Question 1

1V = ________.

Accepted Answer

A) 1 amp ∙ s 
B) 1 J/s 
C) 96485 C 
D) 1 J/C 
E) 1 C/J 
A) 1 amp ∙ s 
B) 1 J/s 
C) 96485 C 
D) 1 J/C 
E) 1 C/J

Question 2

How many minutes will it take to plate out 16.22 g of Al metal from a solution of Al3+ using a current of 14.6 amps in an electrolytic cell?

Accepted Answer

A) 53.0 
B) 66.2 
C) 153 
D) 199 
E) 11900 
A) 53.0 
B) 66.2 
C) 153 
D) 199 
E) 11900

Question 3

How many grams of copper will be plated out by a current of 2.3 A applied for 35 minutes to a 0.50 M solution of copper (II)sulfate?

Accepted Answer

A) 1.6 
B) 3.2 
C) 1.8 ×   
D) 3.6 ×   
E) 0.019 
A) 1.6 
B) 3.2 
C) 1.8 ×   
D) 3.6 ×   
E) 0.019

Question 4

Which of the following reactions will occur spontaneously as written?

Accepted Answer

A) Sn4+ (aq)+ Fe3+ (aq)→ Sn2+ (aq)+ Fe2+ (aq) 
B) 3Fe (s)+ 2Cr3+ (aq)→ 2Cr (s)+ 3Fe2+ (aq) 
C) Sn4+ (aq)+ Fe2+ (aq)→ Sn2+ (aq)+ Fe (s) 
D) 3Sn4+ (aq)+ 2Cr (s)→ 2Cr3+ (aq)+ 3Sn2+ (aq) 
E) 3Fe2+ (aq)→ Fe (s)+ 2Fe3+ (aq) 
A) Sn4+ (aq)+ Fe3+ (aq)→ Sn2+ (aq)+ Fe2+ (aq) 
B) 3Fe (s)+ 2Cr3+ (aq)→ 2Cr (s)+ 3Fe2+ (aq) 
C) Sn4+ (aq)+ Fe2+ (aq)→ Sn2+ (aq)+ Fe (s) 
D) 3Sn4+ (aq)+ 2Cr (s)→ 2Cr3+ (aq)+ 3Sn2+ (aq) 
E) 3Fe2+ (aq)→ Fe (s)+ 2Fe3+ (aq)

Question 5

The half-reaction occurring at the anode in the balanced reaction shown below is ________. 3MnO4- (aq)+ 24H+ (aq)+ 5Fe (s)→ 3Mn2+ (aq)+ 5Fe3+ (aq)+ 12H2O (l)

Accepted Answer

A) MnO4- (aq)+ 8H+ (aq)+ 5e- → Mn2+ (aq)+ 4H2O (l) 
B) 2MnO4- (aq)+ 12H+ (aq)+ 6e- → 2Mn2+ (aq)+ 3H2O (l) 
C) Fe (s)→ Fe3+ (aq)+ 3e- 
D) Fe (s)→ Fe2+ (aq)+ 2e- 
E) Fe2+ (aq)→ Fe3+ (aq)+ e- 
A) MnO4- (aq)+ 8H+ (aq)+ 5e- → Mn2+ (aq)+ 4H2O (l) 
B) 2MnO4- (aq)+ 12H+ (aq)+ 6e- → 2Mn2+ (aq)+ 3H2O (l) 
C) Fe (s)→ Fe3+ (aq)+ 3e- 
D) Fe (s)→ Fe2+ (aq)+ 2e- 
E) Fe2+ (aq)→ Fe3+ (aq)+ e-

Question 6

Based on standard reduction potentials,the most difficult species to reduce and the poorest oxidizing agent is ________.

Accepted Answer

The answer of Based on standard reduction potentials,the most difficult...

Question 7

Consider an electrochemical cell based on the reaction: 2H+ (aq)+ Sn (s)→ Sn2+ (aq)+ H2 (g)
Which of the following actions would not change the measured cell potential?

Accepted Answer

A) lowering the pH in the cathode compartment 
B) addition of more tin metal to the anode compartment 
C) increasing the tin (II)ion concentration in the anode compartment 
D) increasing the pressure of hydrogen gas in the cathode compartment 
E) Any of the above will change the measured cell potential. 
A) lowering the pH in the cathode compartment 
B) addition of more tin metal to the anode compartment 
C) increasing the tin (II)ion concentration in the anode compartment 
D) increasing the pressure of hydrogen gas in the cathode compartment 
E) Any of the above will change the measured cell potential.

Question 8

Calculate the number of grams of aluminum produced in 1.00 hour by electrolysis of AlCl3 at a current of 10.0 A.

Accepted Answer

Question 9

What is the correct coefficient for the electrons in the following half-reaction: Ni6+ + ___e- → Ni

Accepted Answer

A) 6 
B) 1 
C) 2 
D) 3 
E) 5 
A) 6 
B) 1 
C) 2 
D) 3 
E) 5

Question 10

Define the Nernst equation.

Accepted Answer

the depend

Question 11

What is the coefficient of the permanganate ion when the following equation is balanced?
MnO4- + Br- → Mn2+ + Br2 (acidic solution)

Accepted Answer

A) 1 
B) 2 
C) 3 
D) 5 
E) 4 
A) 1 
B) 2 
C) 3 
D) 5 
E) 4

Question 12

How much time (min)will it require to plate out 4.56 g of Ni metal from a solution of Ni2+ using a current of 35.5 amps in an electrolytic cell?

Accepted Answer

A) 4.55 
B) 3.52 
C) 211 
D) 7.04 
E) 422 
A) 4.55 
B) 3.52 
C) 211 
D) 7.04 
E) 422

Question 13

Which transformation could take place at the anode of an electrochemical cell?

Accepted Answer

A) Cr2O72- → Cr2+ 
B)    to   
C) O2 to H2O 
D) HAsO2 to As 
E) None of the above could take place at the anode. 
A) Cr2O72- → Cr2+ 
B)    to   
C) O2 to H2O 
D) HAsO2 to As 
E) None of the above could take place at the anode.

Question 14

What is the anode in an alkaline battery?

Accepted Answer

A) MnO2 
B) KOH 
C) Zn powder 
D) Mn2O3 
E) Pt 
A) MnO2 
B) KOH 
C) Zn powder 
D) Mn2O3 
E) Pt

Question 15

What is the oxidation number of sulfur in the S2O32- ion?

Accepted Answer

A) +2 
B) +1 
C) 0 
D) -1 
E) -2 
A) +2 
B) +1 
C) 0 
D) -1 
E) -2

Question 16

Which transformation could take place at the cathode of an electrochemical cell?

Accepted Answer

A) MnO2 → MnO4- 
B) Br2 → BrO3- 
C) NO → HNO2 
D) HSO4- → H2SO3 
E) Mn2+ → MnO4- 
A) MnO2 → MnO4- 
B) Br2 → BrO3- 
C) NO → HNO2 
D) HSO4- → H2SO3 
E) Mn2+ → MnO4-

Question 17

In the electrochemical cell using the redox reaction below,the oxidation half reaction is ________.   (aq)+ Fe (s)→   (aq)+   (aq)

Accepted Answer

A) Sn4+ + 2e- → Sn2+ 
B) Fe → Fe2+ + 2e- 
C) Sn4+ → Sn2+ + 2e- 
D) Fe + 2e- → Fe2+ 
E) Fe +   →   
A) Sn4+ + 2e- → Sn2+ 
B) Fe → Fe2+ + 2e- 
C) Sn4+ → Sn2+ + 2e- 
D) Fe + 2e- → Fe2+ 
E) Fe +   →

Question 18

The half-reaction occurring at the cathode in the balanced reaction shown below is ________. 3MnO4- (aq)+ 24H+ (aq)+ 5Fe (s)→ 3Mn2+ (aq)+ 5Fe3+ (aq)+ 12H2O (l)

Accepted Answer

A) MnO4- (aq)+ 8H+ (aq)+ 5   → Mn2+ (aq)+ 4H2O (l) 
B) 2MnO4- (aq)+ 12H+ (aq)+ 6e- → 2Mn2+ (aq)+ 3H2O (l) 
C) Fe (s)→ Fe3+ (aq)+ 3e- 
D) Fe (s)→ Fe2+ (aq)+ 2e- 
E) Fe2+ (aq)→ Fe3+ (aq)+ e- 
A) MnO4- (aq)+ 8H+ (aq)+ 5   → Mn2+ (aq)+ 4H2O (l) 
B) 2MnO4- (aq)+ 12H+ (aq)+ 6e- → 2Mn2+ (aq)+ 3H2O (l) 
C) Fe (s)→ Fe3+ (aq)+ 3e- 
D) Fe (s)→ Fe2+ (aq)+ 2e- 
E) Fe2+ (aq)→ Fe3+ (aq)+ e-

Question 19

In the galvanic cell using the redox reaction below,the reduction half-reaction is ________. Zn (s)+   (aq)→   (aq)+ Cu (s)

Accepted Answer

A) Cu2+ + 2e- → Cu 
B) Zn → Zn2+ + 2e- 
C) Cu2+ → Cu + 2e- 
D) Zn + 2e- → Zn2+ 
A) Cu2+ + 2e- → Cu 
B) Zn → Zn2+ + 2e- 
C) Cu2+ → Cu + 2e- 
D) Zn + 2e- → Zn2+

Question 20

What is the oxidation number of phosphorous in the PH3 molecule?

Accepted Answer

A) -3 
B) -4 
C) -5 
D) +1 
E) 0 
A) -3 
B) -4 
C) -5 
D) +1 
E) 0

Exam 20: Electrochemistry

1V = ________.

How many minutes will it take to plate out 16.22 g of Al metal from a solution of Al3+ using a current of 14.6 amps in an electrolytic cell?

How many grams of copper will be plated out by a current of 2.3 A applied for 35 minutes to a 0.50 M solution of copper (II)sulfate?

Which of the following reactions will occur spontaneously as written?

The half-reaction occurring at the anode in the balanced reaction shown below is ________. 3MnO4- (aq)+ 24H+ (aq)+ 5Fe (s)→ 3Mn2+ (aq)+ 5Fe3+ (aq)+ 12H2O (l)

Based on standard reduction potentials,the most difficult species to reduce and the poorest oxidizing agent is ________.

Consider an electrochemical cell based on the reaction: 2H+ (aq)+ Sn (s)→ Sn2+ (aq)+ H2 (g) Which of the following actions would not change the measured cell potential?

Calculate the number of grams of aluminum produced in 1.00 hour by electrolysis of AlCl3 at a current of 10.0 A.

What is the correct coefficient for the electrons in the following half-reaction: Ni6+ + ___e- → Ni

Define the Nernst equation.

What is the coefficient of the permanganate ion when the following equation is balanced? MnO4- + Br- → Mn2+ + Br2 (acidic solution)

How much time (min)will it require to plate out 4.56 g of Ni metal from a solution of Ni2+ using a current of 35.5 amps in an electrolytic cell?

Which transformation could take place at the anode of an electrochemical cell?

What is the anode in an alkaline battery?

What is the oxidation number of sulfur in the S2O32- ion?

Which transformation could take place at the cathode of an electrochemical cell?

In the electrochemical cell using the redox reaction below,the oxidation half reaction is ________. (aq)+ Fe (s)→ (aq)+ (aq)

The half-reaction occurring at the cathode in the balanced reaction shown below is ________. 3MnO4- (aq)+ 24H+ (aq)+ 5Fe (s)→ 3Mn2+ (aq)+ 5Fe3+ (aq)+ 12H2O (l)

In the galvanic cell using the redox reaction below,the reduction half-reaction is ________. Zn (s)+ (aq)→ (aq)+ Cu (s)

What is the oxidation number of phosphorous in the PH3 molecule?

Introduction: Matter, energy, and Measurement

Atoms, molecules, and Ions

Chemical Reactions and Reaction Stoichiometry

Reactions in Aqueous Solution

Thermochemistry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Molecular Geometry and Bonding Theories

Gases

Liquids and Intermolecular Forces

Solids and Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Additional Aspects of Aqueous Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Nuclear Chemistry

Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

The Chemistry of Life: Organic and Biological Chemistry

Filters

How many minutes will it take to plate out 16.22 g of Al metal from a solution of Al³⁺ using a current of 14.6 amps in an electrolytic cell?

The half-reaction occurring at the anode in the balanced reaction shown below is ________. 3MnO₄^- (aq)+ 24H⁺ (aq)+ 5Fe (s)→ 3Mn²⁺ (aq)+ 5Fe³⁺ (aq)+ 12H₂O (l)

Consider an electrochemical cell based on the reaction: 2H⁺ (aq)+ Sn (s)→ Sn²⁺ (aq)+ H₂ (g) Which of the following actions would not change the measured cell potential?

Calculate the number of grams of aluminum produced in 1.00 hour by electrolysis of AlCl₃ at a current of 10.0 A.

What is the correct coefficient for the electrons in the following half-reaction: Ni⁶⁺ + ___e^- → Ni

What is the coefficient of the permanganate ion when the following equation is balanced? MnO₄^- + Br^- → Mn²⁺ + Br₂ (acidic solution)

How much time (min)will it require to plate out 4.56 g of Ni metal from a solution of Ni²⁺ using a current of 35.5 amps in an electrolytic cell?

What is the oxidation number of sulfur in the S₂O₃^2- ion?

The half-reaction occurring at the cathode in the balanced reaction shown below is ________. 3MnO₄^- (aq)+ 24H⁺ (aq)+ 5Fe (s)→ 3Mn²⁺ (aq)+ 5Fe³⁺ (aq)+ 12H₂O (l)

What is the oxidation number of phosphorous in the PH₃ molecule?