Aluminum metal is refined in a very energy-intensive process from bauxite ore using the Hall process, which requires electrolysis of aluminum oxide, Al2O3, in molten cryolite at more than 1,012F1F1F1S1F1F1F10C. In an industrial electrolysis cell, 1,900 kg of aluminum oxide was reduced with a current of 1,500 amps. How long did it take to reduce all the reactant to aluminum metal?

A) 1,000 hr B) 2,000 hr C) 330 hr D) 4,000 hr E) 660 hr A) 1,000 hr B) 2,000 hr C) 330 hr D) 4,000 hr E) 660 hr

Consider the following standard reduction potentials. Reduction Half-Reaction (volts) F1F1F1S1F1F1F10 2.38 F1F1F1S1F1F1F10 0.76 0.16 Which reaction AF1F1F1S1F1F1F10D will proceed spontaneously as written from left to right?

A) B) C) D) E) None of these will proceed spontaneously. A) B) C) D) E) None of these will proceed spontaneously.

Identify the strongest reducing agent in the following half-reactions. The standard reduction potentials are listed.F1F1F1S1F1F1F100.95 V F1F1F1S1F1F1F100.61 V F1F1F1S1F1F1F101.48 V F1F1F1S1F1F1F101.22 V

A) Cr B) MnO2 C) Hg2SO4 D) Sn E) Hg A) Cr B) MnO2 C) Hg2SO4 D) Sn E) Hg

Consider the following standard reduction potentials. Reduction Half-Reaction (volts) F1F1F1S1F1F1F10 0.74 F1F1F1S1F1F1F10 0.40 F1F1F1S1F1F1F10 0.23 Which reaction A-D will proceed spontaneously as written from left to right?

A) B) C) D) E) None of these will proceed spontaneously. A) B) C) D) E) None of these will proceed spontaneously.

Calculate the value of K for the following reaction at 298 K. given the following reduction potentials EF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 F1F1F1S1F1F1F101.077 V EF1F1F1S1F1F1F10 F1F1F1S1F1F1F10 F1F1F1S1F1F1F101.229 V

A) 1.92 F1F1F1S1F1F1F10 1010 B) 3.70 F1F1F1S1F1F1F10 102 C) 1.04 D) 1.18 E) 3.54 F1F1F1S1F1F1F10 101 A) 1.92 F1F1F1S1F1F1F10 1010 B) 3.70 F1F1F1S1F1F1F10 102 C) 1.04 D) 1.18 E) 3.54 F1F1F1S1F1F1F10 101

A typical hearing aid battery has a capacity of 5 ampere-hour (A F1F1F1S1F1F1F10 hr) and can supply up to 23.4 kJ of energy. What is the voltage of the battery?

A) 78 V B) 1.3 V C) 1.3 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F103 V D) 7.8 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F103 V E) 0.90 V A) 78 V B) 1.3 V C) 1.3 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F103 V D) 7.8 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F103 V E) 0.90 V

Exam 18: Electrochemistry: The Quest for Clean Energy

Aluminum metal is refined in a very energy-intensive process from bauxite ore using the Hall process, which requires electrolysis of aluminum oxide, Al₂O₃, in molten cryolite at more than 1,012C. In an industrial electrolysis cell, 1,900 kg of aluminum oxide was reduced with a current of 1,500 amps. How long did it take to reduce all the reactant to aluminum metal?

(Multiple Choice)

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Question 21

The following reaction occurs in a new battery called the super iron battery. In this reaction, ________ is oxidized.

(Multiple Choice)

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Question 22

If the potential of a voltaic cell is 1.20 V, what is the free-energy change when one mole of electrons is transferred in the oxidation-reduction reaction?

(Multiple Choice)

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Question 23

A concentration cell is constructed by using the same half-reaction for both the cathode and anode. What is the value of standard cell potential, , for a concentration cell that combines a silver anode in contact with 0.10 M silver nitrate and a silver cathode in contact with 0.00003 M silver nitrate? (  0.80 V for Ag/Ag^)

(Multiple Choice)

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Question 24

Consider the following standard reduction potentials. Reduction Half-Reaction (volts)  2.38  0.76 0.16 Which reaction AD will proceed spontaneously as written from left to right?

(Multiple Choice)

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Question 25

Which statement does not correctly describe a "dead" battery with a voltage of 0?

(Multiple Choice)

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Question 26

Identify the strongest reducing agent in the following half-reactions. The standard reduction potentials are listed.0.95 V 0.61 V 1.48 V 1.22 V

(Multiple Choice)

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Question 27

Using the following data, determine the standard cell potential for the electrochemical cell constructed using the following reaction. Half-reaction Standard Reduction Potential (V ) 0.771 0.124

(Multiple Choice)

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Question 28

The spontaneous redox reaction in a voltaic cell has ________

(Multiple Choice)

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Question 29

A concentration cell is constructed by using the same half-reaction for both the cathode and anode. What is the value of E_cell for a concentration cell that combines silver electrodes in contact with 0.10 M silver nitrate and 0.00003 M silver nitrate solutions? (  0.80 V for Ag/Ag^)

(Multiple Choice)

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Question 30

The change in free energy for a reaction, G, depends on the stoichiometric coefficients used in writing the reaction, but cell potentials, E, do not depend on these coefficients. Which statement accounts for this difference?

(Multiple Choice)

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Question 31

Using the following data, determine the standard cell potential for the electrochemical cell constructed using the following reaction. Half-reaction Standard Reduction Potential (V ) 0.763 0.337

(Multiple Choice)

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Question 32

Methanol fuel cells depend on the following reaction. How many electrons are transferred in this redox reaction as written?

(Multiple Choice)

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Question 33

Cathodic protection occurs when iron is ________

(Multiple Choice)

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Question 34

Consider the following standard reduction potentials. Reduction Half-Reaction (volts)  0.74  0.40  0.23 Which reaction A-D will proceed spontaneously as written from left to right?

(Multiple Choice)

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Question 35

Calculate the value of K for the following reaction at 298 K. given the following reduction potentials E  1.077 V E  1.229 V

(Multiple Choice)

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Question 36

If the free-energy change of a voltaic cell is 258 kJ, what is the potential of the cell if three moles of electrons are transferred in the oxidation-reduction reaction?

(Multiple Choice)

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Question 37

The work involved in moving exactly 1 mole of electrons through a potential difference of exactly 1 V is ________

(Multiple Choice)

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Question 38

A typical hearing aid battery has a capacity of 5 ampere-hour (A  hr) and can supply up to 23.4 kJ of energy. What is the voltage of the battery?

(Multiple Choice)

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Question 39

Use the table of standard reduction potentials below to identify the metal or metal ion that is the weakest oxidizing agent. Standard Reduction Potentials (volts) in Aqueous Solution 1.70 0.520 0.036 0.400 0.730 1.66

(Multiple Choice)

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Question 40

Showing 21 - 40 of 167

The following reaction occurs in a new battery called the super iron battery. In this reaction, ________ is oxidized.

If the potential of a voltaic cell is 1.20 V, what is the free-energy change when one mole of electrons is transferred in the oxidation-reduction reaction?

Consider the following standard reduction potentials. Reduction Half-Reaction (volts)  2.38  0.76 0.16 Which reaction AD will proceed spontaneously as written from left to right?

Which statement does not correctly describe a "dead" battery with a voltage of 0?

Identify the strongest reducing agent in the following half-reactions. The standard reduction potentials are listed.0.95 V 0.61 V 1.48 V 1.22 V

Using the following data, determine the standard cell potential for the electrochemical cell constructed using the following reaction. Half-reaction Standard Reduction Potential (V ) 0.771 0.124

The spontaneous redox reaction in a voltaic cell has ________

A concentration cell is constructed by using the same half-reaction for both the cathode and anode. What is the value of E_cell for a concentration cell that combines silver electrodes in contact with 0.10 M silver nitrate and 0.00003 M silver nitrate solutions? (  0.80 V for Ag/Ag^)

The change in free energy for a reaction, G, depends on the stoichiometric coefficients used in writing the reaction, but cell potentials, E, do not depend on these coefficients. Which statement accounts for this difference?

Using the following data, determine the standard cell potential for the electrochemical cell constructed using the following reaction. Half-reaction Standard Reduction Potential (V ) 0.763 0.337

Methanol fuel cells depend on the following reaction. How many electrons are transferred in this redox reaction as written?

Cathodic protection occurs when iron is ________

Consider the following standard reduction potentials. Reduction Half-Reaction (volts)  0.74  0.40  0.23 Which reaction A-D will proceed spontaneously as written from left to right?

Calculate the value of K for the following reaction at 298 K. given the following reduction potentials E  1.077 V E  1.229 V

If the free-energy change of a voltaic cell is 258 kJ, what is the potential of the cell if three moles of electrons are transferred in the oxidation-reduction reaction?

The work involved in moving exactly 1 mole of electrons through a potential difference of exactly 1 V is ________

A typical hearing aid battery has a capacity of 5 ampere-hour (A  hr) and can supply up to 23.4 kJ of energy. What is the voltage of the battery?

Use the table of standard reduction potentials below to identify the metal or metal ion that is the weakest oxidizing agent. Standard Reduction Potentials (volts) in Aqueous Solution 1.70 0.520 0.036 0.400 0.730 1.66

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

The following reaction occurs in a new battery called the super iron battery. In this reaction, ________ is oxidized.

If the potential of a voltaic cell is 1.20 V, what is the free-energy change when one mole of electrons is transferred in the oxidation-reduction reaction?

Consider the following standard reduction potentials. Reduction Half-Reaction (volts)  2.38  0.76 0.16 Which reaction AD will proceed spontaneously as written from left to right?

Which statement does not correctly describe a "dead" battery with a voltage of 0?

Identify the strongest reducing agent in the following half-reactions. The standard reduction potentials are listed.0.95 V 0.61 V 1.48 V 1.22 V

Using the following data, determine the standard cell potential for the electrochemical cell constructed using the following reaction. Half-reaction Standard Reduction Potential (V ) 0.771 0.124

The spontaneous redox reaction in a voltaic cell has ________

A concentration cell is constructed by using the same half-reaction for both the cathode and anode. What is the value of Ecell for a concentration cell that combines silver electrodes in contact with 0.10 M silver nitrate and 0.00003 M silver nitrate solutions? (  0.80 V for Ag/Ag)

The change in free energy for a reaction, G, depends on the stoichiometric coefficients used in writing the reaction, but cell potentials, E, do not depend on these coefficients. Which statement accounts for this difference?

Using the following data, determine the standard cell potential for the electrochemical cell constructed using the following reaction. Half-reaction Standard Reduction Potential (V ) 0.763 0.337

Methanol fuel cells depend on the following reaction. How many electrons are transferred in this redox reaction as written?

Cathodic protection occurs when iron is ________

Consider the following standard reduction potentials. Reduction Half-Reaction (volts)  0.74  0.40  0.23 Which reaction A-D will proceed spontaneously as written from left to right?

Calculate the value of K for the following reaction at 298 K. given the following reduction potentials E  1.077 V E  1.229 V

If the free-energy change of a voltaic cell is 258 kJ, what is the potential of the cell if three moles of electrons are transferred in the oxidation-reduction reaction?

The work involved in moving exactly 1 mole of electrons through a potential difference of exactly 1 V is ________

A typical hearing aid battery has a capacity of 5 ampere-hour (A  hr) and can supply up to 23.4 kJ of energy. What is the voltage of the battery?

Use the table of standard reduction potentials below to identify the metal or metal ion that is the weakest oxidizing agent. Standard Reduction Potentials (volts) in Aqueous Solution 1.70 0.520 0.036 0.400 0.730 1.66

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

Filters

A concentration cell is constructed by using the same half-reaction for both the cathode and anode. What is the value of E_cell for a concentration cell that combines silver electrodes in contact with 0.10 M silver nitrate and 0.00003 M silver nitrate solutions? (  0.80 V for Ag/Ag^)