Question 1

Which of the following is the weakest reducing 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 2

A voltaic cell is constructed with two $\mathrm { Zn } ^ { 2 + }$ -Zn electrodes,where the half-reaction is $\quad$
$\quad$$\mathrm { Zn } ^ { 2 + }$ + $2 \mathrm { e } ^ { - }$ ? Zn (s)$\quad$$\quad$E° = -0.763 V The concentrations of zinc ion in the two compartments are 1.17 × $10 ^ { - 2 }$ mol L-1 and 8.70 × $10 ^ { - 2 }$ mol L-1,respectively.The cell emf is ________ V.

Accepted Answer

A) 0.170 
B) -0.678 
C) -0.0850 
D) 515 
E) 0.0850 
A) 0.170 
B) -0.678 
C) -0.0850 
D) 515 
E) 0.0850

Question 3

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25 °C.(The equation is balanced.) 
$\quad$$\quad$Mg(s)+ Cu2+(aq)→ Cu(s)+ Mg2+(aq)
Mg2+(aq)+ 2 e- → Mg(s)$\quad$$\quad$E° = -2.38 V
Cu2+(aq)+ 2 e- → Cu(s)$\quad$$\quad$ E° = +0.34 V

Accepted Answer

A) +2.04 V 
B) -2.04 V 
C) +2.72 V 
D) -1.36 V 
E) +1.36 V 
A) +2.04 V 
B) -2.04 V 
C) +2.72 V 
D) -1.36 V 
E) +1.36 V

Question 4

The standard cell potential (E°)of a voltaic cell constructed using the cell reaction below is 0.76 V: 
$\quad$Zn(s)+ $2 \mathrm { H } ^ { + }$ (aq)? $\mathrm { Zn } ^ { 2 + }$ (aq)+ $\mathrm { H } _ { 2 }$ (g)
With $\mathrm { P } _ { \mathrm { H } _ { 2 } }$ = 1.0 atm and [ $\mathrm { Zn } ^ { 2 + }$ ] = 1.0 mol L-1,the cell potential is 0.45 V.The concentration of $\mathrm { H } ^ { + }$ in the cathode compartment is ________ mol L-1.

Accepted Answer

A) 3.3 × 10-11 
B) 2.4 × 10-3 
C) 1.1 × 10-21 
D) 0.73 
E) 5.8 × 10-6 
A) 3.3 × 10-11 
B) 2.4 × 10-3 
C) 1.1 × 10-21 
D) 0.73 
E) 5.8 × 10-6

Question 5

Which of the following reactions would be the most spontaneous at 298 K?

Accepted Answer

A) A + 2 B → C; E°cell = +0.98 V 
B) A + B → 2 C; E°cell = -0.030 V 
C) A + B → 3 C; E°cell = +0.15 V 
D) A + B → C; E°cell = +1.22 V 
E) A + B → C; E°cell = -1.22 V 
A) A + 2 B → C; E°cell = +0.98 V 
B) A + B → 2 C; E°cell = -0.030 V 
C) A + B → 3 C; E°cell = +0.15 V 
D) A + B → C; E°cell = +1.22 V 
E) A + B → C; E°cell = -1.22 V

Question 6

Which of the following is the weakest oxidizing agent?

Accepted Answer

A) Sn2+(aq) 
B) Cr3+(aq) 
C) Sn4+(aq) 
D) Cr(s) 
E) Sn(s) 
A) Sn2+(aq) 
B) Cr3+(aq) 
C) Sn4+(aq) 
D) Cr(s) 
E) Sn(s)

Question 7

Identify the battery that is in most automobiles.

Accepted Answer

A) dry-cell battery 
B) lithium-ion battery 
C) lead-acid storage battery 
D) NiCad battery 
E) fuel cell 
A) dry-cell battery 
B) lithium-ion battery 
C) lead-acid storage battery 
D) NiCad battery 
E) fuel cell

Question 8

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25 °C.(The equation is balanced.) 
$\quad$$\quad$$\quad$Sn(s)+ 2Ag+ (aq)→ Sn2+(aq)+ 2Ag(s)
Sn2+(aq)+ 2 e- → Sn(s)$\quad$E° = -0.14 V
Ag+ (aq)+ e- → Ag(s)$\quad$ E° = +0.80 V

Accepted Answer

A) +1.74 V 
B) +0.94 V 
C) +1.08 V 
D) -1.08 V 
E) -1.74 V 
A) +1.74 V 
B) +0.94 V 
C) +1.08 V 
D) -1.08 V 
E) -1.74 V

Question 9

The electrolysis of molten $\mathrm { AlCl } _ { 3 }$ for 4.25 hr with an electrical current of 25.0 A produces ---------$g$ of aluminum metal.

Accepted Answer

A) 9.90 × 10-3 
B) 107 
C) 321 
D) 1.32 
E) 35.7 
A) 9.90 × 10-3 
B) 107 
C) 321 
D) 1.32 
E) 35.7

Question 10

What is the oxidizing agent in the redox reaction represented by the following cell notation? 
$\quad$$\quad$$\quad$Ni(s)| Ni2+(aq) $\|$ Ag+(aq)| Ag(s)

Accepted Answer

A) Ni(s) 
B) Ni2+(aq) 
C) Ag+(aq) 
D) Ag(s) 
E) Pt(s) 
A) Ni(s) 
B) Ni2+(aq) 
C) Ag+(aq) 
D) Ag(s) 
E) Pt(s)

Question 11

Which of the following reactions would have the smallest value of K at 298 K?

Accepted Answer

A) A + B → C; E°cell = +1.22 V 
B) A + 2 B → C; E°cell = +0.98 V 
C) A + B → 2 C; E°cell = -0.030 V 
D) A + B → 3 C; E°cell = +0.15 V 
E) A + B → C; E°cell = -0.015 V 
A) A + B → C; E°cell = +1.22 V 
B) A + 2 B → C; E°cell = +0.98 V 
C) A + B → 2 C; E°cell = -0.030 V 
D) A + B → 3 C; E°cell = +0.15 V 
E) A + B → C; E°cell = -0.015 V

Question 12

A voltaic cell is constructed with two silver-silver chloride electrodes,where the half-reaction is 
$\quad$$\quad$AgCl(s)+ $\mathrm { e } ^ { - }$ ? Ag(s)+ $\mathrm { Cl } ^ { - }$ (aq)E° = +0.222 V
The concentrations of chloride ion in the two compartments are 0.0557 mol L-1 and 5.31 mol L-1,respectively.The cell emf is ________ V.

Accepted Answer

A) 0.00557 
B) 0.531 
C) 53.1 
D) 0.234 
E) 0.117 
A) 0.00557 
B) 0.531 
C) 53.1 
D) 0.234 
E) 0.117

Question 13

Use the tabulated half-cell potentials to calculate the equilibrium constant (K)for the following balanced redox reaction at 25 °C: 
$\quad$$\quad$3I2(s)+ 2Fe(s)→ 2Fe3+(aq)+ 6I- (aq)
E°(I2/I-)= + 0.54 V and E°(Fe3+/Fe)= -0.036 V

Accepted Answer

A) 3.5 × 10-59 
B) 1.1 × 1017 
C) 2.4 × 1058 
D) 8.9 × 10-18 
E) 1.7 × 1029 
A) 3.5 × 10-59 
B) 1.1 × 1017 
C) 2.4 × 1058 
D) 8.9 × 10-18 
E) 1.7 × 1029

Question 14

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °: 
$\quad$$\quad$Cu(s)| Cu2+(aq,0.0032 mol L-1) $\|$ Cu2+(aq,4.48 mol L-1)| Cu(s)
E°(Cu2+/Cu)= +0.34 V

Accepted Answer

A) 0.00 V 
B) +0.093 V 
C) +0.34 V 
D) +0.186 V 
E) +0.052 V 
A) 0.00 V 
B) +0.093 V 
C) +0.34 V 
D) +0.186 V 
E) +0.052 V

Question 15

Which of the following is the weakest oxidizing agent?

Accepted Answer

A) H2O2(aq) 
B) Fe3+(aq) 
C) ClO2(g) 
D) I2(s) 
E) Fe(s) 
A) H2O2(aq) 
B) Fe3+(aq) 
C) ClO2(g) 
D) I2(s) 
E) Fe(s)

Question 16

Which of the following is the strongest reducing agent?

Accepted Answer

A) Al(s) 
B) Zn(s) 
C) Mg(s) 
D) Al3+(aq) 
E) Mg2+(aq) 
A) Al(s) 
B) Zn(s) 
C) Mg(s) 
D) Al3+(aq) 
E) Mg2+(aq)

Question 17

Which of the following is the strongest oxidizing agent?

Accepted Answer

A) H2O2(aq) 
B) Fe3+(aq) 
C) ClO2(g) 
D) I2(s) 
E) Fe(s) 
A) H2O2(aq) 
B) Fe3+(aq) 
C) ClO2(g) 
D) I2(s) 
E) Fe(s)

Question 18

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °: 
$\quad$$\quad$$\quad$Fe(s)| Fe3+(aq,0.0011 mol L-1) $\|$ Fe3+(aq,2.33 mol L-1)| Fe(s)
E°(Fe3+/Fe)= -0.036 V

Accepted Answer

A) +0.066 V 
B) -0.036 V 
C) 0.00 V 
D) -0.099 V 
E) +0.20 V 
A) +0.066 V 
B) -0.036 V 
C) 0.00 V 
D) -0.099 V 
E) +0.20 V

Question 19

Determine the cell notation for the redox reaction given below: 
$\quad$$\quad$$\quad$Sn(s)+ 2Ag+ (aq)? Sn2+(aq)+ 2Ag(s)

Accepted Answer

Question 20

What is the shorthand notation that represents the following galvanic cell reaction? 
$\quad$$\quad$$\quad$2Sn2+(aq)+ Cl2(g)→ 2Sn3+(aq)+ 2Cl-(aq)

Accepted Answer

A) Sn2+(aq)| Sn3+(aq)|| Cl2(g)| Cl-(aq) 
B) Sn(s)| Sn2+(aq)|| Sn4+(aq)Cl2(g)| Cl-(aq)| C(s) 
C) Pt(s)| Sn4+(aq),Sn2+(aq),Cl2(g)|| Cl-(aq)| C(s) 
D) Pt(s)| Sn2+(aq),Sn3+(aq)|| Cl2(g)| Cl-(aq)| C(s) 
A) Sn2+(aq)| Sn3+(aq)|| Cl2(g)| Cl-(aq) 
B) Sn(s)| Sn2+(aq)|| Sn4+(aq)Cl2(g)| Cl-(aq)| C(s) 
C) Pt(s)| Sn4+(aq),Sn2+(aq),Cl2(g)|| Cl-(aq)| C(s) 
D) Pt(s)| Sn2+(aq),Sn3+(aq)|| Cl2(g)| Cl-(aq)| C(s)

Which of the following is the weakest reducing agent?

Which of the following reactions would be the most spontaneous at 298 K?

Which of the following is the weakest oxidizing agent?

Identify the battery that is in most automobiles.

The electrolysis of molten $\mathrm { AlCl } _ { 3 }$ for 4.25 hr with an electrical current of 25.0 A produces --------- $g$ of aluminum metal.

What is the oxidizing agent in the redox reaction represented by the following cell notation? $\quad$ $\quad$ $\quad$ Ni(s)| Ni²⁺(aq) $\|$ Ag⁺(aq)| Ag(s)

Which of the following reactions would have the smallest value of K at 298 K?

Use the tabulated half-cell potentials to calculate the equilibrium constant (K)for the following balanced redox reaction at 25 °C: $\quad$ $\quad$ 3I₂(s)+ 2Fe(s)→ 2Fe³⁺(aq)+ 6I^- (aq) E°(I₂/I^-)= + 0.54 V and E°(Fe³⁺/Fe)= -0.036 V

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °: $\quad$ $\quad$ Cu(s)| Cu²⁺(aq,0.0032 mol L^-1) $\|$ Cu²⁺(aq,4.48 mol L^-1)| Cu(s) E°(Cu²⁺/Cu)= +0.34 V

Which of the following is the weakest oxidizing agent?

Which of the following is the strongest reducing agent?

Which of the following is the strongest oxidizing agent?

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °: $\quad$ $\quad$ $\quad$ Fe(s)| Fe³⁺(aq,0.0011 mol L^-1) $\|$ Fe³⁺(aq,2.33 mol L^-1)| Fe(s) E°(Fe³⁺/Fe)= -0.036 V

Determine the cell notation for the redox reaction given below: $\quad$ $\quad$ $\quad$ Sn(s)+ 2Ag⁺ (aq)? Sn²⁺(aq)+ 2Ag(s)

What is the shorthand notation that represents the following galvanic cell reaction? $\quad$ $\quad$ $\quad$ 2Sn²⁺(aq)+ Cl₂(g)→ 2Sn³⁺(aq)+ 2Cl^-(aq)

Units of Measurement for Physical and Chemical Change

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Molecules,compounds,and Nomenclature

Chemical Reactions and Stoichiometry

Gases

Thermochemistry

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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

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Aqueous Ionic Equilibrium

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Filters

Exam 18: Electrochemistry

Which of the following is the weakest reducing agent?

Which of the following reactions would be the most spontaneous at 298 K?

Which of the following is the weakest oxidizing agent?

Identify the battery that is in most automobiles.

The electrolysis of molten AlCl3\mathrm { AlCl } _ { 3 }AlCl3​ for 4.25 hr with an electrical current of 25.0 A produces --------- ggg of aluminum metal.

What is the oxidizing agent in the redox reaction represented by the following cell notation? \quad\quad\quad Ni(s)| Ni2+(aq) ∥\|∥ Ag+(aq)| Ag(s)

Which of the following reactions would have the smallest value of K at 298 K?

Use the tabulated half-cell potentials to calculate the equilibrium constant (K)for the following balanced redox reaction at 25 °C: \quad\quad 3I2(s)+ 2Fe(s)→ 2Fe3+(aq)+ 6I- (aq) E°(I2/I-)= + 0.54 V and E°(Fe3+/Fe)= -0.036 V

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °: \quad\quad Cu(s)| Cu2+(aq,0.0032 mol L-1) ∥\|∥ Cu2+(aq,4.48 mol L-1)| Cu(s) E°(Cu2+/Cu)= +0.34 V

Which of the following is the weakest oxidizing agent?

Which of the following is the strongest reducing agent?

Which of the following is the strongest oxidizing agent?

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °: \quad\quad\quad Fe(s)| Fe3+(aq,0.0011 mol L-1) ∥\|∥ Fe3+(aq,2.33 mol L-1)| Fe(s) E°(Fe3+/Fe)= -0.036 V

Determine the cell notation for the redox reaction given below: \quad\quad\quad Sn(s)+ 2Ag+ (aq)? Sn2+(aq)+ 2Ag(s)

What is the shorthand notation that represents the following galvanic cell reaction? \quad\quad\quad 2Sn2+(aq)+ Cl2(g)→ 2Sn3+(aq)+ 2Cl-(aq)

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

The electrolysis of molten $\mathrm { AlCl } _ { 3 }$ for 4.25 hr with an electrical current of 25.0 A produces --------- $g$ of aluminum metal.

What is the oxidizing agent in the redox reaction represented by the following cell notation? $\quad$ $\quad$ $\quad$ Ni(s)| Ni²⁺(aq) $\|$ Ag⁺(aq)| Ag(s)

Use the tabulated half-cell potentials to calculate the equilibrium constant (K)for the following balanced redox reaction at 25 °C: $\quad$ $\quad$ 3I₂(s)+ 2Fe(s)→ 2Fe³⁺(aq)+ 6I^- (aq) E°(I₂/I^-)= + 0.54 V and E°(Fe³⁺/Fe)= -0.036 V

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °: $\quad$ $\quad$ Cu(s)| Cu²⁺(aq,0.0032 mol L^-1) $\|$ Cu²⁺(aq,4.48 mol L^-1)| Cu(s) E°(Cu²⁺/Cu)= +0.34 V

Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25 °: $\quad$ $\quad$ $\quad$ Fe(s)| Fe³⁺(aq,0.0011 mol L^-1) $\|$ Fe³⁺(aq,2.33 mol L^-1)| Fe(s) E°(Fe³⁺/Fe)= -0.036 V

Determine the cell notation for the redox reaction given below: $\quad$ $\quad$ $\quad$ Sn(s)+ 2Ag⁺ (aq)? Sn²⁺(aq)+ 2Ag(s)

What is the shorthand notation that represents the following galvanic cell reaction? $\quad$ $\quad$ $\quad$ 2Sn²⁺(aq)+ Cl₂(g)→ 2Sn³⁺(aq)+ 2Cl^-(aq)