Which of the following are the expected products when an aqueous solution of lithium sulfate is electrolyzed?\[\begin{array} { l l } \text { Reduction Half-Reaction } & \mathrm { E } ^ { \circ } ( \mathrm { V } ) \\ \mathrm { Li } ^ { + } ( \mathrm { aq } ) + \mathrm { e } ^ { - } \rightarrow \mathrm { Li } ( \mathrm { s } ) & - 3.04 \\ 2 \mathrm { H } _ { 2 } \mathrm { O } ( \ell ) + 2 \mathrm { e } ^ { - } \rightarrow \mathrm { H } _ { 2 } ( \mathrm {~g} ) + 2 \mathrm { OH } ^ { - } ( \mathrm { aq } ) & - 0.83 \\ 2 \mathrm { H } ^ { + } ( \mathrm { aq } ) + 2 \mathrm { e } ^ { - } \rightarrow \mathrm { H } _ { 2 } ( \mathrm {~g} ) & 0.00 \\ \mathrm { O } _ { 2 } ( \mathrm {~g} ) + 4 \mathrm { H } ^ { + } ( \mathrm { aq } ) + 4 \mathrm { e } ^ { - } \rightarrow 2 \mathrm { H } _ { 2 } \mathrm { O } ( \ell ) & 1.23 \\ \mathrm {~S} _ { 2 } \mathrm { O } _ { 8 } { } ^ { 2 - } ( \mathrm { aq } ) + 2 \mathrm { e } ^ { - } \rightarrow 2 \mathrm { SO } _ { 4 } { } ^ { 2 - } ( \mathrm { aq } ) & 2.01 \end{array}\]

A) Li(s) and H2(g) B) H2(g), OH-(aq), O2(g), and H+(aq) C) O2(g), H+(aq), and Li(s) D) H2(g), OH-(aq), and Li(s) E) H2(g), OH-(aq), and S2O82-(aq) A) Li(s) and H2(g) B) H2(g), OH-(aq), O2(g), and H+(aq) C) O2(g), H+(aq), and Li(s) D) H2(g), OH-(aq), and Li(s) E) H2(g), OH-(aq), and S2O82-(aq)

The value of E°cell is $0.59 \mathrm {~V}$ 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

Calculate the standard reduction potential for the given reaction at 25 °C. AuCl4-(aq) + 3 e- → Au(s) + 4 Cl-(aq) The thermodynamic information is as follows: Au3+(aq) + 3 e- → Au(s) E° = +1.50 V Au3+(aq) + 4 Cl-(aq) → AuCl4-(aq) Kf = 2.3 × 1025

A) -1.28 V B) -0.50 V C) +1.00 V D) +1.28 V E) +3.85 V A) -1.28 V B) -0.50 V C) +1.00 V D) +1.28 V E) +3.85 V

Calculate $E _ { \text {cell } } ^ { \circ }$ for the electrochemical cell Ag(s) | AgCl(s) | Cl-(aq, 1.0 M) || Cu2+(aq, 1.0 M) | Cu(s). The standard reduction potentials are as follows: Cu2+(aq) + 2 e- ? Cu(s) E° = +0.337 V AgCl(s) + e- ? Ag(s) + Cl-(aq) E° = +0.222 V

A) -0.115 V B) -0.107 V C) +0.115 V D) +0.452 V E) +0.559 V A) -0.115 V B) -0.107 V C) +0.115 V D) +0.452 V E) +0.559 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?

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)

Exam 20: Principles of Chemical Reactivity: Electron Transfer Reactions

The following has a potential of 0.34 V. $\mathrm { Cu } ^ { 2 + } ( \mathrm { aq } ) + \mathrm { H } _ { 2 } ( \mathrm {~g} ) \rightarrow 2 \mathrm { H } ^ { + } ( \mathrm { aq } ) + \mathrm { Cu } ( \mathrm { s } )$ If the concentrations of each of the ions is 1.0 M and the pressure of H₂ is 1.0 atm, then E° for the half-reaction $\mathrm { Cu } ^ { 2 + } ( \mathrm { aq } ) + 2 e ^ { - } \rightarrow \mathrm { Cu } ( \mathrm { s } )$ is _____.

(Multiple Choice)

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Question 61

Write a balanced net ionic equation for the overall reaction represented by the following cell notation. Cu(s) | Cu²⁺(aq) || Mn²⁺(aq) | Mn(s)

(Multiple Choice)

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Question 62

Which of the following are the expected products when an aqueous solution of lithium sulfate is electrolyzed? Reduction Half-Reaction () ()+\rightarrow() -3.04 2(\ell)+2\rightarrow()+2() -0.83 2()+2\rightarrow() 0.00 ()+4()+4\rightarrow2(\ell) 1.23 ()+2\rightarrow2() 2.01

(Multiple Choice)

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Question 63

Explain the function of a salt bridge in a voltaic cell.

(Essay)

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Question 64

The value of E°_cell is $0.59 \mathrm {~V}$ 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 65

Calculate the standard reduction potential for the given reaction at 25 °C. AuCl₄^-(aq) + 3 e^- → Au(s) + 4 Cl^-(aq) The thermodynamic information is as follows: Au³⁺(aq) + 3 e^- → Au(s) E° = +1.50 V Au³⁺(aq) + 4 Cl^-(aq) → AuCl₄^-(aq) K_f = 2.3 × 10²⁵

(Multiple Choice)

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Question 66

Which of the following species are likely to behave as oxidizing agents? Li(s), H₂(g), MnO₄^-(aq), and Cl^-(aq)

(Multiple Choice)

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Question 67

How many electrons are transferred in the given reaction? Ni + 2 HCl → Ni Cl₂ + H₂

(Multiple Choice)

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Question 68

Which of the following is the cell notation for a voltaic cell based on the following reaction? Cu²⁺(aq) + Fe(s) → Cu(s) + Fe²⁺(aq)

(Multiple Choice)

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Question 69

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)

(Multiple Choice)

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Question 70

How many moles of electrons are produced from a current of 17.0 A in 3.40 hours?

(Multiple Choice)

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Question 71

Calculate $E _ { \text {cell } } ^ { \circ }$ for the electrochemical cell Ag(s) | AgCl(s) | Cl^-(aq, 1.0 M) || Cu²⁺(aq, 1.0 M) | Cu(s). The standard reduction potentials are as follows: Cu²⁺(aq) + 2 e^- ? Cu(s) E° = +0.337 V AgCl(s) + e^- ? Ag(s) + Cl^-(aq) E° = +0.222 V

(Multiple Choice)

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Question 72

Use the following standard reduction potentials to determine which species is the strongest reducing agent. 2 H⁺(aq) + 2 e^- → H₂(g); 0.00 V K⁺(aq) + e^- → K(s); -2.93 V F₂(g) + 2 e^- → 2 F^-(aq); 2.87 V Al³⁺(aq) + 3 e^- → Al(s); -1.66 V Pb²⁺(aq) + 2 e^- → Pb(s); -0.13 V

(Multiple Choice)

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Question 73

Which of the following reactions will require the use of an inert electrode when used in a voltaic cell?

(Multiple Choice)

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Question 74

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?

(Multiple Choice)

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Question 75

Which of the following is the balanced overall reaction and standard cell potential of an electrochemical cell constructed from half-cells with the given half reactions? Pt²⁺(aq) + 2 e- ? Pt(s); E° = 1.180 V Pb²⁺(aq) + 2 e- ? Pb(s); E° = -0.130 V

(Multiple Choice)

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Question 76

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 77

In the context of the diagram given below, which of the following statements is true concerning half-cell II?

(Multiple Choice)

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Question 78

The following electrochemical cell has a potential of +0.326 V at 25 °C. Pt | H₂(g, 1.00 atm) | H⁺(aq, 1.00 M) || Cl^-(aq) | AgCl(s) | Ag The standard reduction potential, E°, of AgCl(s) is +0.222 V. Calculate the Cl^-(aq) ion concentration.

(Multiple Choice)

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Question 79

In an electrolytic cell, reduction occurs at the _ and oxidation occurs at the _.

(Short Answer)

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Question 80

Showing 61 - 80 of 83

Exam 20: Principles of Chemical Reactivity: Electron Transfer Reactions

Write a balanced net ionic equation for the overall reaction represented by the following cell notation. Cu(s) | Cu2+(aq) || Mn2+(aq) | Mn(s)

Which of the following are the expected products when an aqueous solution of lithium sulfate is electrolyzed? Reduction Half-Reaction () ()+\rightarrow() -3.04 2(\ell)+2\rightarrow()+2() -0.83 2()+2\rightarrow() 0.00 ()+4()+4\rightarrow2(\ell) 1.23 ()+2\rightarrow2() 2.01

Explain the function of a salt bridge in a voltaic cell.

The value of E°cell is 0.59 V0.59 \mathrm {~V}0.59 V 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)

Calculate the standard reduction potential for the given reaction at 25 °C. AuCl4-(aq) + 3 e- → Au(s) + 4 Cl-(aq) The thermodynamic information is as follows: Au3+(aq) + 3 e- → Au(s) E° = +1.50 V Au3+(aq) + 4 Cl-(aq) → AuCl4-(aq) Kf = 2.3 × 1025

Which of the following species are likely to behave as oxidizing agents? Li(s), H2(g), MnO4-(aq), and Cl-(aq)

How many electrons are transferred in the given reaction? Ni + 2 HCl → Ni Cl2 + H2

Which of the following is the cell notation for a voltaic cell based on the following reaction? Cu2+(aq) + Fe(s) → Cu(s) + Fe2+(aq)

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)

How many moles of electrons are produced from a current of 17.0 A in 3.40 hours?

Calculate Ecell ∘E _ { \text {cell } } ^ { \circ }Ecell ∘​ for the electrochemical cell Ag(s) | AgCl(s) | Cl-(aq, 1.0 M) || Cu2+(aq, 1.0 M) | Cu(s). The standard reduction potentials are as follows: Cu2+(aq) + 2 e- ? Cu(s) E° = +0.337 V AgCl(s) + e- ? Ag(s) + Cl-(aq) E° = +0.222 V

Use the following standard reduction potentials to determine which species is the strongest reducing agent. 2 H+(aq) + 2 e- → H2(g); 0.00 V K+(aq) + e- → K(s); -2.93 V F2(g) + 2 e- → 2 F-(aq); 2.87 V Al3+(aq) + 3 e- → Al(s); -1.66 V Pb2+(aq) + 2 e- → Pb(s); -0.13 V

Which of the following reactions will require the use of an inert electrode when used in a voltaic cell?

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?

Which of the following is the balanced overall reaction and standard cell potential of an electrochemical cell constructed from half-cells with the given half reactions? Pt2+(aq) + 2 e- ? Pt(s); E° = 1.180 V Pb2+(aq) + 2 e- ? Pb(s); E° = -0.130 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

In the context of the diagram given below, which of the following statements is true concerning half-cell II?

The following electrochemical cell has a potential of +0.326 V at 25 °C. Pt | H2(g, 1.00 atm) | H+(aq, 1.00 M) || Cl-(aq) | AgCl(s) | Ag The standard reduction potential, E°, of AgCl(s) is +0.222 V. Calculate the Cl-(aq) ion concentration.

In an electrolytic cell, reduction occurs at the _____ and oxidation occurs at the _____.

Basic Concepts of Chemistry

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Stoichiometry: Quantitative Information About Chemical Reactions

Principles of Chemical Reactivity: Energy and Chemical Reactions

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Write a balanced net ionic equation for the overall reaction represented by the following cell notation. Cu(s) | Cu²⁺(aq) || Mn²⁺(aq) | Mn(s)

The value of E°_cell is $0.59 \mathrm {~V}$ 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)

Calculate the standard reduction potential for the given reaction at 25 °C. AuCl₄^-(aq) + 3 e^- → Au(s) + 4 Cl^-(aq) The thermodynamic information is as follows: Au³⁺(aq) + 3 e^- → Au(s) E° = +1.50 V Au³⁺(aq) + 4 Cl^-(aq) → AuCl₄^-(aq) K_f = 2.3 × 10²⁵

Which of the following species are likely to behave as oxidizing agents? Li(s), H₂(g), MnO₄^-(aq), and Cl^-(aq)

How many electrons are transferred in the given reaction? Ni + 2 HCl → Ni Cl₂ + H₂

Which of the following is the cell notation for a voltaic cell based on the following reaction? Cu²⁺(aq) + Fe(s) → Cu(s) + Fe²⁺(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)

Calculate $E _ { \text {cell } } ^ { \circ }$ for the electrochemical cell Ag(s) | AgCl(s) | Cl^-(aq, 1.0 M) || Cu²⁺(aq, 1.0 M) | Cu(s). The standard reduction potentials are as follows: Cu²⁺(aq) + 2 e^- ? Cu(s) E° = +0.337 V AgCl(s) + e^- ? Ag(s) + Cl^-(aq) E° = +0.222 V

Use the following standard reduction potentials to determine which species is the strongest reducing agent. 2 H⁺(aq) + 2 e^- → H₂(g); 0.00 V K⁺(aq) + e^- → K(s); -2.93 V F₂(g) + 2 e^- → 2 F^-(aq); 2.87 V Al³⁺(aq) + 3 e^- → Al(s); -1.66 V Pb²⁺(aq) + 2 e^- → Pb(s); -0.13 V

Which of the following is the balanced overall reaction and standard cell potential of an electrochemical cell constructed from half-cells with the given half reactions? Pt²⁺(aq) + 2 e- ? Pt(s); E° = 1.180 V Pb²⁺(aq) + 2 e- ? Pb(s); E° = -0.130 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 following electrochemical cell has a potential of +0.326 V at 25 °C. Pt | H₂(g, 1.00 atm) | H⁺(aq, 1.00 M) || Cl^-(aq) | AgCl(s) | Ag The standard reduction potential, E°, of AgCl(s) is +0.222 V. Calculate the Cl^-(aq) ion concentration.

In an electrolytic cell, reduction occurs at the _ and oxidation occurs at the _.