Question 1

Electrolysis involves using an external current to drive an electrochemical reaction in a non-spontaneous direction.

Accepted Answer

A) True 
 B)False

Question 2

Electrolysis can be used to electroplate metals onto surfaces.

Accepted Answer

A) True 
 B)False

Question 3

The formation of thin layers of material on the electrodes of a secondary cell will result in:

Accepted Answer

A)  an increase in the EMF of the battery. 
B)  formation of explosive hydrates. 
C)  shorter periods of usefulness between recharging sessions. 
D)  the creation of j-p junction gaps at the electrode surfaces. 
A)  an increase in the EMF of the battery. 
B)  formation of explosive hydrates. 
C)  shorter periods of usefulness between recharging sessions. 
D)  the creation of j-p junction gaps at the electrode surfaces.

Question 4

All dry cell batteries are rechargeable.

Accepted Answer

A) True 
 B)False

Question 5

What is the E value for the Galvanic cell formed from these two half-reactions at these concentrations?

Accepted Answer

A)  1.90 V 
B)  1.95 V 
C)  1.99 V 
D)  2.20 V 
A)  1.90 V 
B)  1.95 V 
C)  1.99 V 
D)  2.20 V

Question 6

Copper has a greater tendency to corrode than does zinc.

Accepted Answer

A) True 
 B)False

Question 7

An oxidation occurs at the ____ of a Galvanic cell.

Accepted Answer

A)  intersection 
B)  anode 
C)  p-n junction 
D)  cathode 
A)  intersection 
B)  anode 
C)  p-n junction 
D)  cathode

Question 8

What is the E value for the Galvanic cell formed from these two half-reactions at these concentrations?

Accepted Answer

A)  1.00 V 
B)  1.12 V 
C)  1.24 V 
D)  0.36 V 
A)  1.00 V 
B)  1.12 V 
C)  1.24 V 
D)  0.36 V

Question 9

Which mechanism is most energy efficient?

Accepted Answer

A)  internal combustion motor 
B)  a voltaic fuel cell 
C)  electricity from coal fired plants 
A)  internal combustion motor 
B)  a voltaic fuel cell 
C)  electricity from coal fired plants

Question 10

The Nernst equation describes the pH required to convert electrolytic reactions into spontaneous Galvanic cells.

Accepted Answer

A) True 
 B)False

Question 11

The species undergoing reduction is referred to as the oxidizing agent.

Accepted Answer

A) True 
 B)False

Question 12

Single use, non-rechargeable batteries are referred to as:

Accepted Answer

A)  primary cells 
B)  secondary cells 
C)  tertiary cells 
D)  electrolytic cells 
A)  primary cells 
B)  secondary cells 
C)  tertiary cells 
D)  electrolytic cells

Question 13

How long will it take to collect 1.0 L of H2 (g) at STP in the electrolysis of 2.0 M HCl with a current of 4.25 A?

Accepted Answer

A)  15 min 
B)  34 min 
C)  2.8 hr 
D)  11 hr 
A)  15 min 
B)  34 min 
C)  2.8 hr 
D)  11 hr

Question 14

The kinetics of uniform corrosion will speed up considerably in the presence of good electrical conducting salts such as NaCl

Accepted Answer

A) True 
 B)False

Question 15

The SHE is assigned a voltage of ____ V.

Accepted Answer

A)  − 1.000 
B)  1.000 
C)  0.150 
D)  0.000 
A)  − 1.000 
B)  1.000 
C)  0.150 
D)  0.000

Question 16

What is the E0 value for the Galvanic cell formed from these two half-reactions?

Accepted Answer

A)  −1 .43 V 
B)  +1.43 V 
C)  −0 .93 V 
D)  +0.93 V 
A)  −1 .43 V 
B)  +1.43 V 
C)  −0 .93 V 
D)  +0.93 V

Question 17

In balancing electrochemical half-reactions in acidic media, one can assume an excess of both water and OH-.

Accepted Answer

A) True 
 B)False

Question 18

Identify the correct balanced chemical equation for the cell:

Accepted Answer

A)  Al( s ) + Hg2+( aq ) → Al3+( aq ) + Hg( l ) 
B)  2 Al( s ) + Hg2+( aq ) → 2 Al3+( aq ) + Hg( l ) 
C)  Al( s ) + 3 Hg2+( aq ) → Al3+( aq ) + 3 Hg( l ) 
D)  2 Al( s ) + 3 Hg2+( aq ) → 2 Al3+( aq ) + 3 Hg( l ) 
A)  Al( s ) + Hg2+( aq ) → Al3+( aq ) + Hg( l ) 
B)  2 Al( s ) + Hg2+( aq ) → 2 Al3+( aq ) + Hg( l ) 
C)  Al( s ) + 3 Hg2+( aq ) → Al3+( aq ) + 3 Hg( l ) 
D)  2 Al( s ) + 3 Hg2+( aq ) → 2 Al3+( aq ) + 3 Hg( l )

Question 19

The salt bridge between 1/2 reactions maintains the electrical balance of a Galvanic cell. This bridge is filled with:

Accepted Answer

A)  strong electrolytes. 
B)  inert carbon. 
C)  weak electrolytes. 
D)  interstitial membranes. 
A)  strong electrolytes. 
B)  inert carbon. 
C)  weak electrolytes. 
D)  interstitial membranes.

Question 20

What is the oxidation number of Cl in HClO4?

Accepted Answer

A)  1+ 
B)  2+ 
C)  7+ 
D)  8+ 
A)  1+ 
B)  2+ 
C)  7+ 
D)  8+

Electrolysis involves using an external current to drive an electrochemical reaction in a non-spontaneous direction.

Electrolysis can be used to electroplate metals onto surfaces.

The formation of thin layers of material on the electrodes of a secondary cell will result in:

All dry cell batteries are rechargeable.

What is the E value for the Galvanic cell formed from these two half-reactions at these concentrations?

Copper has a greater tendency to corrode than does zinc.

An oxidation occurs at the ____ of a Galvanic cell.

What is the E value for the Galvanic cell formed from these two half-reactions at these concentrations?

Which mechanism is most energy efficient?

The Nernst equation describes the pH required to convert electrolytic reactions into spontaneous Galvanic cells.

The species undergoing reduction is referred to as the oxidizing agent.

Single use, non-rechargeable batteries are referred to as:

How long will it take to collect 1.0 L of H₂ (g) at STP in the electrolysis of 2.0 M HCl with a current of 4.25 A?

The kinetics of uniform corrosion will speed up considerably in the presence of good electrical conducting salts such as NaCl

The SHE is assigned a voltage of ____ V.

What is the E⁰ value for the Galvanic cell formed from these two half-reactions?

In balancing electrochemical half-reactions in acidic media, one can assume an excess of both water and OH^-.

Identify the correct balanced chemical equation for the cell:

The salt bridge between 1/2 reactions maintains the electrical balance of a Galvanic cell. This bridge is filled with:

What is the oxidation number of Cl in HClO₄?

Introduction to Chemistry

Atoms and Molecules

Molecules Moles Chemical Equations

Stoichiometry

Gases

The Periodic Table and Atomic Structure

Chemical Bonding and Molecular Structure

Molecules and Materials

Energy and Chemistry

Entropy and the Second Law of Thermodynamics

Chemical Kinetics

Chemical Equilibrium

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Exam 13: Electrochemistry

Electrolysis involves using an external current to drive an electrochemical reaction in a non-spontaneous direction.

Electrolysis can be used to electroplate metals onto surfaces.

The formation of thin layers of material on the electrodes of a secondary cell will result in:

All dry cell batteries are rechargeable.

What is the E value for the Galvanic cell formed from these two half-reactions at these concentrations?

Copper has a greater tendency to corrode than does zinc.

An oxidation occurs at the ____ of a Galvanic cell.

What is the E value for the Galvanic cell formed from these two half-reactions at these concentrations?

Which mechanism is most energy efficient?

The Nernst equation describes the pH required to convert electrolytic reactions into spontaneous Galvanic cells.

The species undergoing reduction is referred to as the oxidizing agent.

Single use, non-rechargeable batteries are referred to as:

How long will it take to collect 1.0 L of H2 (g) at STP in the electrolysis of 2.0 M HCl with a current of 4.25 A?

The kinetics of uniform corrosion will speed up considerably in the presence of good electrical conducting salts such as NaCl

The SHE is assigned a voltage of ____ V.

What is the E0 value for the Galvanic cell formed from these two half-reactions?

In balancing electrochemical half-reactions in acidic media, one can assume an excess of both water and OH-.

Identify the correct balanced chemical equation for the cell:

The salt bridge between 1/2 reactions maintains the electrical balance of a Galvanic cell. This bridge is filled with:

What is the oxidation number of Cl in HClO4?

Introduction to Chemistry

Atoms and Molecules

Molecules Moles Chemical Equations

Stoichiometry

Gases

The Periodic Table and Atomic Structure

Chemical Bonding and Molecular Structure

Molecules and Materials

Energy and Chemistry

Entropy and the Second Law of Thermodynamics

Chemical Kinetics

Chemical Equilibrium

Filters

How long will it take to collect 1.0 L of H₂ (g) at STP in the electrolysis of 2.0 M HCl with a current of 4.25 A?

What is the E⁰ value for the Galvanic cell formed from these two half-reactions?

In balancing electrochemical half-reactions in acidic media, one can assume an excess of both water and OH^-.

What is the oxidation number of Cl in HClO₄?