Question 1

What half-reaction occurs at the cathode during the electrolysis of molten potassium bromide?

Accepted Answer

A)  K(s)→ K+(l)+ e- 
B)  Br2(l)+ 2 e- → 2 Br-(l) 
C)  2 Br-(l)→ Br2(l)+ 2 e- 
D)  2 K+(l)+ 2 e- → 2 K(l) 
E)  2 H2O(l)+ 2 e- → H2(g)+ 2 OH-(l) 
A)  K(s)→ K+(l)+ e- 
B)  Br2(l)+ 2 e- → 2 Br-(l) 
C)  2 Br-(l)→ Br2(l)+ 2 e- 
D)  2 K+(l)+ 2 e- → 2 K(l) 
E)  2 H2O(l)+ 2 e- → H2(g)+ 2 OH-(l)

Question 2

Use the following standard reduction potentials to determine which species is the strongest oxidizing agent. Fe2+(aq)+ 2 e- → Fe(s); E° = -0.41 V
Pt2+(aq)+ 2 e- → Pt(s); E° = 1.18 V
Cr2O72-(aq)+ 14 H+(aq)+ 6 e- → 2 Cr3+(aq)+ 7 H2O(   ); E° = 1.33 V

Accepted Answer

A)  Fe 
B)  Pt 
C)  Cr3+ 
D)  Fe2+ 
E)  Cr2O72- 
A)  Fe 
B)  Pt 
C)  Cr3+ 
D)  Fe2+ 
E)  Cr2O72-

Question 3

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

Accepted Answer

A)  Pt2+(aq)+ Pb(s)→ Pt(s)+ Pb2+(aq);   = 1.310 V 
B)  Pt(s)+ Pb2+(aq)→ Pt2+(aq)+ Pb(s);   = −1.310 V 
C)  Pt2+(aq)+ Pb2+(aq)→ Pt(s)+ Pb(s);   = 1.050 V 
D)  Pt2+(aq)+ Pb(s)→ Pt(s)+ Pb2+(aq);   =0.655 V 
E)  Pt(s)+ Pb2+(aq)→ Pt2+(aq)+ Pb(s);   = −0.655 V 
A)  Pt2+(aq)+ Pb(s)→ Pt(s)+ Pb2+(aq);   = 1.310 V 
B)  Pt(s)+ Pb2+(aq)→ Pt2+(aq)+ Pb(s);   = −1.310 V 
C)  Pt2+(aq)+ Pb2+(aq)→ Pt(s)+ Pb(s);   = 1.050 V 
D)  Pt2+(aq)+ Pb(s)→ Pt(s)+ Pb2+(aq);   =0.655 V 
E)  Pt(s)+ Pb2+(aq)→ Pt2+(aq)+ Pb(s);   = −0.655 V

Question 4

Given the following two half-reactions,write the overall reaction in the direction in which it is product-favored,and calculate the standard cell potential. Pb2+(aq)+ 2 e- → Pb(s)
E° = -0.126 V
Fe3+(aq)+ e- → Fe2+(s)
E° = +0.771 V

Accepted Answer

A)  Pb2+(aq)+ 2 Fe2+(s)→ Pb(s)+ 2 Fe3+(aq);   = +0.897 V 
B)  Pb2+(aq)+ Fe2+(s)→ Pb(s)+ Fe3+(aq);   = +0.645 V 
C)  Pb(s)+ 2 Fe3+(aq)→ Pb2+(aq)+ 2 Fe2+(s);   = +1.416 V 
D)  Pb(s)+ 2 Fe3+(aq)→ Pb2+(aq)+ 2 Fe2+(s);   = +0.897 V 
E)  Pb(s)+ Fe3+(aq)→ Pb2+(aq)+ Fe2+(s);   = +0.645 V 
A)  Pb2+(aq)+ 2 Fe2+(s)→ Pb(s)+ 2 Fe3+(aq);   = +0.897 V 
B)  Pb2+(aq)+ Fe2+(s)→ Pb(s)+ Fe3+(aq);   = +0.645 V 
C)  Pb(s)+ 2 Fe3+(aq)→ Pb2+(aq)+ 2 Fe2+(s);   = +1.416 V 
D)  Pb(s)+ 2 Fe3+(aq)→ Pb2+(aq)+ 2 Fe2+(s);   = +0.897 V 
E)  Pb(s)+ Fe3+(aq)→ Pb2+(aq)+ Fe2+(s);   = +0.645 V

Question 5

Which of the following equations represents the Nernst equation?

Accepted Answer

A)    
B)    
C)    
D)    
E)    
A)    
B)    
C)    
D)    
E)

Question 6

Calculate the cell potential at 25 °C for the following overall reaction. Zn2+(aq)+ 2 Fe2+(aq)→ Zn(s)+ 2 Fe3+(aq)
[Zn2+] = 1.50 × 10-4 M,[Fe3+] = 0.0200 M,and [Fe2+] = 0.0100 M.The standard reduction potentials are as follows:
Zn2+(aq)+ 2 e- → Zn(s)
E° = -0.763 V
Fe3+(aq)+ e- → Fe2+(aq)
E° = +0.771 V

Accepted Answer

A)  -1.665 V 
B)  -1.534 V 
C)  -1.439 V 
D)  -0.008 V 
E)  +0.008 V 
A)  -1.665 V 
B)  -1.534 V 
C)  -1.439 V 
D)  -0.008 V 
E)  +0.008 V

What half-reaction occurs at the cathode during the electrolysis of molten potassium bromide?

Use the following standard reduction potentials to determine which species is the strongest oxidizing agent. Fe²⁺(aq)+ 2 e^- → Fe(s); E° = -0.41 V Pt²⁺(aq)+ 2 e^- → Pt(s); E° = 1.18 V Cr₂O₇^2-(aq)+ 14 H⁺(aq)+ 6 e^- → 2 Cr³⁺(aq)+ 7 H₂O( ); E° = 1.33 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

Given the following two half-reactions,write the overall reaction in the direction in which it is product-favored,and calculate the standard cell potential. Pb²⁺(aq)+ 2 e^- → Pb(s) E° = -0.126 V Fe³⁺(aq)+ e^- → Fe²⁺(s) E° = +0.771 V

Which of the following equations represents the Nernst equation?

Basic Concepts of Chemistry

Lets Review: The Tools of Quantitative Chemistry

Atoms, molecules, and Ions

Chemical Reactions

Stoichiometry: Quantitative Information About Chemical Reactions

Principles of Chemical Reactivity: Energy and Chemical Reactions

The Structure of Atoms

The Structure of Atoms and Periodic Trends

Bonding and Molecular Structure

Bonding and Molecular Structure Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

The Solid State

Solutions and Their Behavior

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Chemical Reactivity: Equilibria

Principles of Chemical Reactivity: the Chemistry of Acids and Bases

Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Principles of Chemical Reactivity: Entropy and Free Energy

Environmental Chemistry: Earths Environment, energy, and Sustainability

The Chemistry of the Main Group Elements

The Chemistry of the Transition Elements

Carbon: Not Just Another Element

Biochemistry

Nuclear Chemistry

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Exam 20: Principles of Chemical Reactivity: Electron Transfer Reactions

What half-reaction occurs at the cathode during the electrolysis of molten potassium bromide?

Use the following standard reduction potentials to determine which species is the strongest oxidizing agent. Fe2+(aq)+ 2 e- → Fe(s); E° = -0.41 V Pt2+(aq)+ 2 e- → Pt(s); E° = 1.18 V Cr2O72-(aq)+ 14 H+(aq)+ 6 e- → 2 Cr3+(aq)+ 7 H2O( ); E° = 1.33 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

Given the following two half-reactions,write the overall reaction in the direction in which it is product-favored,and calculate the standard cell potential. Pb2+(aq)+ 2 e- → Pb(s) E° = -0.126 V Fe3+(aq)+ e- → Fe2+(s) E° = +0.771 V

Which of the following equations represents the Nernst equation?

Basic Concepts of Chemistry

Lets Review: The Tools of Quantitative Chemistry

Atoms, molecules, and Ions

Chemical Reactions

Stoichiometry: Quantitative Information About Chemical Reactions

Principles of Chemical Reactivity: Energy and Chemical Reactions

The Structure of Atoms

The Structure of Atoms and Periodic Trends

Bonding and Molecular Structure

Bonding and Molecular Structure Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

The Solid State

Solutions and Their Behavior

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Chemical Reactivity: Equilibria

Principles of Chemical Reactivity: the Chemistry of Acids and Bases

Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Principles of Chemical Reactivity: Entropy and Free Energy

Environmental Chemistry: Earths Environment, energy, and Sustainability

The Chemistry of the Main Group Elements

The Chemistry of the Transition Elements

Carbon: Not Just Another Element

Biochemistry

Nuclear Chemistry

Filters

Use the following standard reduction potentials to determine which species is the strongest oxidizing agent. Fe²⁺(aq)+ 2 e^- → Fe(s); E° = -0.41 V Pt²⁺(aq)+ 2 e^- → Pt(s); E° = 1.18 V Cr₂O₇^2-(aq)+ 14 H⁺(aq)+ 6 e^- → 2 Cr³⁺(aq)+ 7 H₂O( ); E° = 1.33 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

Given the following two half-reactions,write the overall reaction in the direction in which it is product-favored,and calculate the standard cell potential. Pb²⁺(aq)+ 2 e^- → Pb(s) E° = -0.126 V Fe³⁺(aq)+ e^- → Fe²⁺(s) E° = +0.771 V