Question 1

Nitrogen has many possible oxidation numbers; put the following nitrogen compounds in order of increasing oxidation number: NO2, HNO3, NO2-, NO.

Accepted Answer

A)  NO2, HNO3, NO2-, NO 
B)  NO, HNO3, NO2-, NO2 
C)  HNO3, NO2, NO2-, NO 
D)  NO, NO2-, NO2, HNO3 
E)  NO2-, NO, NO2, HNO3 
A)  NO2, HNO3, NO2-, NO 
B)  NO, HNO3, NO2-, NO2 
C)  HNO3, NO2, NO2-, NO 
D)  NO, NO2-, NO2, HNO3 
E)  NO2-, NO, NO2, HNO3 D

Question 2

Which of the species listed is the strongest oxidizing agent?‪   (If needed, refer to Table 17-1 in the text)

Accepted Answer

Pt+2

Question 3

Consider an electrochemical cell consisting of an Fe(s) electrode, Fe(NO3)2 electrolyte connected through a salt bridge to a Ag wire coated in AgCl(s) immersed in an aqueous KCl solution. Is the standard cell and balanced galvanic cell reaction:(If needed, refer to Table 17-1 in the text )

Accepted Answer

A)  0.259 V, Fe(s) + 3AgCl(s) $\rarr$ Fe3+(aq) + 3Ag(s) + 3Cl-(aq) 
B)  0.669 V, Fe(s) + 2AgCl(s) $\rarr$ Fe2+(aq) + 2Ag(s) + 2Cl-(aq) 
C)  -0.669 V, Fe(s) + 2AgCl(s) $\rarr$ Fe2+(aq) + 3Ag(s) + 3Cl-(aq) 
D)  -0.225 V, Fe(s) + 2AgCl(s) $\rarr$ Fe2+(aq) + 2Ag(s) + 2Cl-(aq) 
E)  0.669 V, Fe(s) + AgCl(s) $\rarr$  Fe2+(aq) + Ag(s) + Cl-(aq) 
A)  0.259 V, Fe(s) + 3AgCl(s) $\rarr$ Fe3+(aq) + 3Ag(s) + 3Cl-(aq) 
B)  0.669 V, Fe(s) + 2AgCl(s) $\rarr$ Fe2+(aq) + 2Ag(s) + 2Cl-(aq) 
C)  -0.669 V, Fe(s) + 2AgCl(s) $\rarr$ Fe2+(aq) + 3Ag(s) + 3Cl-(aq) 
D)  -0.225 V, Fe(s) + 2AgCl(s) $\rarr$ Fe2+(aq) + 2Ag(s) + 2Cl-(aq) 
E)  0.669 V, Fe(s) + AgCl(s) $\rarr$  Fe2+(aq) + Ag(s) + Cl-(aq) B

Question 4

Explain electrolytic reactions and cells.

Accepted Answer

An electrolytic cell

Question 5

Balance the following half reaction under acidic conditions:OCl- $\rightarrow$Cl-

Accepted Answer

2H⁺ + OCl

Question 6

An electrochemical cell is constructed that contains Cr3+(aq) and Cr metal as the electrode in one compartment and Cu2+(aq) and copper metal in the other compartment. Calculate the expected standard potential upon appropriately connecting the cell and describe the direction of electron and cation flow.(If needed, refer to Table 17-1 in the text)

Accepted Answer

E°= 1.09 V; electrons will flo

Question 7

For the reaction given below, which half reaction occurs at the cathode?Pb(s) + PbO2(s) + 2HSO4-(aq) + 2H3O+(aq) $\rarr$2PbSO4(aq) +4H2O(l)

Accepted Answer

A)  Pb $\rarr$PbSO4 
B)  PbO2 $\rarr$ PbSO4 
C)  HSO4- $\rarr$PbSO4 
D)  H3O+ $\rarr$ H2O 
E)  PbSO4 $\rarr$PbO2 
A)  Pb $\rarr$PbSO4 
B)  PbO2 $\rarr$ PbSO4 
C)  HSO4- $\rarr$PbSO4 
D)  H3O+ $\rarr$ H2O 
E)  PbSO4 $\rarr$PbO2

Question 8

Which of the species listed is the strongest reducing agent?   (If needed, refer to Table 17-1 in the text )

Accepted Answer

The answer of Which of the species listed is the...

Question 9

Calculate standard cell potentials.

Accepted Answer

All reduction potentials are relative to

Question 10

What is the role of the electrolyte in a galvanic cell?

Accepted Answer

A)  to facilitate rapid diffusion of the redox reagents to each other 
B)  to facilitate electron transport though the solution 
C)  to complete the electrical circuit by ion transport 
D)  to supply the ions for precipitating redox products 
E)  to protect electrodes from corrosion 
A)  to facilitate rapid diffusion of the redox reagents to each other 
B)  to facilitate electron transport though the solution 
C)  to complete the electrical circuit by ion transport 
D)  to supply the ions for precipitating redox products 
E)  to protect electrodes from corrosion

Question 11

Explain the chemistry of everyday redox reactions.

Accepted Answer

Batteries are galvanic cells.

Question 12

The following reaction occurs in a galvanic cell:
NiO2 + Cd + H2O $\rarr$ Cd(OH)2 + Ni(OH)2 + 2 OH-Which redox process in this battery occurs at a passive electrode?

Accepted Answer

A)  Cd $\rarr$ Cd(OH)2 
B)  NiO2 $\rarr$Ni(OH)2 
C)  O2 $\rarr$4 OH- 
D)  H2O $\rarr$OH- 
E)  neither electrode is passive 
A)  Cd $\rarr$ Cd(OH)2 
B)  NiO2 $\rarr$Ni(OH)2 
C)  O2 $\rarr$4 OH- 
D)  H2O $\rarr$OH- 
E)  neither electrode is passive

Question 13

Draw a figure illustrating how a cell would be arranged for the redox reaction of copper with silver ion but using indirect electron transfer and a salt bridge with KNO3 solution. Indicate the direction of electron flow in the wire and the movement of ions in the salt bridge.

Accepted Answer

Question 14

Balance redox reactions using the half-reaction method.

Accepted Answer

Redox reactions can be separat

Question 15

Balance the following half reaction under basic conditions:
MnO4- $\rightarrow$MnO2(s)

Accepted Answer

MnO4- +

Question 16

Consider an automobile which is powered by a perfectly efficient fuel cell that consumes hydrogen and oxygen in the following redox reaction:
2H2(g) + O2(g) $\rightarrow$ 2 H2O (l)If the electric system requires a current of 500 amperes, how many g of H2 are consumed per hour?(If needed, refer to Table 17-1 in the text )

Accepted Answer

18.7 g H<s

Question 17

Relate cell potential to the reaction conditions.

Accepted Answer

A cell potential depends on th

Question 18

Consider an electrochemical cell of the type shown in the figure where the redox half-reaction in both compartments has the identical standard potentials:   Use the Nernst equation to calculate the potential developed by this cell.(If needed, refer to Table 17-1 in the text)

Accepted Answer

The answer of Consider an electrochemical cell of the type...

Question 19

For a brine electrolysis cell (see redox reaction below) operating at 60,000 amps, how many kg of NaOH and Cl2 would be produced in 24.0 hours?
2 NaCl (aq) + 2 H2O $\rightarrow$ 2 NaOH (aq) + Cl2(g) + H2 (g)

Accepted Answer

2.15 x 10³

Question 20

Platinum metal is quite resistant to oxidation as may be deduced by its reduction potential:Pt2+ + 2e $\rarr$ $\quad $ Pt E° $\thickapprox$ 1.2 VExamine a table of reduction potentials (Table 17-1 in the text) and determine two elements capable of oxidizing platinum under standard conditions.

Accepted Answer

A)  Au, F2 
B)  F2, Fe 
C)  F2, Cl2 
D)  Br2, Ag 
E)  Mn, Au 
A)  Au, F2 
B)  F2, Fe 
C)  F2, Cl2 
D)  Br2, Ag 
E)  Mn, Au

Nitrogen has many possible oxidation numbers; put the following nitrogen compounds in order of increasing oxidation number: NO₂, HNO₃, NO₂^-, NO.

Which of the species listed is the strongest oxidizing agent?‪ (If needed, refer to Table 17-1 in the text)

Consider an electrochemical cell consisting of an Fe(s) electrode, Fe(NO₃)₂ electrolyte connected through a salt bridge to a Ag wire coated in AgCl(s) immersed in an aqueous KCl solution. Is the standard cell and balanced galvanic cell reaction:(If needed, refer to Table 17-1 in the text )

Explain electrolytic reactions and cells.

Balance the following half reaction under acidic conditions:OCl^- $\rightarrow$ Cl^-

For the reaction given below, which half reaction occurs at the cathode?Pb(s) + PbO₂(s)+ 2HSO₄^-(aq)+ 2H₃O⁺(aq) $\rarr$ 2PbSO₄(aq) +4H₂O(l)

Which of the species listed is the strongest reducing agent? (If needed, refer to Table 17-1 in the text )

Calculate standard cell potentials.

What is the role of the electrolyte in a galvanic cell?

Explain the chemistry of everyday redox reactions.

The following reaction occurs in a galvanic cell: NiO₂ + Cd + H₂O $\rarr$ Cd(OH)₂ + Ni(OH)₂ + 2 OH^-Which redox process in this battery occurs at a passive electrode?

Draw a figure illustrating how a cell would be arranged for the redox reaction of copper with silver ion but using indirect electron transfer and a salt bridge with KNO₃ solution. Indicate the direction of electron flow in the wire and the movement of ions in the salt bridge.

Balance redox reactions using the half-reaction method.

Balance the following half reaction under basic conditions: MnO₄^- $\rightarrow$ MnO_2(s)

Relate cell potential to the reaction conditions.

Consider an electrochemical cell of the type shown in the figure where the redox half-reaction in both compartments has the identical standard potentials: Use the Nernst equation to calculate the potential developed by this cell.(If needed, refer to Table 17-1 in the text)

For a brine electrolysis cell (see redox reaction below) operating at 60,000 amps, how many kg of NaOH and Cl₂would be produced in 24.0 hours? 2 NaCl (aq) + 2 H₂O $\rightarrow$ 2 NaOH (aq) + Cl₂(g) + H₂ (g)

Platinum metal is quite resistant to oxidation as may be deduced by its reduction potential:Pt²⁺ + 2e $\rarr$ $\quad$ Pt E° $\thickapprox$ 1.2 VExamine a table of reduction potentials (Table 17-1 in the text) and determine two elements capable of oxidizing platinum under standard conditions.

Fundamental Concepts of Chemistry

The Behaviour of Gases

Energy and Its Conservation

Atoms and Light

Atomic Energies and Periodicity

Fundamentals of Chemical Bonding

Theories of Chemical Bonding

Effects of Intermolecular Forces

Properties of Solutions

Organic Chemistrystructure

Organic Chemistryreactions

Spontaneity of Chemical Processes

Kinetics: Mechanisms and Rates of Reactions

Principles of Chemical Equilibrium

Aqueous Acidbase Equilibria

Applications of Aqueous Equilibria

Macromolecules

The Transition Metals

The Main Group Elements

Nuclear Chemistry and Radiochemistry

Filters

Exam 17: Electron Transfer Reactions

Nitrogen has many possible oxidation numbers; put the following nitrogen compounds in order of increasing oxidation number: NO2, HNO3, NO2-, NO.

Which of the species listed is the strongest oxidizing agent?‪ (If needed, refer to Table 17-1 in the text)

Consider an electrochemical cell consisting of an Fe(s) electrode, Fe(NO3)2 electrolyte connected through a salt bridge to a Ag wire coated in AgCl(s) immersed in an aqueous KCl solution. Is the standard cell and balanced galvanic cell reaction:(If needed, refer to Table 17-1 in the text )

Explain electrolytic reactions and cells.

Balance the following half reaction under acidic conditions:OCl- →\rightarrow→ Cl-

For the reaction given below, which half reaction occurs at the cathode?Pb(s) + PbO2(s) + 2HSO4-(aq) + 2H3O+(aq) →\rarr→ 2PbSO4(aq) +4H2O(l)

Which of the species listed is the strongest reducing agent? (If needed, refer to Table 17-1 in the text )

Calculate standard cell potentials.

What is the role of the electrolyte in a galvanic cell?

Explain the chemistry of everyday redox reactions.

The following reaction occurs in a galvanic cell: NiO2 + Cd + H2O →\rarr→ Cd(OH)2 + Ni(OH)2 + 2 OH-Which redox process in this battery occurs at a passive electrode?

Draw a figure illustrating how a cell would be arranged for the redox reaction of copper with silver ion but using indirect electron transfer and a salt bridge with KNO3 solution. Indicate the direction of electron flow in the wire and the movement of ions in the salt bridge.

Balance redox reactions using the half-reaction method.

Balance the following half reaction under basic conditions: MnO4- →\rightarrow→ MnO2(s)

Relate cell potential to the reaction conditions.

Consider an electrochemical cell of the type shown in the figure where the redox half-reaction in both compartments has the identical standard potentials: Use the Nernst equation to calculate the potential developed by this cell.(If needed, refer to Table 17-1 in the text)

For a brine electrolysis cell (see redox reaction below) operating at 60,000 amps, how many kg of NaOH and Cl2 would be produced in 24.0 hours? 2 NaCl (aq) + 2 H2O →\rightarrow→ 2 NaOH (aq) + Cl2(g) + H2 (g)

Platinum metal is quite resistant to oxidation as may be deduced by its reduction potential:Pt2+ + 2e →\rarr→ \quad Pt E° ≈\thickapprox≈ 1.2 VExamine a table of reduction potentials (Table 17-1 in the text) and determine two elements capable of oxidizing platinum under standard conditions.

Fundamental Concepts of Chemistry

The Behaviour of Gases

Energy and Its Conservation

Atoms and Light

Atomic Energies and Periodicity

Fundamentals of Chemical Bonding

Theories of Chemical Bonding

Effects of Intermolecular Forces

Properties of Solutions

Organic Chemistrystructure

Organic Chemistryreactions

Spontaneity of Chemical Processes

Kinetics: Mechanisms and Rates of Reactions

Principles of Chemical Equilibrium

Aqueous Acidbase Equilibria

Applications of Aqueous Equilibria

Macromolecules

The Transition Metals

The Main Group Elements

Nuclear Chemistry and Radiochemistry

Filters

Nitrogen has many possible oxidation numbers; put the following nitrogen compounds in order of increasing oxidation number: NO₂, HNO₃, NO₂^-, NO.

Consider an electrochemical cell consisting of an Fe(s) electrode, Fe(NO₃)₂ electrolyte connected through a salt bridge to a Ag wire coated in AgCl(s) immersed in an aqueous KCl solution. Is the standard cell and balanced galvanic cell reaction:(If needed, refer to Table 17-1 in the text )

Balance the following half reaction under acidic conditions:OCl^- $\rightarrow$ Cl^-

For the reaction given below, which half reaction occurs at the cathode?Pb(s) + PbO₂(s)+ 2HSO₄^-(aq)+ 2H₃O⁺(aq) $\rarr$ 2PbSO₄(aq) +4H₂O(l)

The following reaction occurs in a galvanic cell: NiO₂ + Cd + H₂O $\rarr$ Cd(OH)₂ + Ni(OH)₂ + 2 OH^-Which redox process in this battery occurs at a passive electrode?

Draw a figure illustrating how a cell would be arranged for the redox reaction of copper with silver ion but using indirect electron transfer and a salt bridge with KNO₃ solution. Indicate the direction of electron flow in the wire and the movement of ions in the salt bridge.

Balance the following half reaction under basic conditions: MnO₄^- $\rightarrow$ MnO_2(s)

For a brine electrolysis cell (see redox reaction below) operating at 60,000 amps, how many kg of NaOH and Cl₂would be produced in 24.0 hours? 2 NaCl (aq) + 2 H₂O $\rightarrow$ 2 NaOH (aq) + Cl₂(g) + H₂ (g)

Platinum metal is quite resistant to oxidation as may be deduced by its reduction potential:Pt²⁺ + 2e $\rarr$ $\quad$ Pt E° $\thickapprox$ 1.2 VExamine a table of reduction potentials (Table 17-1 in the text) and determine two elements capable of oxidizing platinum under standard conditions.