Question 1

The study of the relationships between electron flow and redox reactions is called

Accepted Answer

A)  nuclear chemistry. 
B)  electrochemistry. 
C)  thermodynamics. 
D)  electrodynamics. 
E)  inorganic chemistry. 
A)  nuclear chemistry. 
B)  electrochemistry. 
C)  thermodynamics. 
D)  electrodynamics. 
E)  inorganic chemistry.

Question 2

In the reaction shown below, ____ is the oxidizing agent and ____ the reducing agent.

Accepted Answer

A)  Zn2+; H2 
B)  Zn; H+ 
C)  H2; Zn2+ 
D)  H+; Zn2+ 
E)  H+; Zn 
A)  Zn2+; H2 
B)  Zn; H+ 
C)  H2; Zn2+ 
D)  H+; Zn2+ 
E)  H+; Zn

Question 3

Calculate the value of Ecell for a zinc-platinum electrochemical cell when the concentration of Pt2+(aq) is 0.050 M and the concentration of Zn2+(aq) is 1.1 M. E$\circ$cell = 1.96 V under standard conditions. Pt is the less active metal.

Accepted Answer

A)  2.04 V 
B)  2.00 V 
C)  1.96 V 
D)  1.92 V 
E)  1.88 V 
A)  2.04 V 
B)  2.00 V 
C)  1.96 V 
D)  1.92 V 
E)  1.88 V

Question 4

A fuel cell is

Accepted Answer

A)  an electrolytic cell that is used to supply electrical power 
B)  an electrochemical cell that converts chemical energy directly into electricity 
C)  a cell in which a hydrogen-oxygen is ignited to produced electricity 
D)  typically not susceptible to contamination 
E)  currently both technically feasible and commercially viable as a source of electrical power 
A)  an electrolytic cell that is used to supply electrical power 
B)  an electrochemical cell that converts chemical energy directly into electricity 
C)  a cell in which a hydrogen-oxygen is ignited to produced electricity 
D)  typically not susceptible to contamination 
E)  currently both technically feasible and commercially viable as a source of electrical power

Question 5

Exhibit 18-2 Use this list of half-reactions to answer the following question(s).
  Refer to Exhibit 18-2. The strongest reducing agent in the table is

Accepted Answer

A)  Al(s). 
B)  Al3+(aq). 
C)  H+(aq). 
D)  MnO4-(aq). 
E)  Mn2+(aq). 
A)  Al(s). 
B)  Al3+(aq). 
C)  H+(aq). 
D)  MnO4-(aq). 
E)  Mn2+(aq).

Question 6

Exhibit 18-2 Use this list of half-reactions to answer the following question(s).
  Refer to Exhibit 18-2. The potential for the product-favored reaction involving aluminum and copper metals, Al3+(aq) and Cu2+(aq), is

Accepted Answer

A)  2.17 V. 
B)  2.00 V. 
C)  1.79 V. 
D)  1.32 V. 
E)  1.15 V. 
A)  2.17 V. 
B)  2.00 V. 
C)  1.79 V. 
D)  1.32 V. 
E)  1.15 V.

Question 7

The relationship between Gibbs free energy and E$\circ$cell is DG$\circ$ =

Accepted Answer

A)    
B)    
C)  -nFE$\circ$cell. 
D)  nFE$\circ$cell. 
E)  -RT ln K. 
A)    
B)    
C)  -nFE$\circ$cell. 
D)  nFE$\circ$cell. 
E)  -RT ln K.

Question 8

Explain, with reference to the Nernst equation, how it is possible for a cell to have a positive cell potential under standard conditions, but a negative cell potential under other conditions.

Accepted Answer

The value of E_cell

Question 9

Balance the following redox equation.
   The oxidation process is clearly

Accepted Answer

@#IMG-DLM& The reduction can be balanced

Question 10

The value of E$\circ$cell for an aluminum-nickel electrochemical cell is +1.41 V at 25$\circ$C. Calculate the value of DG$\circ$ for this cell under standard conditions.

Accepted Answer

A)  -816 kJ 
B)  -680 kJ 
C)  -272 kJ 
D)  +403 kJ 
E)  +680 kJ 
A)  -816 kJ 
B)  -680 kJ 
C)  -272 kJ 
D)  +403 kJ 
E)  +680 kJ

Question 11

A secondary cell is one which ____; this is possible because ____.

Accepted Answer

A)  is driven by a primary cell; the cell reactions are coupled 
B)  is disposable without harming the environment; no mercury is used 
C)  is rechargeable; the cell reaction is reversible 
D)  has double the lifetime of a primary cell; two primary cells are placed in parallel 
E)  has double the voltage of a primary cell; two primary cells are placed in series 
A)  is driven by a primary cell; the cell reactions are coupled 
B)  is disposable without harming the environment; no mercury is used 
C)  is rechargeable; the cell reaction is reversible 
D)  has double the lifetime of a primary cell; two primary cells are placed in parallel 
E)  has double the voltage of a primary cell; two primary cells are placed in series

Question 12

Which statement about lead storage batteries is not correct?

Accepted Answer

A)  The value of E$\circ$cell is slightly more than 2 V 
B)  The anode reaction involves the conversion of Pb to Pb2+ 
C)  Nitric acid serves as the electrolyte 
D)  The cathode reaction involves the conversion of Pb4+ to Pb2+ 
E)  In order to provide 12 volts, the battery consists of six cells 
A)  The value of E$\circ$cell is slightly more than 2 V 
B)  The anode reaction involves the conversion of Pb to Pb2+ 
C)  Nitric acid serves as the electrolyte 
D)  The cathode reaction involves the conversion of Pb4+ to Pb2+ 
E)  In order to provide 12 volts, the battery consists of six cells

Question 13

The unit used to measure electrical current is the

Accepted Answer

A)  ampere 
B)  coulomb 
C)  faraday 
D)  joule 
E)  volt 
A)  ampere 
B)  coulomb 
C)  faraday 
D)  joule 
E)  volt

Question 14

Which compound contains the atom with the highest oxidation number?

Accepted Answer

A)  FeCl3 
B)  SnH4 
C)  NaClO4 
D)  CrO3 
E)  H2O2 
A)  FeCl3 
B)  SnH4 
C)  NaClO4 
D)  CrO3 
E)  H2O2

The study of the relationships between electron flow and redox reactions is called

In the reaction shown below, is the oxidizing agent and the reducing agent.

Calculate the value of E_cell for a zinc-platinum electrochemical cell when the concentration of Pt²⁺(aq) is 0.050 M and the concentration of Zn²⁺(aq) is 1.1 M. E^$\circ$_cell = 1.96 V under standard conditions. Pt is the less active metal.

A fuel cell is

Exhibit 18-2 Use this list of half-reactions to answer the following question(s). Refer to Exhibit 18-2. The strongest reducing agent in the table is

Exhibit 18-2 Use this list of half-reactions to answer the following question(s). Refer to Exhibit 18-2. The potential for the product-favored reaction involving aluminum and copper metals, Al³⁺(aq) and Cu²⁺(aq), is

The relationship between Gibbs free energy and E^$\circ$_cell is DG^$\circ$ =

Explain, with reference to the Nernst equation, how it is possible for a cell to have a positive cell potential under standard conditions, but a negative cell potential under other conditions.

Balance the following redox equation. The oxidation process is clearly

The value of E^$\circ$_cell for an aluminum-nickel electrochemical cell is +1.41 V at 25^$\circ$C. Calculate the value of DG^$\circ$ for this cell under standard conditions.

A secondary cell is one which ; this is possible because .

Which statement about lead storage batteries is not correct?

The unit used to measure electrical current is the

Which compound contains the atom with the highest oxidation number?

The Nature of Chemistry

Atoms and Elements

Chemical Compounds

Quantities of Reactants and Products

Chemical Reactions

Energy and Chemical Reactions

Electron Configurations and the Periodic Table

Covalent Bonding

Molecular Structure

Gases and the Atmosphere

Liquids, Solids, and Materials

Chemical Kinetics: Rates of Reactions

Chemical Equilibrium

The Chemistry of Solutes and Solutions

Acids and Bases

Additional Aqueous Equilibria

Thermodynamics: Directionality of Chemical Reactions

Nuclear Chemistry

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Exam 18: Electrochemistry and Its Applications

The study of the relationships between electron flow and redox reactions is called

In the reaction shown below, ____ is the oxidizing agent and ____ the reducing agent.

Calculate the value of Ecell for a zinc-platinum electrochemical cell when the concentration of Pt2+(aq) is 0.050 M and the concentration of Zn2+(aq) is 1.1 M. E ∘\circ∘ cell = 1.96 V under standard conditions. Pt is the less active metal.

A fuel cell is

Exhibit 18-2 Use this list of half-reactions to answer the following question(s). Refer to Exhibit 18-2. The strongest reducing agent in the table is

Exhibit 18-2 Use this list of half-reactions to answer the following question(s). Refer to Exhibit 18-2. The potential for the product-favored reaction involving aluminum and copper metals, Al3+(aq) and Cu2+(aq), is

The relationship between Gibbs free energy and E ∘\circ∘ cell is DG ∘\circ∘ =

Explain, with reference to the Nernst equation, how it is possible for a cell to have a positive cell potential under standard conditions, but a negative cell potential under other conditions.

Balance the following redox equation. The oxidation process is clearly

The value of E ∘\circ∘ cell for an aluminum-nickel electrochemical cell is +1.41 V at 25 ∘\circ∘ C. Calculate the value of DG ∘\circ∘ for this cell under standard conditions.

A secondary cell is one which ____; this is possible because ____.

Which statement about lead storage batteries is not correct?

The unit used to measure electrical current is the

Which compound contains the atom with the highest oxidation number?

The Nature of Chemistry

Atoms and Elements

Chemical Compounds

Quantities of Reactants and Products

Chemical Reactions

Energy and Chemical Reactions

Electron Configurations and the Periodic Table

Covalent Bonding

Molecular Structure

Gases and the Atmosphere

Liquids, Solids, and Materials

Chemical Kinetics: Rates of Reactions

Chemical Equilibrium

The Chemistry of Solutes and Solutions

Acids and Bases

Additional Aqueous Equilibria

Thermodynamics: Directionality of Chemical Reactions

Nuclear Chemistry

Filters

In the reaction shown below, is the oxidizing agent and the reducing agent.

Calculate the value of E_cell for a zinc-platinum electrochemical cell when the concentration of Pt²⁺(aq) is 0.050 M and the concentration of Zn²⁺(aq) is 1.1 M. E^$\circ$_cell = 1.96 V under standard conditions. Pt is the less active metal.

Exhibit 18-2 Use this list of half-reactions to answer the following question(s). Refer to Exhibit 18-2. The potential for the product-favored reaction involving aluminum and copper metals, Al³⁺(aq) and Cu²⁺(aq), is

The relationship between Gibbs free energy and E^$\circ$_cell is DG^$\circ$ =

The value of E^$\circ$_cell for an aluminum-nickel electrochemical cell is +1.41 V at 25^$\circ$C. Calculate the value of DG^$\circ$ for this cell under standard conditions.

A secondary cell is one which ; this is possible because .