Question 1

What is the oxidation number of chromium in the ionic compound ammonium dichromate, (NH4)2Cr2O7?

Accepted Answer

A) (F1F1F1S1F1F1F103) 
B) (F1F1F1S1F1F1F104) 
C) (F1F1F1S1F1F1F105) 
D) (F1F1F1S1F1F1F106) 
E) (F1F1F1S1F1F1F107) 
A) (F1F1F1S1F1F1F103) 
B) (F1F1F1S1F1F1F104) 
C) (F1F1F1S1F1F1F105) 
D) (F1F1F1S1F1F1F106) 
E) (F1F1F1S1F1F1F107) D

Question 2

Electrochemical cell potentials can be used to determine equilibrium constants that would be otherwise difficult to determine because concentrations are small. Calculate the value of Ksp for CdS from the following data.   EF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 F1F1F1S1F1F1F101.21 V   EF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 F1F1F1S1F1F1F100.40 V

Accepted Answer

A) 3 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1055 
B) 4 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1028 
C) 2 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1014 
D) 3 F1F1F1S1F1F1F10 1027 
E) 1 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1036 
A) 3 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1055 
B) 4 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1028 
C) 2 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1014 
D) 3 F1F1F1S1F1F1F10 1027 
E) 1 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1036 B

Question 3

Consider the following standard reduction potentials. Reduction Half-Reaction   (volts)   F1F1F1S1F1F1F10 0.45   F1F1F1S1F1F1F10 0.34   F1F1F1S1F1F1F10 0.76   F1F1F1S1F1F1F10 1.66   F1F1F1S1F1F1F10 0.14
Which corrosion reaction when two metals come in contact is not likely to occur?

Accepted Answer

A) Iron will be oxidized as copper ions are reduced. 
B) Aluminum will be oxidized as copper ions are reduced. 
C) Tin will be oxidized as copper ions are reduced. 
D) Zinc will be oxidized as copper ions are reduced. 
E) Iron will be oxidized as aluminum ions are reduced. 
A) Iron will be oxidized as copper ions are reduced. 
B) Aluminum will be oxidized as copper ions are reduced. 
C) Tin will be oxidized as copper ions are reduced. 
D) Zinc will be oxidized as copper ions are reduced. 
E) Iron will be oxidized as aluminum ions are reduced. E

Question 4

The following reaction occurs in basic solution. Identify the reducing agent. Note that the reaction equation is not balanced.

Accepted Answer

A) Zn(s) 
B) NO3F1F1F1S1F1F1F10(aq) 
C) OHF1F1F1S1F1F1F10(aq) 
D) H2O(l ) 
E) Zn(OH)42F1F1F1S1F1F1F10(aq) 
A) Zn(s) 
B) NO3F1F1F1S1F1F1F10(aq) 
C) OHF1F1F1S1F1F1F10(aq) 
D) H2O(l ) 
E) Zn(OH)42F1F1F1S1F1F1F10(aq)

Question 5

Consider the following standard reduction potentials. Reduction Half-Reaction   (volts)   F1F1F1S1F1F1F10 0.74   F1F1F1S1F1F1F10 0.40   F1F1F1S1F1F1F10 0.23
The Cr/Cr3F1F1F1S1F1F1F10 half-reaction can be paired with the other two to produce voltaic cells because ________

Accepted Answer

A) Cr is a powerful oxidizing agent. 
B) Cr is a powerful reducing agent. 
C) Cr3F1F1F1S1F1F1F10 is a powerful oxidizing agent. 
D) Cr3F1F1F1S1F1F1F10 is a powerful reducing agent. 
E) Cd and Ni are readily oxidized. 
A) Cr is a powerful oxidizing agent. 
B) Cr is a powerful reducing agent. 
C) Cr3F1F1F1S1F1F1F10 is a powerful oxidizing agent. 
D) Cr3F1F1F1S1F1F1F10 is a powerful reducing agent. 
E) Cd and Ni are readily oxidized.

Question 6

Applying a current to a rechargeable battery converts it from ________ cell to ________ cell.

Accepted Answer

A) a voltaic; an electrolytic 
B) an electrolytic; a voltaic 
C) a Leclanché; a Nernst 
D) a Nernst; a Leclanché 
E) a Born cell; a Haber 
A) a voltaic; an electrolytic 
B) an electrolytic; a voltaic 
C) a Leclanché; a Nernst 
D) a Nernst; a Leclanché 
E) a Born cell; a Haber

Question 7

Using the following data, determine the standard cell potential   for the electrochemical cell constructed using the following reaction.   Half-reaction Standard Reduction Potential (V)   F1F1F1S1F1F1F100.34   F1F1F1S1F1F1F101.66

Accepted Answer

A) (F1F1F1S1F1F1F101.32 V) 
B) (F1F1F1S1F1F1F101.32 V) 
C) (F1F1F1S1F1F1F102.00 V) 
D) (F1F1F1S1F1F1F102.00 V) 
E) (F1F1F1S1F1F1F102.30 V) 
A) (F1F1F1S1F1F1F101.32 V) 
B) (F1F1F1S1F1F1F101.32 V) 
C) (F1F1F1S1F1F1F102.00 V) 
D) (F1F1F1S1F1F1F102.00 V) 
E) (F1F1F1S1F1F1F102.30 V)

Question 8

Use the table of standard reduction potentials below to identify the metal or metal ion that is the strongest oxidizing agent. Standard Reduction
Potentials (volts) in Aqueous Solution   F1F1F1S1F1F1F101.80   F1F1F1S1F1F1F101.50   F1F1F1S1F1F1F100.771   F1F1F1S1F1F1F100.535   F1F1F1S1F1F1F100.124   F1F1F1S1F1F1F101.66   F1F1F1S1F1F1F102.37   F1F1F1S1F1F1F102.93

Accepted Answer

A) Pb4F1F1F1S1F1F1F10 
B) Pb2F1F1F1S1F1F1F10 
C) KF1F1F1S1F1F1F10 
D) K 
E) Al 
A) Pb4F1F1F1S1F1F1F10 
B) Pb2F1F1F1S1F1F1F10 
C) KF1F1F1S1F1F1F10 
D) K 
E) Al

Question 9

Which one of the following items does not characterize a reducing agent?

Accepted Answer

A) A reducing agent loses electrons. 
B) A reducing agent causes another species to be reduced. 
C) The oxidation number of a reducing agent increases. 
D) A good reducing agent is a metal in a high oxidation state, such as Mn7F1F1F1S1F1F1F10. 
E) An example of a good reducing agent is an alkali metal, such as Na. 
A) A reducing agent loses electrons. 
B) A reducing agent causes another species to be reduced. 
C) The oxidation number of a reducing agent increases. 
D) A good reducing agent is a metal in a high oxidation state, such as Mn7F1F1F1S1F1F1F10. 
E) An example of a good reducing agent is an alkali metal, such as Na.

Question 10

Electrochemical cell potentials can be used to determine equilibrium constants that would be otherwise difficult to determine because concentrations are small. Calculate the value of Ksp for AgI from the following data.   EF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 F1F1F1S1F1F1F100.80 V   EF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 F1F1F1S1F1F1F100.15 V

Accepted Answer

A) 3.03 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1014 
B) 8.4 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1017 
C) 7.12 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1012 
D) 1.13 F1F1F1S1F1F1F10 1016 
E) 3.31 F1F1F1S1F1F1F10 1013 
A) 3.03 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1014 
B) 8.4 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1017 
C) 7.12 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1012 
D) 1.13 F1F1F1S1F1F1F10 1016 
E) 3.31 F1F1F1S1F1F1F10 1013

Question 11

Bubbles will form on wires attached to a 9-volt battery placed in water. Which statements correctly describe what is happening?
I. The wire attached to the (F1F1F1S1F1F1F10) battery electrode becomes the cathode, and water is being reduced there to produce hydrogen gas.
II. The wire attached to the (F1F1F1S1F1F1F10) battery electrode becomes the anode, and water is being oxidized there to produce oxygen gas.
III. The wire attached to the (F1F1F1S1F1F1F10) battery electrode becomes the cathode, and water is being oxidized there to produce oxygen gas.
IV. The wire attached to the (F1F1F1S1F1F1F10) battery electrode becomes the anode, and water is being reduced there to produce hydrogen gas.

Accepted Answer

A) I and II 
B) III and IV 
C) I and III 
D) II and IV 
E) I and IV 
A) I and II 
B) III and IV 
C) I and III 
D) II and IV 
E) I and IV

Question 12

If in using a lead-acid battery to start a car, 1.00 g of Pb is consumed on the anode, how long will it take to recharge the battery, using a current of 0.500 amperes, and turn the PbSO4 that was produced back into Pb?

Accepted Answer

Question 13

For the electrochemical cell indicated below, in which zinc is being oxidized, identify the components labeled as aF1F1F1S1F1F1F10d. Use the terms zinc nitrate solution, copper nitrate solution, copper electrode, and salt bridge. Also, identify the cathode and the anode, and label the electrodes as F1F1F1S1F1F1F10 and F1F1F1S1F1F1F10.

Accepted Answer

(a) zinc nitrate (b) salt brid

Question 14

Starting with F1F1F1S1F1F1F10G F1F1F1S1F1F1F10 F1F1F1S1F1F1F10GF1F1F1S1F1F1F10F1F1F1S1F1F1F10 RT lnQ and F1F1F1S1F1F1F10G F1F1F1S1F1F1F10 F1F1F1S1F1F1F10nFE, derive the Nernst equation.

Accepted Answer

Start with F1F1F1S1F1F1F10G F1F1F1S1F1

Question 15

Based on the information in the table of standard reduction potentials below, what is the standard cell potential for an electrochemical cell that has chromium, Cr, and cadmium, Cd, electrodes? Also, identify the anode. Standard Reduction
Potentials (volts) in Aqueous Solution   F1F1F1S1F1F1F101.70   F1F1F1S1F1F1F100.520   F1F1F1S1F1F1F100.036   F1F1F1S1F1F1F100.400   F1F1F1S1F1F1F100.73   F1F1F1S1F1F1F101.66

Accepted Answer

A) (F1F1F1S1F1F1F100.33 V with Cr as the anode) 
B) (F1F1F1S1F1F1F100.33 V with Cr as the anode) 
C) (F1F1F1S1F1F1F100.26 V with Cd as the anode) 
D) (F1F1F1S1F1F1F100.33 V with Cd as the anode) 
E) (F1F1F1S1F1F1F100.33 V with Cd as the anode) 
A) (F1F1F1S1F1F1F100.33 V with Cr as the anode) 
B) (F1F1F1S1F1F1F100.33 V with Cr as the anode) 
C) (F1F1F1S1F1F1F100.26 V with Cd as the anode) 
D) (F1F1F1S1F1F1F100.33 V with Cd as the anode) 
E) (F1F1F1S1F1F1F100.33 V with Cd as the anode)

Question 16

The electrodes on batteries are labeled F1F1F1S1F1F1F10 and F1F1F1S1F1F1F10. The ________ is labeled ________, and ________ occurs there.

Accepted Answer

A) anode; positive; oxidation 
B) anode; negative; reduction 
C) cathode; positive; reduction 
D) cathode; negative; reduction 
E) cathode; positive; oxidation 
A) anode; positive; oxidation 
B) anode; negative; reduction 
C) cathode; positive; reduction 
D) cathode; negative; reduction 
E) cathode; positive; oxidation

Question 17

In the smelting of iron from iron oxide according to the equation   what is the change in oxidation number for iron?

Accepted Answer

A) (F1F1F1S1F1F1F103) 
B) (F1F1F1S1F1F1F103) 
C) (F1F1F1S1F1F1F102) 
D) (F1F1F1S1F1F1F102) 
E) 0 
A) (F1F1F1S1F1F1F103) 
B) (F1F1F1S1F1F1F103) 
C) (F1F1F1S1F1F1F102) 
D) (F1F1F1S1F1F1F102) 
E) 0

Question 18

Calculate the cell potential (Ecell) for the following reaction if [AgF1F1F1S1F1F1F10] F1F1F1S1F1F1F10 0.10 M and [Zn2F1F1F1S1F1F1F10] F1F1F1S1F1F1F10 0.25 M.   Half-reaction Standard Reduction Potential (V)   F1F1F1S1F1F1F10 0.763   F1F1F1S1F1F1F10 0.337

Accepted Answer

Question 19

Cadmium is a toxic heavy metal. The U.S. Environmental Protection Agency limits the concentration of cadmium ions in drinking water to less than 4 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F108 M. Assess the feasibility of monitoring of cadmium in drinking water using a voltaic cell based on the following half-reactions.   EF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 F1F1F1S1F1F1F100.7996 V   EF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 F1F1F1S1F1F1F100.4.030 V If the silver ion concentration were 1.000 M, what cadmium ion concentration at 298 K would increase the cell potential by 10 mV from the standard cell potential?

Accepted Answer

A) 0.36 M 
B) 4.6 M 
C) 0.46 M 
D) 0.68 M 
E) 6.8 M 
A) 0.36 M 
B) 4.6 M 
C) 0.46 M 
D) 0.68 M 
E) 6.8 M

Question 20

Electrochemical cell potentials can be used to determine equilibrium constants that would be otherwise difficult to determine because concentrations are small. Calculate the value of Ksp for AgI from the following data.   EF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 F1F1F1S1F1F1F100.80 V   EF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 F1F1F1S1F1F1F100.15 V

Accepted Answer

8.4 x 10F1

What is the oxidation number of chromium in the ionic compound ammonium dichromate, (NH₄)₂Cr₂O₇?

Electrochemical cell potentials can be used to determine equilibrium constants that would be otherwise difficult to determine because concentrations are small. Calculate the value of K_sp for CdS from the following data. E  1.21 V E  0.40 V

Consider the following standard reduction potentials. Reduction Half-Reaction (volts)  0.45  0.34  0.76  1.66  0.14 Which corrosion reaction when two metals come in contact is not likely to occur?

The following reaction occurs in basic solution. Identify the reducing agent. Note that the reaction equation is not balanced.

Consider the following standard reduction potentials. Reduction Half-Reaction (volts)  0.74  0.40  0.23 The Cr/Cr³^ half-reaction can be paired with the other two to produce voltaic cells because ________

Applying a current to a rechargeable battery converts it from cell to cell.

Using the following data, determine the standard cell potential for the electrochemical cell constructed using the following reaction. Half-reaction Standard Reduction Potential (V) 0.34 1.66

Use the table of standard reduction potentials below to identify the metal or metal ion that is the strongest oxidizing agent. Standard Reduction Potentials (volts) in Aqueous Solution 1.80 1.50 0.771 0.535 0.124 1.66 2.37 2.93

Which one of the following items does not characterize a reducing agent?

Electrochemical cell potentials can be used to determine equilibrium constants that would be otherwise difficult to determine because concentrations are small. Calculate the value of K_sp for AgI from the following data. E  0.80 V E  0.15 V

If in using a lead-acid battery to start a car, 1.00 g of Pb is consumed on the anode, how long will it take to recharge the battery, using a current of 0.500 amperes, and turn the PbSO₄ that was produced back into Pb?

For the electrochemical cell indicated below, in which zinc is being oxidized, identify the components labeled as ad. Use the terms zinc nitrate solution, copper nitrate solution, copper electrode, and salt bridge. Also, identify the cathode and the anode, and label the electrodes as  and .

Starting with G  G RT lnQ and G  nFE, derive the Nernst equation.

The electrodes on batteries are labeled  and . The is labeled , and occurs there.

In the smelting of iron from iron oxide according to the equation what is the change in oxidation number for iron?

Calculate the cell potential (E_cell) for the following reaction if [Ag^]  0.10 M and [Zn²^]  0.25 M. Half-reaction Standard Reduction Potential (V)  0.763  0.337

Electrochemical cell potentials can be used to determine equilibrium constants that would be otherwise difficult to determine because concentrations are small. Calculate the value of K_sp for AgI from the following data. E  0.80 V E  0.15 V

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Solution Chemistry: The Hydrosphere

Thermochemistry: Energy Changes in Reactions

Properties of Gases: The Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Solids: Crystals, Alloys, and Polymers

Chemical Kinetics: Reactions in the Atmosphere

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acidbase Equilibria: Proton Transfer in Biological Systems

Additional Aqueous Equilibria: Chemistry and the Oceans

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Nuclear Chemistry: Applications to Energy and Medicine

Organic and Biological Molecules: the Compounds of Life

The Main Group Elements: Life and the Periodic Table

Transition Metals: Biological and Medical Applications

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Exam 18: Electrochemistry: The Quest for Clean Energy

What is the oxidation number of chromium in the ionic compound ammonium dichromate, (NH4)2Cr2O7?

Electrochemical cell potentials can be used to determine equilibrium constants that would be otherwise difficult to determine because concentrations are small. Calculate the value of Ksp for CdS from the following data. E  1.21 V E  0.40 V

Consider the following standard reduction potentials. Reduction Half-Reaction (volts)  0.45  0.34  0.76  1.66  0.14 Which corrosion reaction when two metals come in contact is not likely to occur?

The following reaction occurs in basic solution. Identify the reducing agent. Note that the reaction equation is not balanced.

Consider the following standard reduction potentials. Reduction Half-Reaction (volts)  0.74  0.40  0.23 The Cr/Cr3 half-reaction can be paired with the other two to produce voltaic cells because ________

Applying a current to a rechargeable battery converts it from ________ cell to ________ cell.

Using the following data, determine the standard cell potential for the electrochemical cell constructed using the following reaction. Half-reaction Standard Reduction Potential (V) 0.34 1.66

Use the table of standard reduction potentials below to identify the metal or metal ion that is the strongest oxidizing agent. Standard Reduction Potentials (volts) in Aqueous Solution 1.80 1.50 0.771 0.535 0.124 1.66 2.37 2.93

Which one of the following items does not characterize a reducing agent?

Electrochemical cell potentials can be used to determine equilibrium constants that would be otherwise difficult to determine because concentrations are small. Calculate the value of Ksp for AgI from the following data. E  0.80 V E  0.15 V

If in using a lead-acid battery to start a car, 1.00 g of Pb is consumed on the anode, how long will it take to recharge the battery, using a current of 0.500 amperes, and turn the PbSO4 that was produced back into Pb?

Starting with G  G RT lnQ and G  nFE, derive the Nernst equation.

The electrodes on batteries are labeled  and . The ________ is labeled ________, and ________ occurs there.

In the smelting of iron from iron oxide according to the equation what is the change in oxidation number for iron?

Calculate the cell potential (Ecell) for the following reaction if [Ag]  0.10 M and [Zn2]  0.25 M. Half-reaction Standard Reduction Potential (V)  0.763  0.337

Electrochemical cell potentials can be used to determine equilibrium constants that would be otherwise difficult to determine because concentrations are small. Calculate the value of Ksp for AgI from the following data. E  0.80 V E  0.15 V

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Solution Chemistry: The Hydrosphere

Thermochemistry: Energy Changes in Reactions

Properties of Gases: The Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Solids: Crystals, Alloys, and Polymers

Chemical Kinetics: Reactions in the Atmosphere

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acidbase Equilibria: Proton Transfer in Biological Systems

Additional Aqueous Equilibria: Chemistry and the Oceans

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Nuclear Chemistry: Applications to Energy and Medicine

Organic and Biological Molecules: the Compounds of Life

The Main Group Elements: Life and the Periodic Table

Transition Metals: Biological and Medical Applications

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What is the oxidation number of chromium in the ionic compound ammonium dichromate, (NH₄)₂Cr₂O₇?

Electrochemical cell potentials can be used to determine equilibrium constants that would be otherwise difficult to determine because concentrations are small. Calculate the value of K_sp for CdS from the following data. E  1.21 V E  0.40 V

Consider the following standard reduction potentials. Reduction Half-Reaction (volts)  0.74  0.40  0.23 The Cr/Cr³^ half-reaction can be paired with the other two to produce voltaic cells because ________

Applying a current to a rechargeable battery converts it from cell to cell.

Electrochemical cell potentials can be used to determine equilibrium constants that would be otherwise difficult to determine because concentrations are small. Calculate the value of K_sp for AgI from the following data. E  0.80 V E  0.15 V

If in using a lead-acid battery to start a car, 1.00 g of Pb is consumed on the anode, how long will it take to recharge the battery, using a current of 0.500 amperes, and turn the PbSO₄ that was produced back into Pb?

The electrodes on batteries are labeled  and . The is labeled , and occurs there.

Calculate the cell potential (E_cell) for the following reaction if [Ag^]  0.10 M and [Zn²^]  0.25 M. Half-reaction Standard Reduction Potential (V)  0.763  0.337

Electrochemical cell potentials can be used to determine equilibrium constants that would be otherwise difficult to determine because concentrations are small. Calculate the value of K_sp for AgI from the following data. E  0.80 V E  0.15 V