Question 1

What is undergoing reduction in the redox reaction represented by the following cell notation? 
$\quad$$\quad$$\quad$Fe(s)| Fe3+(aq) $\|$ Cl2(g)| Cl- (aq)| Pt(s)

Accepted Answer

A) Fe(s) 
B) Fe3+(aq) 
C) Cl2(g) 
D) Cl- (aq) 
E) Pt(s) 
A) Fe(s) 
B) Fe3+(aq) 
C) Cl2(g) 
D) Cl- (aq) 
E) Pt(s)

Question 2

Determine which of the following pairs of reactants will result in a spontaneous reaction at 25 °C.

Accepted Answer

A) Pb2+(aq)+ Cu(s); if E°(Pb2+/Pb)= -0.13V and E°(Cu2+/Cu)= +0.16V 
B) Ag+(aq)+ Br- (aq); if E°(Ag+/Ag)= 0.80V and E°(Br2/Br-)= +1.09V 
C) Li+(aq)+ Al(s); if E°(Li+/Li)= -3.04V and E°(Al3+/Al)= -1.66V 
D) Fe3+(aq)+ Ni(s); if E°(Fe3+/Fe)= -0.04V and E°(Ni2+/Ni)= -0.23V 
E) Cd2+(aq)+ I-(aq); if E°(Cd2+/Cd)= -0.40V and E°(I2/I-)= + 0.54V 
A) Pb2+(aq)+ Cu(s); if E°(Pb2+/Pb)= -0.13V and E°(Cu2+/Cu)= +0.16V 
B) Ag+(aq)+ Br- (aq); if E°(Ag+/Ag)= 0.80V and E°(Br2/Br-)= +1.09V 
C) Li+(aq)+ Al(s); if E°(Li+/Li)= -3.04V and E°(Al3+/Al)= -1.66V 
D) Fe3+(aq)+ Ni(s); if E°(Fe3+/Fe)= -0.04V and E°(Ni2+/Ni)= -0.23V 
E) Cd2+(aq)+ I-(aq); if E°(Cd2+/Cd)= -0.40V and E°(I2/I-)= + 0.54V

Question 3

The standard emf for the cell using the overall cell reaction below is +0.48 V: 
$\quad$$\quad$Zn(s)+ $\mathrm { Ni } ^ { 2 + }$ (aq)? $\mathrm { Zn } ^ { 2 + }$ (aq)+ Ni(s)
The emf generated by the cell when [ $\mathrm { Ni } ^ { 2 + }$ ] = 6.50 mol L-1 and [ $\mathrm { Zn } ^ { 2 + }$ ] = 0.500 mol L-1 is --------$\text { V. }$

Accepted Answer

A) 0.55 
B) 0.45 
C) 0.61 
D) 0.50 
E) 0.51 
A) 0.55 
B) 0.45 
C) 0.61 
D) 0.50 
E) 0.51

Question 4

Consider the following standard reduction potentials: 
$\quad$$\quad$Ni2+(aq)+ 2 e- → Ni(s)E° = -0.26 V
$\quad$$\quad$I2(s)+ 2 e- → 2 I-(aq)E° = +0.54 V
Under standard conditions,

Accepted Answer

A) Ni2+(aq)is a stronger oxidizing agent than I2(s),and I-(aq)is a stronger reducing agent than Ni(s). 
B) I2(s)is a stronger oxidizing agent than Ni2+(aq),and Ni(s)is a stronger reducing agent than I-(aq). 
C) Ni(s)is a stronger oxidizing agent than I-(aq),and Ni2+(aq)is a stronger reducing agent than I2(s). 
D) I-(aq)is a stronger oxidizing agent than Ni(s),and I2(s)is a stronger reducing agent than Ni2+(aq). 
A) Ni2+(aq)is a stronger oxidizing agent than I2(s),and I-(aq)is a stronger reducing agent than Ni(s). 
B) I2(s)is a stronger oxidizing agent than Ni2+(aq),and Ni(s)is a stronger reducing agent than I-(aq). 
C) Ni(s)is a stronger oxidizing agent than I-(aq),and Ni2+(aq)is a stronger reducing agent than I2(s). 
D) I-(aq)is a stronger oxidizing agent than Ni(s),and I2(s)is a stronger reducing agent than Ni2+(aq).

Question 5

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: 
$\quad$$\quad$$\quad$Sn(s)| Sn2+(aq,0.022 mol L-1) $\|$ Ag+(aq,2.7 mol L-1)| Ag(s)
E°(Sn2+/Sn)= -0.14 V and E°(Ag+/Ag)= +0.80 V

Accepted Answer

A) +1.01 V 
B) -0.83 V 
C) +1.31 V 
D) +0.01 V 
E) -0.66 V 
A) +1.01 V 
B) -0.83 V 
C) +1.31 V 
D) +0.01 V 
E) -0.66 V

Question 6

Which of the following is the strongest oxidizing agent?

Accepted Answer

A) Br2(l) 
B) Au3+(aq) 
C) Ag(s) 
D) Br- (aq) 
E) Au(s) 
A) Br2(l) 
B) Au3+(aq) 
C) Ag(s) 
D) Br- (aq) 
E) Au(s)

Question 7

For the galvanic cell reaction,expressed below using shorthand notation,what half-reaction occurs at the cathode? 
$\quad$$\quad$Zn(s)| Zn2+(aq)|| Ni2+(aq)| Ni(s)

Accepted Answer

A) Zn(s)→ Zn2+(aq)+ 2 e- 
B) Zn2+(aq)+ 2 e- → Zn(s) 
C) Ni(s)→ Ni2+(aq)+ 2 e- 
D) Ni2+(aq)+ 2 e- → Ni(s) 
A) Zn(s)→ Zn2+(aq)+ 2 e- 
B) Zn2+(aq)+ 2 e- → Zn(s) 
C) Ni(s)→ Ni2+(aq)+ 2 e- 
D) Ni2+(aq)+ 2 e- → Ni(s)

What is undergoing reduction in the redox reaction represented by the following cell notation? $\quad$ $\quad$ $\quad$ Fe(s)| Fe³⁺(aq) $\|$ Cl₂(g)| Cl^- (aq)| Pt(s)

Determine which of the following pairs of reactants will result in a spontaneous reaction at 25 °C.

Consider the following standard reduction potentials: $\quad$ $\quad$ Ni²⁺(aq)+ 2 e^- → Ni(s)E° = -0.26 V $\quad$ $\quad$ I₂(s)+ 2 e^- → 2 I^-(aq)E° = +0.54 V Under standard conditions,

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: $\quad$ $\quad$ $\quad$ Sn(s)| Sn²⁺(aq,0.022 mol L^-1) $\|$ Ag⁺(aq,2.7 mol L^-1)| Ag(s) E°(Sn²⁺/Sn)= -0.14 V and E°(Ag⁺/Ag)= +0.80 V

Which of the following is the strongest oxidizing agent?

For the galvanic cell reaction,expressed below using shorthand notation,what half-reaction occurs at the cathode? $\quad$ $\quad$ Zn(s)| Zn²⁺(aq)|| Ni²⁺(aq)| Ni(s)

Units of Measurement for Physical and Chemical Change

Atoms and Elements

Molecules,compounds,and Nomenclature

Chemical Reactions and Stoichiometry

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding II: Molecular Shapes, valence Bond Theory, and Molecular Orbital Theory

Liquids, solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Gibbs Energy and Thermodynamics

Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry II: Reactions

Biochemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Transition Metals and Coordination Compounds

Filters

Exam 18: Electrochemistry

What is undergoing reduction in the redox reaction represented by the following cell notation? \quad\quad\quad Fe(s)| Fe3+(aq) ∥\|∥ Cl2(g)| Cl- (aq)| Pt(s)

Determine which of the following pairs of reactants will result in a spontaneous reaction at 25 °C.

Consider the following standard reduction potentials: \quad\quad Ni2+(aq)+ 2 e- → Ni(s)E° = -0.26 V \quad\quad I2(s)+ 2 e- → 2 I-(aq)E° = +0.54 V Under standard conditions,

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: \quad\quad\quad Sn(s)| Sn2+(aq,0.022 mol L-1) ∥\|∥ Ag+(aq,2.7 mol L-1)| Ag(s) E°(Sn2+/Sn)= -0.14 V and E°(Ag+/Ag)= +0.80 V

Which of the following is the strongest oxidizing agent?

For the galvanic cell reaction,expressed below using shorthand notation,what half-reaction occurs at the cathode? \quad\quad Zn(s)| Zn2+(aq)|| Ni2+(aq)| Ni(s)

Units of Measurement for Physical and Chemical Change

Atoms and Elements

Molecules,compounds,and Nomenclature

Chemical Reactions and Stoichiometry

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding II: Molecular Shapes, valence Bond Theory, and Molecular Orbital Theory

Liquids, solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Aqueous Ionic Equilibrium

Gibbs Energy and Thermodynamics

Radioactivity and Nuclear Chemistry

Organic Chemistry I: Structures

Organic Chemistry II: Reactions

Biochemistry

Chemistry of the Nonmetals

Metals and Metallurgy

Transition Metals and Coordination Compounds

Filters

What is undergoing reduction in the redox reaction represented by the following cell notation? $\quad$ $\quad$ $\quad$ Fe(s)| Fe³⁺(aq) $\|$ Cl₂(g)| Cl^- (aq)| Pt(s)

Consider the following standard reduction potentials: $\quad$ $\quad$ Ni²⁺(aq)+ 2 e^- → Ni(s)E° = -0.26 V $\quad$ $\quad$ I₂(s)+ 2 e^- → 2 I^-(aq)E° = +0.54 V Under standard conditions,

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °C: $\quad$ $\quad$ $\quad$ Sn(s)| Sn²⁺(aq,0.022 mol L^-1) $\|$ Ag⁺(aq,2.7 mol L^-1)| Ag(s) E°(Sn²⁺/Sn)= -0.14 V and E°(Ag⁺/Ag)= +0.80 V

For the galvanic cell reaction,expressed below using shorthand notation,what half-reaction occurs at the cathode? $\quad$ $\quad$ Zn(s)| Zn²⁺(aq)|| Ni²⁺(aq)| Ni(s)