Question 1

Which component of the following cell notation is the anode? P | Q || R | S

Accepted Answer

A)  P 
B)  Q 
C)  R 
D)  S 
E)  One of the | symbols is the anode. 
A)  P 
B)  Q 
C)  R 
D)  S 
E)  One of the | symbols is the anode.

Question 2

A voltaic cell prepared using aluminum and nickel has the following cell notation. 
Al(s) | Al3+(aq) || Ni2+(aq) | Ni(s)
Which of the following represents the correctly balanced spontaneous reaction equation for the cell?

Accepted Answer

A)  Ni2+(aq) + Al(s) F1F1F1S1F1F1F10 Al3+(aq) + Ni(s) 
B)  3Ni2+(aq) + 2Al(s) F1F1F1S1F1F1F10 2Al3+(aq) + 3Ni(s) 
C)  Ni(s) + Al3+(aq) F1F1F1S1F1F1F10 Ni2+(aq) + Al(s) 
D)  3Ni(s) + 2Al3+(aq) F1F1F1S1F1F1F10 3Ni2+(aq) + 2Al(s) 
E)  none of the above 
A)  Ni2+(aq) + Al(s) F1F1F1S1F1F1F10 Al3+(aq) + Ni(s) 
B)  3Ni2+(aq) + 2Al(s) F1F1F1S1F1F1F10 2Al3+(aq) + 3Ni(s) 
C)  Ni(s) + Al3+(aq) F1F1F1S1F1F1F10 Ni2+(aq) + Al(s) 
D)  3Ni(s) + 2Al3+(aq) F1F1F1S1F1F1F10 3Ni2+(aq) + 2Al(s) 
E)  none of the above

Question 3

The voltaic cell made up of cobalt, copper, and their M2+ ions, has E°cell = 0.62 V. If E° of the cathode half-cell is 0.34 V, what is E° of the anode half-cell? 
Cu2+(aq) + Co(s) F1F1F1S1F1F1F10 Cu(s) + Co2+(aq)

Accepted Answer

A)  -0.28 V 
B)  -0.96 V 
C)  0.28 V 
D)  0.96 V 
E)  none of the above 
A)  -0.28 V 
B)  -0.96 V 
C)  0.28 V 
D)  0.96 V 
E)  none of the above

Question 4

In the electrolyte of an electrochemical cell, current is carried by electrons moving from the anode to the cathode.

Accepted Answer

A) True 
 B)False

Question 5

Explain what is meant by a fuel cell. Provide a balanced equation to represent the reaction in any fuel cell of your choice.

Accepted Answer

A fuel cell is a voltaic cell in which t

Question 6

Which of the following statements about voltaic and electrolytic cells is correct?

Accepted Answer

A)  The electrons in the external wire flow from cathode to anode in both types of cell. 
B)  Oxidation occurs at the cathode only in a voltaic cell. 
C)  The free energy change, F1F1F1S1F1F1F10G, is negative for an electrolytic cell. 
D)  The cathode is labeled as positive (+) in a voltaic cell but negative (-) in an electrolytic cell. 
E)  Reduction occurs at the anode in an electrolytic cell. 
A)  The electrons in the external wire flow from cathode to anode in both types of cell. 
B)  Oxidation occurs at the cathode only in a voltaic cell. 
C)  The free energy change, F1F1F1S1F1F1F10G, is negative for an electrolytic cell. 
D)  The cathode is labeled as positive (+) in a voltaic cell but negative (-) in an electrolytic cell. 
E)  Reduction occurs at the anode in an electrolytic cell.

Question 7

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the hydrogen sulfate ion will be ______. 
Al(s) + HSO4-(aq) + OH-(aq) F1F1F1S1F1F1F10 Al2O3(s) + S2-(aq) + H2O(l)

Accepted Answer

A)  1 
B)  3 
C)  4 
D)  8 
E)  none of the above 
A)  1 
B)  3 
C)  4 
D)  8 
E)  none of the above

Question 8

Consider the reaction in the lead-acid cell 
Pb(s) + PbO2(s) + 2H2SO4(aq) F1F1F1S1F1F1F10 2PbSO4(aq) + 2H2O(l)
For which E°cell = 2.04 V at 298 K. F1F1F1S1F1F1F10G° for this reaction is

Accepted Answer

A)  -3.94 × 105 kJ. 
B)  -3.94 × 102 kJ. 
C)  -1.97 × 105 kJ. 
D)  -7.87 × 102 kJ. 
E)  none of the above. 
A)  -3.94 × 105 kJ. 
B)  -3.94 × 102 kJ. 
C)  -1.97 × 105 kJ. 
D)  -7.87 × 102 kJ. 
E)  none of the above.

Question 9

For the reaction occurring in a voltaic (galvanic) cell, F1F1F1S1F1F1F10G > 0.

Accepted Answer

A) True 
 B)False

Question 10

Chromium metal is electroplated from acidic aqueous solutions containing the dichromate ion, Cr2O72-. What is the minimum time needed to plate out 10.0 g of chromium metal from such a solution, if the current is 50.0 A?

Accepted Answer

A)  6.2 minutes 
B)  12.4 minutes 
C)  18.6 minutes 
D)  24.7 minute 
E)  37.1 minutes 
A)  6.2 minutes 
B)  12.4 minutes 
C)  18.6 minutes 
D)  24.7 minute 
E)  37.1 minutes

Question 11

Write down equations representing the anode half-reaction, the cathode half-reaction, and the overall cell reaction for the lead-acid battery.

Accepted Answer

Anode half-reaction: Pb(s) + SO₄^2-(aq) F1F1

Question 12

The value of the equilibrium constant for the reaction of nickel(II) ions with cadmium metal is 1.17 × 105. Calculate F1F1F1S1F1F1F10G° for the reaction at 25°C.

Accepted Answer

A)  -12.6 kJ 
B)  -28.9 kJ 
C)  12.6 kJ 
D)  28.9 kJ 
E)  none of the above 
A)  -12.6 kJ 
B)  -28.9 kJ 
C)  12.6 kJ 
D)  28.9 kJ 
E)  none of the above

Question 13

Calculate E°cell for the reaction of nickel(II) ions with cadmium metal at 25°C. K = 1.17 × 105
 Ni2+(aq) + Cd(s) F1F1F1S1F1F1F10 Cd2+(aq) + Ni(s)

Accepted Answer

A)  0.075 V 
B)  0.10 V 
C)  0.12 V 
D)  0.15 V 
E)  0.30 V 
A)  0.075 V 
B)  0.10 V 
C)  0.12 V 
D)  0.15 V 
E)  0.30 V

Question 14

What mass of silver will be formed when 15.0 A are passed through molten AgCl for 25.0 minutes?

Accepted Answer

A)  0.419 g 
B)  6.29 g 
C)  12.6 g 
D)  25.2 g 
E)  33.4 g 
A)  0.419 g 
B)  6.29 g 
C)  12.6 g 
D)  25.2 g 
E)  33.4 g

Question 15

A concentration cell consists of two Al/Al3+electrodes. The electrolyte in compartment A is 0.050 M Al(NO3)3 and in compartment B is 1.25 M Al(NO3)3. What is the voltage of the cell at 25°C?

Accepted Answer

A)  0.083 V 
B)  0.062 V 
C)  0.041V 
D)  0.028 V 
E)  none of the above 
A)  0.083 V 
B)  0.062 V 
C)  0.041V 
D)  0.028 V 
E)  none of the above

Question 16

Which one of the following statements about electrochemical cells is correct?

Accepted Answer

A)  In a salt bridge, current is carried by cations moving toward the anode, and anions toward the cathode. 
B)  In the external wire, electrons travel from cathode to anode. 
C)  The anode of a voltaic cell is labeled minus (-). 
D)  Oxidation occurs at the cathode, in an electrolytic cell. 
E)  None of the above statements is correct. 
A)  In a salt bridge, current is carried by cations moving toward the anode, and anions toward the cathode. 
B)  In the external wire, electrons travel from cathode to anode. 
C)  The anode of a voltaic cell is labeled minus (-). 
D)  Oxidation occurs at the cathode, in an electrolytic cell. 
E)  None of the above statements is correct.

Question 17

Given that E° for X + e- F1F1F1S1F1F1F10 Y is greater than E° for A + 2e- F1F1F1S1F1F1F10 B, it is correct to say that, under standard conditions

Accepted Answer

A)  X will oxidize A. 
B)  Y will oxidize A. 
C)  Y will reduce A. 
D)  B will oxidize X. 
E)  B will reduce X. 
A)  X will oxidize A. 
B)  Y will oxidize A. 
C)  Y will reduce A. 
D)  B will oxidize X. 
E)  B will reduce X.

Question 18

In the electrolysis of aqueous potassium nitrate using inert electrodes, which one of the following species is oxidized?

Accepted Answer

A)  potassium ion 
B)  nitrate ion 
C)  water 
D)  oxygen 
E)  hydronium ion 
A)  potassium ion 
B)  nitrate ion 
C)  water 
D)  oxygen 
E)  hydronium ion

Question 19

Which of the following elements can be isolated by electrolysis of the aqueous salt shown?

Accepted Answer

A)  phosphorus from K3PO4(aq) 
B)  sodium from NaBr(aq) 
C)  aluminum from AlCl3(aq) 
D)  fluorine from KF(aq) 
E)  iodine from NaI(aq) 
A)  phosphorus from K3PO4(aq) 
B)  sodium from NaBr(aq) 
C)  aluminum from AlCl3(aq) 
D)  fluorine from KF(aq) 
E)  iodine from NaI(aq)

Question 20

Which one of the following is not a redox reaction?

Accepted Answer

A)  Al(OH)4-(aq) + 4H+(aq) F1F1F1S1F1F1F10 Al3+(aq) + 4H2O(l) 
B)  C6H12O6(s) + 6O2(g) F1F1F1S1F1F1F10 6CO2(g) + 6H2O(l) 
C)  Na6FeCl8(s) + 2Na(l) F1F1F1S1F1F1F10 8NaCl(s) + Fe(s) 
D)  2H2O2(aq) F1F1F1S1F1F1F10 2H2O(l) + O2(g) 
E)  CO2(g) + H2(g) F1F1F1S1F1F1F10 CO(g) + H2O(g) 
A)  Al(OH)4-(aq) + 4H+(aq) F1F1F1S1F1F1F10 Al3+(aq) + 4H2O(l) 
B)  C6H12O6(s) + 6O2(g) F1F1F1S1F1F1F10 6CO2(g) + 6H2O(l) 
C)  Na6FeCl8(s) + 2Na(l) F1F1F1S1F1F1F10 8NaCl(s) + Fe(s) 
D)  2H2O2(aq) F1F1F1S1F1F1F10 2H2O(l) + O2(g) 
E)  CO2(g) + H2(g) F1F1F1S1F1F1F10 CO(g) + H2O(g)

Exam 21: Electrochemistry: Chemical Change and Electrical Work

Which component of the following cell notation is the anode? P | Q || R | S

A voltaic cell prepared using aluminum and nickel has the following cell notation. Al(s) | Al3+(aq) || Ni2+(aq) | Ni(s) Which of the following represents the correctly balanced spontaneous reaction equation for the cell?

The voltaic cell made up of cobalt, copper, and their M2+ ions, has E°cell = 0.62 V. If E° of the cathode half-cell is 0.34 V, what is E° of the anode half-cell? Cu2+(aq) + Co(s)  Cu(s) + Co2+(aq)

In the electrolyte of an electrochemical cell, current is carried by electrons moving from the anode to the cathode.

Explain what is meant by a fuel cell. Provide a balanced equation to represent the reaction in any fuel cell of your choice.

Which of the following statements about voltaic and electrolytic cells is correct?

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the hydrogen sulfate ion will be ______. Al(s) + HSO4-(aq) + OH-(aq)  Al2O3(s) + S2-(aq) + H2O(l)

Consider the reaction in the lead-acid cell Pb(s) + PbO2(s) + 2H2SO4(aq)  2PbSO4(aq) + 2H2O(l) For which E°cell = 2.04 V at 298 K. G° for this reaction is

For the reaction occurring in a voltaic (galvanic) cell, G > 0.

Chromium metal is electroplated from acidic aqueous solutions containing the dichromate ion, Cr2O72-. What is the minimum time needed to plate out 10.0 g of chromium metal from such a solution, if the current is 50.0 A?

Write down equations representing the anode half-reaction, the cathode half-reaction, and the overall cell reaction for the lead-acid battery.

The value of the equilibrium constant for the reaction of nickel(II) ions with cadmium metal is 1.17 × 105. Calculate G° for the reaction at 25°C.

Calculate E°cell for the reaction of nickel(II) ions with cadmium metal at 25°C. K = 1.17 × 105 Ni2+(aq) + Cd(s)  Cd2+(aq) + Ni(s)

What mass of silver will be formed when 15.0 A are passed through molten AgCl for 25.0 minutes?

A concentration cell consists of two Al/Al3+electrodes. The electrolyte in compartment A is 0.050 M Al(NO3)3 and in compartment B is 1.25 M Al(NO3)3. What is the voltage of the cell at 25°C?

Which one of the following statements about electrochemical cells is correct?

Given that E° for X + e-  Y is greater than E° for A + 2e-  B, it is correct to say that, under standard conditions

In the electrolysis of aqueous potassium nitrate using inert electrodes, which one of the following species is oxidized?

Which of the following elements can be isolated by electrolysis of the aqueous salt shown?

Which one of the following is not a redox reaction?

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

The Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry: Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids, Solids, and Phase Changes

The Properties of Mixtures: Solutions and Colloids

Periodic Patterns in the Main Group Elements: Bonding, Structure, and Reactivity

Organic Compounds and the Atomic Properties of Carbon

Kinetics: Rates and Mechanisms of Chemical Reactions

Equilibrium: the Extent of Chemical Reactions

Acid-Base Equilibria

Ionic Equilibria in Aqueous Systems

Thermodynamics: Entropy, Free Energy, and the Direction of Chemical Reactions

The Elements in Nature and Industry

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

A voltaic cell prepared using aluminum and nickel has the following cell notation. Al(s) | Al³⁺(aq) || Ni²⁺(aq) | Ni(s) Which of the following represents the correctly balanced spontaneous reaction equation for the cell?

The voltaic cell made up of cobalt, copper, and their M²⁺ ions, has E°_cell = 0.62 V. If E° of the cathode half-cell is 0.34 V, what is E° of the anode half-cell? Cu²⁺(aq) + Co(s)  Cu(s) + Co²⁺(aq)

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the hydrogen sulfate ion will be ______. Al(s) + HSO₄^-(aq) + OH^-(aq)  Al₂O₃(s) + S^2-(aq) + H₂O(l)

Consider the reaction in the lead-acid cell Pb(s) + PbO₂(s) + 2H₂SO₄(aq)  2PbSO₄(aq) + 2H₂O(l) For which E°_cell = 2.04 V at 298 K. G° for this reaction is

Chromium metal is electroplated from acidic aqueous solutions containing the dichromate ion, Cr₂O₇^2-. What is the minimum time needed to plate out 10.0 g of chromium metal from such a solution, if the current is 50.0 A?

The value of the equilibrium constant for the reaction of nickel(II) ions with cadmium metal is 1.17 × 10⁵. Calculate G°for the reaction at 25°C.

Calculate E°_cell for the reaction of nickel(II) ions with cadmium metal at 25°C. K = 1.17 × 10⁵ Ni²⁺(aq) + Cd(s)  Cd²⁺(aq) + Ni(s)

A concentration cell consists of two Al/Al³⁺electrodes. The electrolyte in compartment A is 0.050 M Al(NO₃)₃and in compartment B is 1.25 M Al(NO₃)₃. What is the voltage of the cell at 25°C?

Given that E° for X + e^-  Y is greater than E° for A + 2e^-  B, it is correct to say that, under standard conditions