.555 V E) +1.034 V D

Consider the following half-reactions. Cl2(g)+ 2 e- → 2 Cl-(aq) E° = +1.36 V Ag+(aq)+ e- → Ag(s) E° = +0.80 V Cu2+(aq)+ 2 e- → Cu(s) E° = +0.34 V Sn2+(aq)+ 2 e- → Sn(s) E° = -0.14 V Al3+(aq)+ 3 e- → Al(s) E° = -1.66 V Which of the following species will reduce Cu2+(aq)ion?

A) Ag(s)and Sn2+(aq) B) Cl-(aq)and Ag(s) C) Cl2(g)and Ag+(aq) D) Sn(s)and Al(s) E) Sn2+(aq)and Al3+(aq) A) Ag(s)and Sn2+(aq) B) Cl-(aq)and Ag(s) C) Cl2(g)and Ag+(aq) D) Sn(s)and Al(s) E) Sn2+(aq)and Al3+(aq) D

The standard reduction potentials for a reaction are as follows: Pb2+(aq)+ 2 e- → Pb(s) E° = -0.126 V PbSO4(s)+ 2 e- → Pb(s)+ SO42-(aq) E° = -0.355 V Calculate the Ksp for lead(II)sulfate (PbSO4)at 25 °C.

A) 3.4 × 10-28 B) 1.8 × 10-8 C) 5.6 × 10-5 D) 5.6 × 107 E) 2.9 × 1037 A) 3.4 × 10-28 B) 1.8 × 10-8 C) 5.6 × 10-5 D) 5.6 × 107 E) 2.9 × 1037

Which of the following statements is true concerning the electrochemical cell Zn(s)| Zn2+(aq,1.0 M)|| Ca2+(aq,1.0 M)| Ca(s) The standard reduction potentials are given follows: Zn2+(aq)+ 2 e− → Zn(s); E° = -0.76 V Ca2+(aq)+ 2 e− → Ca(s); E° = -2.87 V

A) The standard cell potential is -3.63 V. B) The standard cell potential is -2.11 V. C) The standard cell potential is -2.11 V.. D) The standard cell potential is -3.63 V.. E) The standard cell potential is 2.11 V. A) The standard cell potential is -3.63 V. B) The standard cell potential is -2.11 V. C) The standard cell potential is -2.11 V.. D) The standard cell potential is -3.63 V.. E) The standard cell potential is 2.11 V.

The value of E°cell is for the following reaction: Cl2(g)+ 2 Fe2+(aq)→ 2 Fe3+(aq)+ 2 Cl-(aq) Calculate the value of E°cell for the reaction below. Cl-(g)+ Fe3+(aq)→ Fe2+(aq)+ ½ Cl2(g)

A) -1.18 V B) -0.30 V C) 0.59 V D) 0.30 V E) -0.59 V A) -1.18 V B) -0.30 V C) 0.59 V D) 0.30 V E) -0.59 V

Exam 20: Principles of Chemical Reactivity: Electron Transfer Reactions

Calculate Δ_rG° for the disproportionation reaction of copper(I)ion (Cu⁺)at 25 °C. 2 Cu⁺(aq)→ Cu²⁺(aq)+ Cu(s) The standard reduction potentials are as follows: Cu⁺(aq)+ e^- → Cu(s) E° = +0.518 V Cu²⁺(aq)+ 2 e^- → Cu(s) E° = +0.337 V

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(Multiple Choice)

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Question 1

Correct Answer:

Verified

Calculate E_cell for the following electrochemical cell at 25 °C. Pt(s)| Fe³⁺(aq,0.100 M),Fe²⁺(aq,0.040 M)|| Cl^-(aq,0.50 M)| AgCl(s)| Ag(s) The standard reduction potentials are as follows: AgCl(s)+ e^- → Ag(s)+ Cl^-(aq) E° = +0.222 V Fe³⁺(aq)+ e^- → Fe²⁺(aq) E° = +0.771 V

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(Multiple Choice)

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Question 2

Correct Answer:

Verified

Consider the following half-reactions. Cl₂(g)+ 2 e^- → 2 Cl^-(aq) E° = +1.36 V Ag⁺(aq)+ e^- → Ag(s) E° = +0.80 V Cu²⁺(aq)+ 2 e^- → Cu(s) E° = +0.34 V Sn²⁺(aq)+ 2 e^- → Sn(s) E° = -0.14 V Al³⁺(aq)+ 3 e^- → Al(s) E° = -1.66 V Which of the following species will reduce Cu²⁺(aq)ion?

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Question 3

Correct Answer:

Verified

The standard reduction potentials for a reaction are as follows: Pb²⁺(aq)+ 2 e^- → Pb(s) E° = -0.126 V PbSO₄(s)+ 2 e^- → Pb(s)+ SO₄^2-(aq) E° = -0.355 V Calculate the K_sp for lead(II)sulfate (PbSO₄)at 25 °C.

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Question 4

Which of the following statements is true concerning the electrochemical cell Zn(s)| Zn²⁺(aq,1.0 M)|| Ca²⁺(aq,1.0 M)| Ca(s) The standard reduction potentials are given follows: Zn²⁺(aq)+ 2 e− → Zn(s); E° = -0.76 V Ca²⁺(aq)+ 2 e− → Ca(s); E° = -2.87 V

(Multiple Choice)

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Question 5

The cell potential of the following electrochemical cell is determined by using an unspecified concentration of acid.Calculate the pH of the acid solution,given that the measured cell potential is -0.431 V and the anode reduction potential (E°)is 0.222 V at 25 °C. Ag(s)| AgCl(s)| Cl−(aq,1.0 M)|| H⁺(aq)| H₂(g,1.0 atm)| Pt(s)

(Multiple Choice)

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Question 6

One Faraday is defined as the:

(Multiple Choice)

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Question 7

Which of the following statements is true for electron transfer reactions?

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Question 8

Calculate the value of the equilibrium constant (K)at 25 °C for the following cell reaction: Sn(s)+ Pb²⁺(aq)→ Sn²⁺(aq)+ Pb(s); E°_cell= 0.014 V

(Multiple Choice)

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Question 9

The value of E°_cell is for the following reaction: Cl₂(g)+ 2 Fe²⁺(aq)→ 2 Fe³⁺(aq)+ 2 Cl^-(aq) Calculate the value of E°_cell for the reaction below. Cl^-(g)+ Fe³⁺(aq)→ Fe²⁺(aq)+ ½ Cl₂(g)

(Multiple Choice)

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Question 10

Balance the following half-reaction occurring in a basic solution. MnO₂(s)→ Mn(OH)₂(s)

(Multiple Choice)

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Question 11

According to the cell notation below,which of the following species is undergoing reduction? Ni | Ni²⁺(aq)|| Mn²⁺(aq)| MnO₂(s)| Pt(s)

(Multiple Choice)

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Question 12

Calculate E_cell for the following electrochemical cell at 25°C.The standard cell potential,E°_cell,is 0.460 V. Cu(s)| Cu²⁺(aq,0.016 M)|| Ag⁺(aq,0.11 M)| Ag(s)

(Multiple Choice)

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Question 13

The electrochemical reaction that powers a lead-acid storage battery is as follows: Pb(s)+ PbO₂(s)+ 4 H⁺(aq)+ 2 SO₄^2-(aq)→ 2 PbSO₄(s)+ 2 H₂O( ) A single cell of this battery consists of a Pb electrode and a PbO₂ electrode,each submerged in sulfuric acid.Which of the following reactions occurs at the cathode during discharge?

(Multiple Choice)

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Question 14

Write the balanced oxidation half-reaction for the following overall reaction: 2 H⁺(aq)+ Ca(s)→ Ca²⁺(aq)+ H₂(g)

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Question 15

Which of the following statements is true for the following reaction,assuming the given reaction proceeds in the forward direction? Fe³⁺(aq)+ Co(s)→ Fe²⁺(aq)+ Co²⁺(aq)

(Multiple Choice)

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Question 16

Which of the following are the expected products when an aqueous solution of lithium sulfate is electrolyzed? Reduction Half-Reaction E° (V) Li⁺(aq)+ e^-→ Li(s) -3)04 2 H₂O(l)+ 2 e^- → H₂(g)+ 2 OH^-(aq) -0)83 2 H⁺(aq)+ 2 e^- → H₂(g) 0)00 O₂(g)+ 4 H⁺(aq)+ 4 e^- → 2 H₂O(l) 1)23 S₂O₈^2-(aq)+ 2 e^- → 2 SO₄^2-(aq) 2)01

(Multiple Choice)

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Question 17

The unit for electromotive force,emf,is the volt.1 volt is equal to _____.

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Question 18

Which of the following is the cell notation for a voltaic cell based on the following reaction? Cu²⁺(aq)+ Pb(s)+ SO₄^2-(aq)→ Cu(s)+ PbSO₄(s)

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Question 19

Write a balanced net ionic equation for the overall reaction represented by the following cell notation. Al(s)| Al³⁺(aq)|| Cl₂(g)| Cl-(aq)| Pt(s)

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Question 20

Showing 1 - 20 of 86

Exam 20: Principles of Chemical Reactivity: Electron Transfer Reactions

Calculate ΔrG° for the disproportionation reaction of copper(I)ion (Cu+)at 25 °C. 2 Cu+(aq)→ Cu2+(aq)+ Cu(s) The standard reduction potentials are as follows: Cu+(aq)+ e- → Cu(s) E° = +0.518 V Cu2+(aq)+ 2 e- → Cu(s) E° = +0.337 V

Calculate Ecell for the following electrochemical cell at 25 °C. Pt(s)| Fe3+(aq,0.100 M),Fe2+(aq,0.040 M)|| Cl-(aq,0.50 M)| AgCl(s)| Ag(s) The standard reduction potentials are as follows: AgCl(s)+ e- → Ag(s)+ Cl-(aq) E° = +0.222 V Fe3+(aq)+ e- → Fe2+(aq) E° = +0.771 V

Consider the following half-reactions. Cl2(g)+ 2 e- → 2 Cl-(aq) E° = +1.36 V Ag+(aq)+ e- → Ag(s) E° = +0.80 V Cu2+(aq)+ 2 e- → Cu(s) E° = +0.34 V Sn2+(aq)+ 2 e- → Sn(s) E° = -0.14 V Al3+(aq)+ 3 e- → Al(s) E° = -1.66 V Which of the following species will reduce Cu2+(aq)ion?

The standard reduction potentials for a reaction are as follows: Pb2+(aq)+ 2 e- → Pb(s) E° = -0.126 V PbSO4(s)+ 2 e- → Pb(s)+ SO42-(aq) E° = -0.355 V Calculate the Ksp for lead(II)sulfate (PbSO4)at 25 °C.

Which of the following statements is true concerning the electrochemical cell Zn(s)| Zn2+(aq,1.0 M)|| Ca2+(aq,1.0 M)| Ca(s) The standard reduction potentials are given follows: Zn2+(aq)+ 2 e− → Zn(s); E° = -0.76 V Ca2+(aq)+ 2 e− → Ca(s); E° = -2.87 V

One Faraday is defined as the:

Which of the following statements is true for electron transfer reactions?

Calculate the value of the equilibrium constant (K)at 25 °C for the following cell reaction: Sn(s)+ Pb2+(aq)→ Sn2+(aq)+ Pb(s); E°cell = 0.014 V

The value of E°cell is for the following reaction: Cl2(g)+ 2 Fe2+(aq)→ 2 Fe3+(aq)+ 2 Cl-(aq) Calculate the value of E°cell for the reaction below. Cl-(g)+ Fe3+(aq)→ Fe2+(aq)+ ½ Cl2(g)

Balance the following half-reaction occurring in a basic solution. MnO2(s)→ Mn(OH)2(s)

According to the cell notation below,which of the following species is undergoing reduction? Ni | Ni2+(aq)|| Mn2+(aq)| MnO2(s)| Pt(s)

Calculate Ecell for the following electrochemical cell at 25°C.The standard cell potential,E°cell,is 0.460 V. Cu(s)| Cu2+(aq,0.016 M)|| Ag+(aq,0.11 M)| Ag(s) ​

Write the balanced oxidation half-reaction for the following overall reaction: 2 H+(aq)+ Ca(s)→ Ca2+(aq)+ H2(g)

Which of the following statements is true for the following reaction,assuming the given reaction proceeds in the forward direction? Fe3+(aq)+ Co(s)→ Fe2+(aq)+ Co2+(aq)

The unit for electromotive force,emf,is the volt.1 volt is equal to _____.

Which of the following is the cell notation for a voltaic cell based on the following reaction? Cu2+(aq)+ Pb(s)+ SO42-(aq)→ Cu(s)+ PbSO4(s)

Write a balanced net ionic equation for the overall reaction represented by the following cell notation. Al(s)| Al3+(aq)|| Cl2(g)| Cl-(aq)| Pt(s)

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Calculate Δ_rG° for the disproportionation reaction of copper(I)ion (Cu⁺)at 25 °C. 2 Cu⁺(aq)→ Cu²⁺(aq)+ Cu(s) The standard reduction potentials are as follows: Cu⁺(aq)+ e^- → Cu(s) E° = +0.518 V Cu²⁺(aq)+ 2 e^- → Cu(s) E° = +0.337 V

Calculate E_cell for the following electrochemical cell at 25 °C. Pt(s)| Fe³⁺(aq,0.100 M),Fe²⁺(aq,0.040 M)|| Cl^-(aq,0.50 M)| AgCl(s)| Ag(s) The standard reduction potentials are as follows: AgCl(s)+ e^- → Ag(s)+ Cl^-(aq) E° = +0.222 V Fe³⁺(aq)+ e^- → Fe²⁺(aq) E° = +0.771 V

The standard reduction potentials for a reaction are as follows: Pb²⁺(aq)+ 2 e^- → Pb(s) E° = -0.126 V PbSO₄(s)+ 2 e^- → Pb(s)+ SO₄^2-(aq) E° = -0.355 V Calculate the K_sp for lead(II)sulfate (PbSO₄)at 25 °C.

Which of the following statements is true concerning the electrochemical cell Zn(s)| Zn²⁺(aq,1.0 M)|| Ca²⁺(aq,1.0 M)| Ca(s) The standard reduction potentials are given follows: Zn²⁺(aq)+ 2 e− → Zn(s); E° = -0.76 V Ca²⁺(aq)+ 2 e− → Ca(s); E° = -2.87 V

Calculate the value of the equilibrium constant (K)at 25 °C for the following cell reaction: Sn(s)+ Pb²⁺(aq)→ Sn²⁺(aq)+ Pb(s); E°_cell= 0.014 V

The value of E°_cell is for the following reaction: Cl₂(g)+ 2 Fe²⁺(aq)→ 2 Fe³⁺(aq)+ 2 Cl^-(aq) Calculate the value of E°_cell for the reaction below. Cl^-(g)+ Fe³⁺(aq)→ Fe²⁺(aq)+ ½ Cl₂(g)

Balance the following half-reaction occurring in a basic solution. MnO₂(s)→ Mn(OH)₂(s)

According to the cell notation below,which of the following species is undergoing reduction? Ni | Ni²⁺(aq)|| Mn²⁺(aq)| MnO₂(s)| Pt(s)

Calculate E_cell for the following electrochemical cell at 25°C.The standard cell potential,E°_cell,is 0.460 V. Cu(s)| Cu²⁺(aq,0.016 M)|| Ag⁺(aq,0.11 M)| Ag(s)

Write the balanced oxidation half-reaction for the following overall reaction: 2 H⁺(aq)+ Ca(s)→ Ca²⁺(aq)+ H₂(g)

Which of the following statements is true for the following reaction,assuming the given reaction proceeds in the forward direction? Fe³⁺(aq)+ Co(s)→ Fe²⁺(aq)+ Co²⁺(aq)

Which of the following is the cell notation for a voltaic cell based on the following reaction? Cu²⁺(aq)+ Pb(s)+ SO₄^2-(aq)→ Cu(s)+ PbSO₄(s)

Write a balanced net ionic equation for the overall reaction represented by the following cell notation. Al(s)| Al³⁺(aq)|| Cl₂(g)| Cl-(aq)| Pt(s)