Question 1

Which statement about this concentration cell is incorrect?

Accepted Answer

A) The electrode on the left side is the anode. 
B) The cell potential is positive. 
C) Anions in the salt bridge migrate to the left side. 
D) Hydrogen ions are reduced on the right side. 
E) The pH of the solution on the right side is higher than the pH on the left side. 
A) The electrode on the left side is the anode. 
B) The cell potential is positive. 
C) Anions in the salt bridge migrate to the left side. 
D) Hydrogen ions are reduced on the right side. 
E) The pH of the solution on the right side is higher than the pH on the left side.

Question 2

If the free-energy change of the following voltaic cell   is F1F1F1S1F1F1F1046.3 kJ, what is the standard potential of the cell?

Accepted Answer

F1F1F1S1F

Question 3

Which statement regarding battery-powered electric cars is not correct? Currently, battery-powered electric cars ________

Accepted Answer

A) are more efficient than internal combustion engines. 
B) have a limited range due to battery capacity. 
C) use electrical energy produced primarily by the combustion of coal and natural gas. 
D) show promise in shifting the energy needs of our transportation system from petroleum to nuclear and solar sources. 
E) do not contribute to pollution of the atmosphere by producing carbon dioxide, nitrogen oxides, and other gases. 
A) are more efficient than internal combustion engines. 
B) have a limited range due to battery capacity. 
C) use electrical energy produced primarily by the combustion of coal and natural gas. 
D) show promise in shifting the energy needs of our transportation system from petroleum to nuclear and solar sources. 
E) do not contribute to pollution of the atmosphere by producing carbon dioxide, nitrogen oxides, and other gases.

Question 4

Copper metal is purified by electrolysis. How much copper metal could be produced from copper(II) oxide by applying a current of 10.0 amps at the appropriate negative potential for 12.0 hours?

Accepted Answer

A) 284 g 
B) 142 g 
C) 28.4 g 
D) 14.2 g 
E) 4.48 g 
A) 284 g 
B) 142 g 
C) 28.4 g 
D) 14.2 g 
E) 4.48 g

Question 5

The energy supplied by a battery can be determined by ________

Accepted Answer

A) multiplying amperes supplied by seconds. 
B) dividing amperes supplied by seconds. 
C) multiplying coulombs supplied by volts. 
D) multiplying coulombs supplied by seconds. 
E) dividing coulombs supplied by seconds. 
A) multiplying amperes supplied by seconds. 
B) dividing amperes supplied by seconds. 
C) multiplying coulombs supplied by volts. 
D) multiplying coulombs supplied by seconds. 
E) dividing coulombs supplied by seconds.

Question 6

A voltaic cell is constructed based on the oxidation of zinc metal and the reduction of silver cations. Solutions of silver nitrate and zinc nitrate also were used. Locate the silver metal on the diagram.

Accepted Answer

A) a 
B) b 
C) c 
D) d 
A) a 
B) b 
C) c 
D) d

Question 7

Use the table of standard reduction potentials below to identify the metal or metal ion that is the weakest reducing agent. 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) Cr 
B) Fe 
C) Cu 
D) Ce4F1F1F1S1F1F1F10 
E) Al3F1F1F1S1F1F1F10 
A) Cr 
B) Fe 
C) Cu 
D) Ce4F1F1F1S1F1F1F10 
E) Al3F1F1F1S1F1F1F10

Question 8

Consider the following standard reduction potentials. Reduction Half-Reaction   (volts)   F1F1F1S1F1F1F10 2.38   F1F1F1S1F1F1F10 0.76   0.16
The Mg/Mg2F1F1F1S1F1F1F10 half-reaction can be paired with the other two to produce voltaic cells because ________

Accepted Answer

A) Mg is a powerful oxidizing agent. 
B) Mg is a powerful reducing agent. 
C) Mg2F1F1F1S1F1F1F10 is a powerful reducing agent. 
D) Mg2F1F1F1S1F1F1F10 is a powerful oxidizing agent. 
E) Zn and CuF1F1F1S1F1F1F10 are readily oxidized. 
A) Mg is a powerful oxidizing agent. 
B) Mg is a powerful reducing agent. 
C) Mg2F1F1F1S1F1F1F10 is a powerful reducing agent. 
D) Mg2F1F1F1S1F1F1F10 is a powerful oxidizing agent. 
E) Zn and CuF1F1F1S1F1F1F10 are readily oxidized.

Question 9

The diagram below represents a voltaic cell. In this cell, which species is oxidized? Cd(s)|Cd2F1F1F1S1F1F1F10(aq)||Fe2F1F1F1S1F1F1F10(aq),Fe3F1F1F1S1F1F1F10(aq)|Pt(s)

Accepted Answer

A) Cd(s) 
B) Cd2F1F1F1S1F1F1F10(aq) 
C) Fe2F1F1F1S1F1F1F10(aq) 
D) Fe3F1F1F1S1F1F1F10(aq) 
E) Pt(s) 
A) Cd(s) 
B) Cd2F1F1F1S1F1F1F10(aq) 
C) Fe2F1F1F1S1F1F1F10(aq) 
D) Fe3F1F1F1S1F1F1F10(aq) 
E) Pt(s)

Question 10

Sodium carbonate is produced using the Solvay process, which involves a final step where sodium bicarbonate is heated to produce sodium carbonate, water, and carbon dioxide. What are the oxidation numbers of the sodium, carbon, and oxygen, respectively, in sodium carbonate?

Accepted Answer

A) (F1F1F1S1F1F1F101, F1F1F1S1F1F1F104, and F1F1F1S1F1F1F102) 
B) (F1F1F1S1F1F1F101, F1F1F1S1F1F1F102, and F1F1F1S1F1F1F102) 
C) 0, F1F1F1S1F1F1F102, and F1F1F1S1F1F1F102) 
D) (F1F1F1S1F1F1F101, F1F1F1S1F1F1F102, and F1F1F1S1F1F1F102) 
E) (F1F1F1S1F1F1F101, F1F1F1S1F1F1F102, and 0) 
A) (F1F1F1S1F1F1F101, F1F1F1S1F1F1F104, and F1F1F1S1F1F1F102) 
B) (F1F1F1S1F1F1F101, F1F1F1S1F1F1F102, and F1F1F1S1F1F1F102) 
C) 0, F1F1F1S1F1F1F102, and F1F1F1S1F1F1F102) 
D) (F1F1F1S1F1F1F101, F1F1F1S1F1F1F102, and F1F1F1S1F1F1F102) 
E) (F1F1F1S1F1F1F101, F1F1F1S1F1F1F102, and 0)

Question 11

Which one of the following is not an advantage of lithium batteries?

Accepted Answer

A) the extremely negative standard reduction potential of lithium 
B) the small molar mass of lithium 
C) the high mobility of lithium in solids 
D) the small cell potentials produced by these batteries 
E) a high battery capacity 
A) the extremely negative standard reduction potential of lithium 
B) the small molar mass of lithium 
C) the high mobility of lithium in solids 
D) the small cell potentials produced by these batteries 
E) a high battery capacity

Question 12

What must be true about the standard reduction potentials for the following reaction to proceed spontaneously?

Accepted Answer

The standard reduction potenti

Question 13

In the following reaction   what is the change in oxidation number for S?

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 14

If in using a lead-acid battery to start a car, 1.00 gram 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

A) 15.5 min 
B) 1,864 min 
C) 31.1 min 
D) 21.2 min 
E) 42.4 min 
A) 15.5 min 
B) 1,864 min 
C) 31.1 min 
D) 21.2 min 
E) 42.4 min

Question 15

Reduction is the ________

Accepted Answer

A) gain of electrons. 
B) loss of electrons. 
C) gain of protons. 
D) loss of protons. 
E) loss of mass. 
A) gain of electrons. 
B) loss of electrons. 
C) gain of protons. 
D) loss of protons. 
E) loss of mass.

Question 16

A voltaic cell is constructed based on the oxidation of zinc metal and the reduction of silver cations. Solutions of silver nitrate and zinc nitrate also were used. Locate the salt bridge in the diagram.

Accepted Answer

A) a 
B) b 
C) c 
D) d 
A) a 
B) b 
C) c 
D) d

Question 17

How does a fuel cell differ from a conventional battery?

Accepted Answer

A conventional battery has a f

Question 18

Which statement does not correctly describe a standard hydrogen electrode (SHE)?

Accepted Answer

A) The SHE is assigned a standard reduction potential of exactly 1 V. 
B)    
C) Pt|H2(g, 1atm)|HF1F1F1S1F1F1F10(aq, 1 M )|| 
D) ||HF1F1F1S1F1F1F10(aq, 1 M )|H2(g, 1atm)|Pt 
E) The SHE consists of a platinum electrode immersed in an acid solution and a stream of hydrogen gas. 
A) The SHE is assigned a standard reduction potential of exactly 1 V. 
B)    
C) Pt|H2(g, 1atm)|HF1F1F1S1F1F1F10(aq, 1 M )|| 
D) ||HF1F1F1S1F1F1F10(aq, 1 M )|H2(g, 1atm)|Pt 
E) The SHE consists of a platinum electrode immersed in an acid solution and a stream of hydrogen gas.

Question 19

Neuron cells generate electrical signals by concentration gradients across membranes. Assuming a potassium ion concentration of 0.003 M inside the cell, and a concentration of 0.135 M outside the cell, what is the electrical potential across the cell membrane? Body temperature is 310 K. The sign identifies the change in the electrical potential across the membrane and which way the ions flow.

Accepted Answer

A) (F1F1F1S1F1F1F10204 mV) 
B) (F1F1F1S1F1F1F10102 mV) 
C) (F1F1F1S1F1F1F1010.0 mV) 
D) (F1F1F1S1F1F1F10204 mV) 
E) (F1F1F1S1F1F1F10136 mV) 
A) (F1F1F1S1F1F1F10204 mV) 
B) (F1F1F1S1F1F1F10102 mV) 
C) (F1F1F1S1F1F1F1010.0 mV) 
D) (F1F1F1S1F1F1F10204 mV) 
E) (F1F1F1S1F1F1F10136 mV)

Question 20

The standard cell potential for the nickel-cadmium battery is 1.35 V, and the cell reaction can be written as   Which one of the following statements do you expect to be true based on the Nernst equation? Note Q F1F1F1S1F1F1F10 reaction quotient, and K F1F1F1S1F1F1F10 equilibrium constant for the cell reaction.

Accepted Answer

A) As the battery is used, the cell voltage approaches zero because Q approaches K in value. 
B) When the battery no longer works, the cell voltage is zero because Q F1F1F1S1F1F1F10 K. 
C) As the battery is used, the cell voltage does not change because Q equals 1. 
D) When the battery is fully charged, Q F1F1F1S1F1F1F10 K. 
E) When the battery is fully charged, Q F1F1F1S1F1F1F10 K. 
A) As the battery is used, the cell voltage approaches zero because Q approaches K in value. 
B) When the battery no longer works, the cell voltage is zero because Q F1F1F1S1F1F1F10 K. 
C) As the battery is used, the cell voltage does not change because Q equals 1. 
D) When the battery is fully charged, Q F1F1F1S1F1F1F10 K. 
E) When the battery is fully charged, Q F1F1F1S1F1F1F10 K.

Exam 18: Electrochemistry: The Quest for Clean Energy

Which statement about this concentration cell is incorrect?

If the free-energy change of the following voltaic cell is 46.3 kJ, what is the standard potential of the cell?

Which statement regarding battery-powered electric cars is not correct? Currently, battery-powered electric cars ________

Copper metal is purified by electrolysis. How much copper metal could be produced from copper(II) oxide by applying a current of 10.0 amps at the appropriate negative potential for 12.0 hours?

The energy supplied by a battery can be determined by ________

A voltaic cell is constructed based on the oxidation of zinc metal and the reduction of silver cations. Solutions of silver nitrate and zinc nitrate also were used. Locate the silver metal on the diagram.

Use the table of standard reduction potentials below to identify the metal or metal ion that is the weakest reducing agent. Standard Reduction Potentials (volts) in Aqueous Solution 1.70 0.520 0.036 0.400 0.73 1.66

Consider the following standard reduction potentials. Reduction Half-Reaction (volts)  2.38  0.76 0.16 The Mg/Mg2 half-reaction can be paired with the other two to produce voltaic cells because ________

The diagram below represents a voltaic cell. In this cell, which species is oxidized? Cd(s)|Cd2(aq)||Fe2(aq),Fe3(aq)|Pt(s)

Sodium carbonate is produced using the Solvay process, which involves a final step where sodium bicarbonate is heated to produce sodium carbonate, water, and carbon dioxide. What are the oxidation numbers of the sodium, carbon, and oxygen, respectively, in sodium carbonate?

Which one of the following is not an advantage of lithium batteries?

What must be true about the standard reduction potentials for the following reaction to proceed spontaneously?

In the following reaction what is the change in oxidation number for S?

If in using a lead-acid battery to start a car, 1.00 gram 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?

Reduction is the ________

A voltaic cell is constructed based on the oxidation of zinc metal and the reduction of silver cations. Solutions of silver nitrate and zinc nitrate also were used. Locate the salt bridge in the diagram.

How does a fuel cell differ from a conventional battery?

Which statement does not correctly describe a standard hydrogen electrode (SHE)?

The standard cell potential for the nickel-cadmium battery is 1.35 V, and the cell reaction can be written as Which one of the following statements do you expect to be true based on the Nernst equation? Note Q  reaction quotient, and K  equilibrium constant for the cell reaction.

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

Consider the following standard reduction potentials. Reduction Half-Reaction (volts)  2.38  0.76 0.16 The Mg/Mg²^half-reaction can be paired with the other two to produce voltaic cells because ________

The diagram below represents a voltaic cell. In this cell, which species is oxidized? Cd(s)|Cd²^(aq)||Fe²^(aq),Fe³^(aq)|Pt(s)

If in using a lead-acid battery to start a car, 1.00 gram 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?