Question 1

Which element is oxidized in the reaction below? Fe+2 + H+ + Cr2O7-2 → Fe+3 + Cr+3 + H2O

Accepted Answer

A) Fe 
B) Cr 
C) O 
D) H 
A) Fe 
B) Cr 
C) O 
D) H

Question 2

What is the coefficient of the dichromate ion when the following equation is balanced? Fe2+ + Cr2O72- → Fe3+ + Cr3+ (acidic solution)

Accepted Answer

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

Question 3

At constant temperature and pressure the Gibbs free energy value is a measure of the __________ of a process.

Accepted Answer

The answer of At constant temperature and pressure the Gibbs...

Question 4

Which of the following reactions will occur spontaneously as written?

Accepted Answer

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

Question 5

In a voltaic cell, electrons flow from the __________ to the __________.

Accepted Answer

A) salt bride, anode 
B) anode, salt bridge 
C) cathode, anode 
D) salt bridge, cathode 
E) anode, cathode 
A) salt bride, anode 
B) anode, salt bridge 
C) cathode, anode 
D) salt bridge, cathode 
E) anode, cathode

Question 6

Which element is reduced in the reaction below? Fe(CO)5 (l)+ 2HI (g)→ Fe(CO)4I2 (s)+ CO (g)+ H2 (g)

Accepted Answer

A) Fe 
B) C 
C) O 
D) H 
E) I 
A) Fe 
B) C 
C) O 
D) H 
E) I

Question 7

Which substance is the reducing agent in the following reaction? Fe2S3 + 12HNO3 → 2Fe(NO3)3 + 3S + 6NO2 + 6H2O

Accepted Answer

A) HNO3 
B) S 
C) NO2 
D) Fe2S3 
E) H2O 
A) HNO3 
B) S 
C) NO2 
D) Fe2S3 
E) H2O

Question 8

What is the oxidation number of bromine in the BrO3- ion?

Accepted Answer

A) -1 
B) +1 
C) +3 
D) +5 
E) +7 
A) -1 
B) +1 
C) +3 
D) +5 
E) +7

Question 9

A voltaic cell is constructed with two Zn2+-Zn electrodes, where the half-reaction is Zn2+ + 2e- → Zn (s)E° = -0.763 V
The concentrations of zinc ion in the two compartments are 5.50 M and 1.11 × 10-2 M, respectively. The cell emf is __________ V.

Accepted Answer

A) -1.54 × 10-3 
B) -378 
C) 0.0798 
D) 0.160 
E) -0.761 
A) -1.54 × 10-3 
B) -378 
C) 0.0798 
D) 0.160 
E) -0.761

Question 10

Which substance is the reducing agent in the reaction below? Pb + PbO2 + 2H2SO4 → 2PbSO4 + 2H2O

Accepted Answer

A) Pb 
B) H2SO4 
C) PbO2 
D) PbSO4 
E) H2O 
A) Pb 
B) H2SO4 
C) PbO2 
D) PbSO4 
E) H2O

Question 11

Cathodic protection of a metal pipe against corrosion usually entails

Accepted Answer

A) attaching an active metal to make the pipe the anode in an electrochemical cell. 
B) coating the pipe with another metal whose standard reduction potential is less negative than that of the pipe. 
C) attaching an active metal to make the pipe the cathode in an electrochemical cell. 
D) attaching a dry cell to reduce any metal ions which might be formed. 
E) coating the pipe with a fluoropolymer to act as a source of fluoride ion (since the latter is so hard to oxidize). 
A) attaching an active metal to make the pipe the anode in an electrochemical cell. 
B) coating the pipe with another metal whose standard reduction potential is less negative than that of the pipe. 
C) attaching an active metal to make the pipe the cathode in an electrochemical cell. 
D) attaching a dry cell to reduce any metal ions which might be formed. 
E) coating the pipe with a fluoropolymer to act as a source of fluoride ion (since the latter is so hard to oxidize).

Question 12

Which substance is serving as the reducing agent in the following reaction? 14H+ + Cr2O72- + 3Ni → 3Ni2+ + 2Cr3+ + 7H2O

Accepted Answer

A) Ni 
B) H+ 
C) Cr2O72- 
D) H2O 
E) Ni2+ 
A) Ni 
B) H+ 
C) Cr2O72- 
D) H2O 
E) Ni2+

Question 13

The standard emf for the cell using the overall cell reaction below is +0.48 V: Zn (s)+ Ni2+ (aq)→ Zn2+ (aq)+ Ni (s)
The emf generated by the cell when [Ni2+] = 2.50 M and [Zn2+] = 0.100 M is ________ V.

Accepted Answer

A) 0.40 
B) 0.50 
C) 0.52 
D) 0.56 
E) 0.44 
A) 0.40 
B) 0.50 
C) 0.52 
D) 0.56 
E) 0.44

Question 14

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 15

Which element is oxidized in the reaction below? Fe(CO)5 (l)+ 2HI (g)→ Fe(CO)4I2 (s)+ CO (g)+ H2 (g)

Accepted Answer

A) Fe 
B) C 
C) O 
D) H 
E) I 
A) Fe 
B) C 
C) O 
D) H 
E) I

Question 16

Which element is reduced in the reaction below? Fe+2  + H+ + Cr2O7-2 → Fe+3 + Cr+3 + H2O

Accepted Answer

A) Fe 
B) Cr 
C) O 
D) H 
A) Fe 
B) Cr 
C) O 
D) H

Question 17

The standard reduction potential of X is 1.23 V and that of Y is -0.44 V therefore X is oxidized by Y.

Accepted Answer

A) True 
 B)False

Question 18

How many seconds are required to produce 1.0 g of silver metal by the electrolysis of a AgNO3 solution using a current of 5.0 amps?

Accepted Answer

A) 4.5 × 103 
B) 3.2 × 103 
C) 180 
D) 3.7 × 10-5 
E) 360 
A) 4.5 × 103 
B) 3.2 × 103 
C) 180 
D) 3.7 × 10-5 
E) 360

Question 19

Which one of the following types of elements is most likely to be a good oxidizing agent?

Accepted Answer

A) alkali metals 
B) lanthanides 
C) alkaline earth elements 
D) transition elements 
E) halogens 
A) alkali metals 
B) lanthanides 
C) alkaline earth elements 
D) transition elements 
E) halogens

Question 20

The reduction half reaction occurring in the standard hydrogen electrode is __________.

Accepted Answer

A) H2 (g, 1 atm)→ 2H+ (aq, 1M)+ 2e- 
B) 2H+ (aq)+ 2OH- → H2O (l) 
C) O2 (g)+ 4H+ (aq)+ 4e- → 2H2O (l) 
D) 2H+ (aq, 1M)+ 2e- → H2 (g, 1 atm) 
E) 2H+ (aq, 1M)+ Cl2 (aq)→ 2HCl (aq) 
A) H2 (g, 1 atm)→ 2H+ (aq, 1M)+ 2e- 
B) 2H+ (aq)+ 2OH- → H2O (l) 
C) O2 (g)+ 4H+ (aq)+ 4e- → 2H2O (l) 
D) 2H+ (aq, 1M)+ 2e- → H2 (g, 1 atm) 
E) 2H+ (aq, 1M)+ Cl2 (aq)→ 2HCl (aq)

Exam 20: Electrochemistry

Which element is oxidized in the reaction below? Fe+2 + H+ + Cr2O7-2 → Fe+3 + Cr+3 + H2O

What is the coefficient of the dichromate ion when the following equation is balanced? Fe2+ + Cr2O72- → Fe3+ + Cr3+ (acidic solution)

At constant temperature and pressure the Gibbs free energy value is a measure of the __________ of a process.

Which of the following reactions will occur spontaneously as written?

In a voltaic cell, electrons flow from the __________ to the __________.

Which element is reduced in the reaction below? Fe(CO)5 (l)+ 2HI (g)→ Fe(CO)4I2 (s)+ CO (g)+ H2 (g)

Which substance is the reducing agent in the following reaction? Fe2S3 + 12HNO3 → 2Fe(NO3)3 + 3S + 6NO2 + 6H2O

What is the oxidation number of bromine in the BrO3- ion?

A voltaic cell is constructed with two Zn2+-Zn electrodes, where the half-reaction is Zn2+ + 2e- → Zn (s)E° = -0.763 V The concentrations of zinc ion in the two compartments are 5.50 M and 1.11 × 10-2 M, respectively. The cell emf is __________ V.

Which substance is the reducing agent in the reaction below? Pb + PbO2 + 2H2SO4 → 2PbSO4 + 2H2O

Cathodic protection of a metal pipe against corrosion usually entails

Which substance is serving as the reducing agent in the following reaction? 14H+ + Cr2O72- + 3Ni → 3Ni2+ + 2Cr3+ + 7H2O

The standard emf for the cell using the overall cell reaction below is +0.48 V: Zn (s)+ Ni2+ (aq)→ Zn2+ (aq)+ Ni (s) The emf generated by the cell when [Ni2+] = 2.50 M and [Zn2+] = 0.100 M is ________ V.

1V = __________.

Which element is oxidized in the reaction below? Fe(CO)5 (l)+ 2HI (g)→ Fe(CO)4I2 (s)+ CO (g)+ H2 (g)

Which element is reduced in the reaction below? Fe+2 + H+ + Cr2O7-2 → Fe+3 + Cr+3 + H2O

The standard reduction potential of X is 1.23 V and that of Y is -0.44 V therefore X is oxidized by Y.

How many seconds are required to produce 1.0 g of silver metal by the electrolysis of a AgNO3 solution using a current of 5.0 amps?

Which one of the following types of elements is most likely to be a good oxidizing agent?

The reduction half reaction occurring in the standard hydrogen electrode is __________.

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

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

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Chemistry of the Nonmetals

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Which element is oxidized in the reaction below? Fe⁺² + H⁺ + Cr₂O₇^-2 → Fe⁺³ + Cr⁺³ + H₂O

What is the coefficient of the dichromate ion when the following equation is balanced? Fe²⁺ + Cr₂O₇^2- → Fe³⁺ + Cr³⁺ (acidic solution)

In a voltaic cell, electrons flow from the to the .

Which element is reduced in the reaction below? Fe(CO)₅ (l)+ 2HI (g)→ Fe(CO)₄I₂ (s)+ CO (g)+ H₂ (g)

Which substance is the reducing agent in the following reaction? Fe₂S₃ + 12HNO₃ → 2Fe(NO₃)₃ + 3S + 6NO₂ + 6H₂O

What is the oxidation number of bromine in the BrO₃^- ion?

A voltaic cell is constructed with two Zn²⁺-Zn electrodes, where the half-reaction is Zn²⁺ + 2e^- → Zn (s)E° = -0.763 V The concentrations of zinc ion in the two compartments are 5.50 M and 1.11 × 10^-2 M, respectively. The cell emf is __________ V.

Which substance is the reducing agent in the reaction below? Pb + PbO₂ + 2H₂SO₄ → 2PbSO₄ + 2H₂O

Which substance is serving as the reducing agent in the following reaction? 14H⁺ + Cr₂O₇^2- + 3Ni → 3Ni²⁺ + 2Cr³⁺ + 7H₂O

The standard emf for the cell using the overall cell reaction below is +0.48 V: Zn (s)+ Ni²⁺ (aq)→ Zn²⁺ (aq)+ Ni (s) The emf generated by the cell when [Ni²⁺] = 2.50 M and [Zn²⁺] = 0.100 M is ________ V.

Which element is oxidized in the reaction below? Fe(CO)₅ (l)+ 2HI (g)→ Fe(CO)₄I₂ (s)+ CO (g)+ H₂ (g)

Which element is reduced in the reaction below? Fe⁺² + H⁺ + Cr₂O₇^-2 → Fe⁺³ + Cr⁺³ + H₂O

How many seconds are required to produce 1.0 g of silver metal by the electrolysis of a AgNO₃ solution using a current of 5.0 amps?