Question 1

Oxidation occurs at the cathode of a galvanic cell, but at the anode of an electrolytic cell.

Accepted Answer

A) True 
 B)False

Question 2

When metal A is placed in a solution of metal ions B2+, a reaction occurs between A and B2+, and metal ions A2+ appear in the solution. When metal B is placed in acid solution, gas bubbles form on its surface. When metal A is placed in a solution of metal ions C2+, no reaction occurs. Which of the following reactions would not occur spontaneously?

Accepted Answer

A)  C(s) + 2H+(aq) $\rightarrow$H2(g) + C2+(aq) 
B)  C(s) + A2+(aq) $\rightarrow$ A(s) + C2+(aq) 
C)  B(s) + C2+(aq) $\rightarrow$ C(s) + B2+(aq) 
D)  A(s) + 2H+(aq) $\rightarrow$ H2(g) + A2+(aq) 
E)  B(s) + 2H+(aq) $\rightarrow$H2(g) + B2+(aq) 
A)  C(s) + 2H+(aq) $\rightarrow$H2(g) + C2+(aq) 
B)  C(s) + A2+(aq) $\rightarrow$ A(s) + C2+(aq) 
C)  B(s) + C2+(aq) $\rightarrow$ C(s) + B2+(aq) 
D)  A(s) + 2H+(aq) $\rightarrow$ H2(g) + A2+(aq) 
E)  B(s) + 2H+(aq) $\rightarrow$H2(g) + B2+(aq)

Question 3

What product forms at the anode during the electrolysis of molten NaBr?

Accepted Answer

A)  Na+(l) 
B)  Na(l) 
C)  Br¯(l) 
D)  Br3¯(l) 
E)  Br2(g) 
A)  Na+(l) 
B)  Na(l) 
C)  Br¯(l) 
D)  Br3¯(l) 
E)  Br2(g)

Question 4

A voltaic cell prepared using zinc and iodine has the following cell notation.   Which of the following equations correctly represents the balanced, spontaneous cell reaction?

Accepted Answer

A)  2I¯(aq) + Zn2+(aq) $\rightarrow$ I2(s) + Zn(s) 
B)  I2(s) + Zn(s) $\rightarrow$ 2I¯(aq) + Zn2+(aq) 
C)  2I¯(aq) + Zn(s) $\rightarrow$I2(s) + Zn2+(aq) 
D)  I2(s) + Zn2+(aq) $\rightarrow$ 2I¯(aq) + Zn(s) 
E)  None of these choices, since graphite must be in the equation. 
A)  2I¯(aq) + Zn2+(aq) $\rightarrow$ I2(s) + Zn(s) 
B)  I2(s) + Zn(s) $\rightarrow$ 2I¯(aq) + Zn2+(aq) 
C)  2I¯(aq) + Zn(s) $\rightarrow$I2(s) + Zn2+(aq) 
D)  I2(s) + Zn2+(aq) $\rightarrow$ 2I¯(aq) + Zn(s) 
E)  None of these choices, since graphite must be in the equation.

Question 5

The value of E $\degree$cell for the reaction   is 1.59 V. Calculate $\Delta$G $\degree$ for the reaction.

Accepted Answer

A)  -921 kJ 
B)  -767 kJ 
C)  -460 kJ 
D)  -307 kJ 
E)  None of these choices is correct. 
A)  -921 kJ 
B)  -767 kJ 
C)  -460 kJ 
D)  -307 kJ 
E)  None of these choices is correct.

Question 6

A concentration cell is based on the aqueous reaction   The cell consists of copper electrodes dipping into solutions of Cu2+ ions. The anions present are sulfate ions. Draw a neat diagram to represent this cell, showing and labeling all necessary components including: anode, cathode, electron flow, cation flow and anion flow.

Accepted Answer

Question 7

A salt bridge provides a path for electrons to move between the anode and cathode compartments of a voltaic cell.

Accepted Answer

A) True 
 B)False

Question 8

Calculate E$\degree$cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous.   Overall reaction:

Accepted Answer

A)  E$\degree$cell = -1.00 V, nonspontaneous 
B)  E$\degree$cell = -1.00 V, spontaneous 
C)  E$\degree$cell = 1.00 V, nonspontaneous 
D)  E$\degree$cell = 1.00 V, spontaneous 
E)  E$\degree$cell = -0.23 V, nonspontaneous 
A)  E$\degree$cell = -1.00 V, nonspontaneous 
B)  E$\degree$cell = -1.00 V, spontaneous 
C)  E$\degree$cell = 1.00 V, nonspontaneous 
D)  E$\degree$cell = 1.00 V, spontaneous 
E)  E$\degree$cell = -0.23 V, nonspontaneous

Question 9

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

Accepted Answer

A)  The anode will definitely gain weight in a voltaic cell. 
B)  Oxidation occurs at the cathode of both cells. 
C)  The free energy change, $\Delta$G, is negative for the voltaic cell. 
D)  The electrons in the external wire flow from cathode to anode in an electrolytic cell. 
E)  None of these choices is correct. 
A)  The anode will definitely gain weight in a voltaic cell. 
B)  Oxidation occurs at the cathode of both cells. 
C)  The free energy change, $\Delta$G, is negative for the voltaic cell. 
D)  The electrons in the external wire flow from cathode to anode in an electrolytic cell. 
E)  None of these choices is correct.

Question 10

Consider the reaction: CuO(s) + H2(g) $\rightarrow$ Cu(s) + H2O(l) In this reaction, which substances are the oxidant and reductant, respectively?

Accepted Answer

A)  CuO and H2 
B)  H2 and CuO 
C)  CuO and Cu 
D)  H2O and H2 
E)  None of these choices is correct. 
A)  CuO and H2 
B)  H2 and CuO 
C)  CuO and Cu 
D)  H2O and H2 
E)  None of these choices is correct.

Question 11

A voltaic cell consists of a Mn/Mn2+ electrode (E$\degree$= -1.18 V) and a Fe/Fe2+ electrode (E$\degree$= -0.44 V). Calculate [Fe2+] if [Mn2+] = 0.050 M and Ecell = 0.78 V at 25$\degree$C.

Accepted Answer

A)  0.040 M 
B)  0.24 M 
C)  1.1 M 
D)  1.8 M 
E)  None of these choices is correct. 
A)  0.040 M 
B)  0.24 M 
C)  1.1 M 
D)  1.8 M 
E)  None of these choices is correct.

Question 12

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for zinc will be _____.

Accepted Answer

A)  2 
B)  7 
C)  8 
D)  16 
E)  None of these choices is correct. 
A)  2 
B)  7 
C)  8 
D)  16 
E)  None of these choices is correct.

Question 13

A concentration cell is based on the aqueous reaction   The cell consists of copper electrodes dipping into solutions of Cu2+ ions. The anions present are sulfate ions. Write the shorthand cell notation for this cell.

Accepted Answer

Question 14

Consider the reaction of iodine with manganese dioxide: 
3I2(s) + 2MnO2(s) + 8OH¯(aq)   6I¯(aq) + 2MnO4¯(aq) + 4H2O(l)
The equilibrium constant for the overall reaction is 8.30 *10¯7. Calculate E$\degree$cell for the reaction at 25$\degree$C.

Accepted Answer

A)  -0.36 V 
B)  -0.18 V 
C)  -0.12 V 
D)  -0.060 V 
E)  None of these choices is correct. 
A)  -0.36 V 
B)  -0.18 V 
C)  -0.12 V 
D)  -0.060 V 
E)  None of these choices is correct.

Question 15

A battery is considered "dead" when:

Accepted Answer

A)  Q  1 
D)  Q = K 
E)  Q/K = 0 
A)  Q  1 
D)  Q = K 
E)  Q/K = 0

Question 16

The lead-acid battery is an example of a secondary battery.

Accepted Answer

A) True 
 B)False

Question 17

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the hydrogen sulfate ion will be ______.

Accepted Answer

A)  1 
B)  3 
C)  4 
D)  8 
E)  None of these choices is correct. 
A)  1 
B)  3 
C)  4 
D)  8 
E)  None of these choices is correct.

Question 18

What product forms at the cathode during the electrolysis of molten lithium iodide?

Accepted Answer

A)  Li+(l) 
B)  Li(l) 
C)  I¯(l) 
D)  I2(g) 
E)  I3¯(l) 
A)  Li+(l) 
B)  Li(l) 
C)  I¯(l) 
D)  I2(g) 
E)  I3¯(l)

Question 19

A cell can be prepared from copper and tin. What is the E$\degree$cell for the cell that forms from the following half-reactions?

Accepted Answer

A)  0.47 V 
B)  0.21 V 
C)  -0.21 V 
D)  -0.47 V 
E)  0.42 V 
A)  0.47 V 
B)  0.21 V 
C)  -0.21 V 
D)  -0.47 V 
E)  0.42 V

Question 20

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

Accepted Answer

A) True 
 B)False

Oxidation occurs at the cathode of a galvanic cell, but at the anode of an electrolytic cell.

What product forms at the anode during the electrolysis of molten NaBr?

A voltaic cell prepared using zinc and iodine has the following cell notation. Which of the following equations correctly represents the balanced, spontaneous cell reaction?

The value of E $\degree$ _cell for the reaction $The value of E \degree <sub>cell</sub> for the reaction is 1.59 V. Calculate \Delta G \degree for the reaction.$ is 1.59 V. Calculate $\Delta$ G $\degree$ for the reaction.

A salt bridge provides a path for electrons to move between the anode and cathode compartments of a voltaic cell.

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

Consider the reaction: CuO(s) + H₂(g) $\rightarrow$ Cu(s) + H₂O(l) In this reaction, which substances are the oxidant and reductant, respectively?

A voltaic cell consists of a Mn/Mn²⁺ electrode (E $\degree$ = -1.18 V) and a Fe/Fe²⁺ electrode (E $\degree$ = -0.44 V). Calculate [Fe²⁺] if [Mn²⁺] = 0.050 M and E_cell = 0.78 V at 25 $\degree$ C.

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for zinc will be _____.

A concentration cell is based on the aqueous reaction The cell consists of copper electrodes dipping into solutions of Cu²⁺ ions. The anions present are sulfate ions. Write the shorthand cell notation for this cell.

A battery is considered "dead" when:

The lead-acid battery is an example of a secondary battery.

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the hydrogen sulfate ion will be ______.

What product forms at the cathode during the electrolysis of molten lithium iodide?

A cell can be prepared from copper and tin. What is the E $\degree$ _cell for the cell that forms from the following half-reactions? $A cell can be prepared from copper and tin. What is the E \degree <sub>cell</sub> for the cell that forms from the following half-reactions?$

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

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

Three 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

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

Exam 21: Electrochemistry: Chemical Change and Electrical Work

Oxidation occurs at the cathode of a galvanic cell, but at the anode of an electrolytic cell.

What product forms at the anode during the electrolysis of molten NaBr?

A voltaic cell prepared using zinc and iodine has the following cell notation. Which of the following equations correctly represents the balanced, spontaneous cell reaction?

The value of E °\degree° cell for the reaction is 1.59 V. Calculate Δ\DeltaΔ G °\degree° for the reaction.

A salt bridge provides a path for electrons to move between the anode and cathode compartments of a voltaic cell.

Calculate E °\degree° cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. Overall reaction:

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

Consider the reaction: CuO(s) + H2(g) →\rightarrow→ Cu(s) + H2O(l) In this reaction, which substances are the oxidant and reductant, respectively?

A voltaic cell consists of a Mn/Mn2+ electrode (E °\degree° = -1.18 V) and a Fe/Fe2+ electrode (E °\degree° = -0.44 V). Calculate [Fe2+] if [Mn2+] = 0.050 M and Ecell = 0.78 V at 25 °\degree° C.

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for zinc will be _____.

A concentration cell is based on the aqueous reaction The cell consists of copper electrodes dipping into solutions of Cu2+ ions. The anions present are sulfate ions. Write the shorthand cell notation for this cell.

Consider the reaction of iodine with manganese dioxide: 3I2(s) + 2MnO2(s) + 8OH¯(aq) 6I¯(aq) + 2MnO4¯(aq) + 4H2O(l) The equilibrium constant for the overall reaction is 8.30 *10¯7. Calculate E °\degree° cell for the reaction at 25 °\degree° C.

A battery is considered "dead" when:

The lead-acid battery is an example of a secondary battery.

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the hydrogen sulfate ion will be ______.

What product forms at the cathode during the electrolysis of molten lithium iodide?

A cell can be prepared from copper and tin. What is the E °\degree° cell for the cell that forms from the following half-reactions?

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

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

Three 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

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

The value of E $\degree$ _cell for the reaction $The value of E \degree <sub>cell</sub> for the reaction is 1.59 V. Calculate \Delta G \degree for the reaction.$ is 1.59 V. Calculate $\Delta$ G $\degree$ for the reaction.

Consider the reaction: CuO(s) + H₂(g) $\rightarrow$ Cu(s) + H₂O(l) In this reaction, which substances are the oxidant and reductant, respectively?

A voltaic cell consists of a Mn/Mn²⁺ electrode (E $\degree$ = -1.18 V) and a Fe/Fe²⁺ electrode (E $\degree$ = -0.44 V). Calculate [Fe²⁺] if [Mn²⁺] = 0.050 M and E_cell = 0.78 V at 25 $\degree$ C.

A concentration cell is based on the aqueous reaction The cell consists of copper electrodes dipping into solutions of Cu²⁺ ions. The anions present are sulfate ions. Write the shorthand cell notation for this cell.

A cell can be prepared from copper and tin. What is the E $\degree$ _cell for the cell that forms from the following half-reactions? $A cell can be prepared from copper and tin. What is the E \degree <sub>cell</sub> for the cell that forms from the following half-reactions?$

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