Question 1

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,$\Delta$G,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,$\Delta$G,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 2

In the shorthand notation for cells,a double vertical line is used to separate the reduced and oxidized forms of a redox couple.

Accepted Answer

A) True 
 B)False

Question 3

Calculate E°cell for the reaction of nickel(II)ions with cadmium metal at 25°C.K = 1.17 $\times$ 105
 Ni2+(aq)+ Cd(s) $\to$ 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 4

Which one of the following pairs of substances could be used to construct a single redox electrode (i.e. ,they have an element in common,but in different oxidation states)?

Accepted Answer

A) HCl and Cl- 
B) H+ and OH- 
C) H2O and H+ 
D) Fe3+ and Fe2O3 
E) MnO2 and Mn2+ 
A) HCl and Cl- 
B) H+ and OH- 
C) H2O and H+ 
D) Fe3+ and Fe2O3 
E) MnO2 and Mn2+

Question 5

A cell can be prepared from copper and tin.What is the E°cell for the cell that forms from the following half-reactions?
Cu2+(aq)+ 2e-  
Cu(s);E° = 0.34 V
Sn4+(aq)+ 2e-  
Sn2+(aq);E° = 0.13 V

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 6

Consider the reaction
CuO(s)+ H2(g) $\to$ 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 7

Two cells are connected in series,so that the same current flows through two electrodes where the following half-reactions occur
Cu2+(aq)+ 2e- $\to$ Cu(s)and Ag+(aq)+ e- $\to$ Ag(s)
For every 1.00 g of copper produced in the first process,how many grams of silver will be produced in the second one?

Accepted Answer

A) 0.294 g 
B) 0.588 g 
C) 0.850 g 
D) 1.70 g 
E) 3.40 g 
A) 0.294 g 
B) 0.588 g 
C) 0.850 g 
D) 1.70 g 
E) 3.40 g

Question 8

Examine the following half-reactions and select the strongest oxidizing agent among the substances.
[PtCl4]2-(aq)+ 2e-  
Pt(s)+ 4Cl-(aq);E° = 0.755 V
RuO4(s)+ 8H+(aq)+ 8e-  
Ru(s)+ 4H2O(l);E° = 1.038 V
FeO42-(aq)+ 8H+(aq)+ 3e-  
Fe3+(aq)+ 4H2O(l);E° = 2.07 V
H4XeO6(aq)+ 2H+(aq)+ 2e-  
XeO3(aq)+ 3H2O(l);E° = 2.42 V

Accepted Answer

A) [PtCl4]2-(aq) 
B) RuO4(s) 
C) HFeO4- (aq) 
D) H4XeO6(aq) 
E) Cl-(aq) 
A) [PtCl4]2-(aq) 
B) RuO4(s) 
C) HFeO4- (aq) 
D) H4XeO6(aq) 
E) Cl-(aq)

Question 9

Cryolite,Na3AlF6 is used in the electrolysis of aluminum oxide because

Accepted Answer

A) it is a good source of fluoride ions. 
B) it provides a source of fluorine,an oxidizing agent. 
C) it provides a source of sodium,a reducing agent. 
D) it reduces the energy requirement of the process,by lowering the melting point. 
E) it is very soluble in water. 
A) it is a good source of fluoride ions. 
B) it provides a source of fluorine,an oxidizing agent. 
C) it provides a source of sodium,a reducing agent. 
D) it reduces the energy requirement of the process,by lowering the melting point. 
E) it is very soluble in water.

Question 10

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) $\to$ Cu(s)+ Co2+(aq)

Accepted Answer

A) -0.28 V 
B) -0.96V 
C) 0.28 V 
D) 0.96 V 
E) None of these choices is correct. 
A) -0.28 V 
B) -0.96V 
C) 0.28 V 
D) 0.96 V 
E) None of these choices is correct.

Question 11

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

Accepted Answer

A) True 
 B)False

Question 12

Consider the following balanced redox reaction
3CuO(s)+ 2NH3(aq) $\to$N2(g)+ 3H2O(l)+ 3Cu(s)
Which of the following statements is true?

Accepted Answer

A) CuO(s)is the oxidizing agent and copper is reduced. 
B) CuO(s)is the oxidizing agent and copper is oxidized. 
C) CuO(s)is the reducing agent and copper is oxidized. 
D) CuO(s)is the reducing agent and copper is reduced. 
E) CuO(s)is the oxidizing agent and N2(g)is the reducing agent. 
A) CuO(s)is the oxidizing agent and copper is reduced. 
B) CuO(s)is the oxidizing agent and copper is oxidized. 
C) CuO(s)is the reducing agent and copper is oxidized. 
D) CuO(s)is the reducing agent and copper is reduced. 
E) CuO(s)is the oxidizing agent and N2(g)is the reducing agent.

Question 13

A voltaic cell consists of a Cd/Cd2+ electrode (E° = -0.40 V)and a Fe/Fe2+ electrode (E°= -0.44 V).If Ecell = 0 and the temperature is 25°C,what is the ratio [Fe2+]/[Cd2+]?

Accepted Answer

A) 2 $\times$ 101 
B) 1 $\times$ 101 
C) 1 
D) 1 $\times$ 10-1 
E) 5 $\times$ 10-2 
A) 2 $\times$ 101 
B) 1 $\times$ 101 
C) 1 
D) 1 $\times$ 10-1 
E) 5 $\times$ 10-2

Question 14

A voltaic cell prepared using zinc and iodine has the following cell notation.
Zn(s)| Zn2+(aq)|| I-(aq)| I2(s)| C (graphite)
Which of the following equations correctly represents the balanced,spontaneous,cell reaction?

Accepted Answer

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

Question 15

Consider the non-aqueous cell reaction
2Na(l)+ FeCl2(s)  
2NaCl(s)+ Fe(s)
For which E°cell = 2.35 V at 200°C.$\Delta$G° at this temperature is

Accepted Answer

A) 453 kJ 
B) -453 kJ 
C) 907 kJ 
D) -907 kJ 
E) None of these choices is correct. 
A) 453 kJ 
B) -453 kJ 
C) 907 kJ 
D) -907 kJ 
E) None of these choices is correct.

Question 16

Calculate $\Delta$G° for the oxidation of 3 moles of copper by nitric acid.
Cu2+(aq)+ 2e-  
Cu(s);E° = 0.34 V
NO3-(aq)+ 4H+(aq)+ 3e-  
NO(g)+ 2H2O(l);E° = 0.957 V

Accepted Answer

A) -120 kJ 
B) -180 kJ 
C) -240 kJ 
D) -300 kJ 
E) -360 kJ 
A) -120 kJ 
B) -180 kJ 
C) -240 kJ 
D) -300 kJ 
E) -360 kJ

Question 17

What mass of copper will be deposited when 18.2 A are passed through a CuSO4 solution for 45.0 minutes?

Accepted Answer

A) 16.2 g 
B) 33.4 g 
C) 40.6 g 
D) 81.3 g 
E) 163 g 
A) 16.2 g 
B) 33.4 g 
C) 40.6 g 
D) 81.3 g 
E) 163 g

Question 18

A voltaic cell consists of an Au/Au3+ electrode (E° = 1.50 V)and a Cu/Cu2+ electrode (E° = 0.34 V).Calculate [Au3+] if [Cu2+] = 1.20 M and Ecell = 1.13 V at 25°C.

Accepted Answer

A) 0.001 M 
B) 0.002 M 
C) 0.01 M 
D) 0.02 M 
E) 0.04 M 
A) 0.001 M 
B) 0.002 M 
C) 0.01 M 
D) 0.02 M 
E) 0.04 M

Question 19

Manganese dioxide (MnO2)for use in dry cells is made by electrolyzing solutions of Mn2+,where the following reaction occurs at the anode:
Mn2+(aq)+ 2H2O(l) $\to$ MnO2(s)+ 4H+(aq)+ 2e-
 Using a current of 100.amperes (A),how many hours will it take to produce 5.00 kg of MnO2,according to the above reaction?

Accepted Answer

The answer of Manganese dioxide (MnO2)for use in dry cells...

Question 20

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.

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

In the shorthand notation for cells,a double vertical line is used to separate the reduced and oxidized forms of a redox couple.

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

Which one of the following pairs of substances could be used to construct a single redox electrode (i.e. ,they have an element in common,but in different oxidation states)?

A cell can be prepared from copper and tin.What is the E°_cell for the cell that forms from the following half-reactions? Cu²⁺(aq)+ 2e^- Cu(s);E° = 0.34 V Sn⁴⁺(aq)+ 2e^- Sn²⁺(aq);E° = 0.13 V

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

Cryolite,Na₃AlF₆ is used in the electrolysis of aluminum oxide because

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) $\to$ Cu(s)+ Co²⁺(aq)

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

Consider the following balanced redox reaction 3CuO(s)+ 2NH₃(aq) $\to$ N₂(g)+ 3H₂O(l)+ 3Cu(s) Which of the following statements is true?

A voltaic cell consists of a Cd/Cd²⁺ electrode (E° = -0.40 V)and a Fe/Fe²⁺ electrode (E°= -0.44 V).If E_cell = 0 and the temperature is 25°C,what is the ratio [Fe²⁺]/[Cd²⁺]?

A voltaic cell prepared using zinc and iodine has the following cell notation. Zn(s)| Zn²⁺(aq)|| I^-(aq)| I₂(s)| C (graphite) Which of the following equations correctly represents the balanced,spontaneous,cell reaction?

What mass of copper will be deposited when 18.2 A are passed through a CuSO₄ solution for 45.0 minutes?

A voltaic cell consists of an Au/Au³⁺ electrode (E° = 1.50 V)and a Cu/Cu²⁺ electrode (E° = 0.34 V).Calculate [Au³⁺] if [Cu²⁺] = 1.20 M and E_cell = 1.13 V at 25°C.

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

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 Solutions

The Main-Group Elements: Applying Principles of Bonding and Structure

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 Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

Exam 21: Electrochemistry: Chemical Change and Electrical Work

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

In the shorthand notation for cells,a double vertical line is used to separate the reduced and oxidized forms of a redox couple.

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

Which one of the following pairs of substances could be used to construct a single redox electrode (i.e. ,they have an element in common,but in different oxidation states)?

A cell can be prepared from copper and tin.What is the E°cell for the cell that forms from the following half-reactions? Cu2+(aq)+ 2e- Cu(s);E° = 0.34 V Sn4+(aq)+ 2e- Sn2+(aq);E° = 0.13 V

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

Cryolite,Na3AlF6 is used in the electrolysis of aluminum oxide because

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) →\to→ Cu(s)+ Co2+(aq)

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

Consider the following balanced redox reaction 3CuO(s)+ 2NH3(aq) →\to→ N2(g)+ 3H2O(l)+ 3Cu(s) Which of the following statements is true?

A voltaic cell consists of a Cd/Cd2+ electrode (E° = -0.40 V)and a Fe/Fe2+ electrode (E°= -0.44 V).If Ecell = 0 and the temperature is 25°C,what is the ratio [Fe2+]/[Cd2+]?

A voltaic cell prepared using zinc and iodine has the following cell notation. Zn(s)| Zn2+(aq)|| I-(aq)| I2(s)| C (graphite) Which of the following equations correctly represents the balanced,spontaneous,cell reaction?

Consider the non-aqueous cell reaction 2Na(l)+ FeCl2(s) 2NaCl(s)+ Fe(s) For which E°cell = 2.35 V at 200°C. Δ\DeltaΔ G° at this temperature is

Calculate Δ\DeltaΔ G° for the oxidation of 3 moles of copper by nitric acid. Cu2+(aq)+ 2e- Cu(s);E° = 0.34 V NO3-(aq)+ 4H+(aq)+ 3e- NO(g)+ 2H2O(l);E° = 0.957 V

What mass of copper will be deposited when 18.2 A are passed through a CuSO4 solution for 45.0 minutes?

A voltaic cell consists of an Au/Au3+ electrode (E° = 1.50 V)and a Cu/Cu2+ electrode (E° = 0.34 V).Calculate [Au3+] if [Cu2+] = 1.20 M and Ecell = 1.13 V at 25°C.

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

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 Solutions

The Main-Group Elements: Applying Principles of Bonding and Structure

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 Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

Filters

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

A cell can be prepared from copper and tin.What is the E°_cell for the cell that forms from the following half-reactions? Cu²⁺(aq)+ 2e^- Cu(s);E° = 0.34 V Sn⁴⁺(aq)+ 2e^- Sn²⁺(aq);E° = 0.13 V

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

Cryolite,Na₃AlF₆ is used in the electrolysis of aluminum oxide because

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) $\to$ Cu(s)+ Co²⁺(aq)

Consider the following balanced redox reaction 3CuO(s)+ 2NH₃(aq) $\to$ N₂(g)+ 3H₂O(l)+ 3Cu(s) Which of the following statements is true?

A voltaic cell consists of a Cd/Cd²⁺ electrode (E° = -0.40 V)and a Fe/Fe²⁺ electrode (E°= -0.44 V).If E_cell = 0 and the temperature is 25°C,what is the ratio [Fe²⁺]/[Cd²⁺]?

A voltaic cell prepared using zinc and iodine has the following cell notation. Zn(s)| Zn²⁺(aq)|| I^-(aq)| I₂(s)| C (graphite) Which of the following equations correctly represents the balanced,spontaneous,cell reaction?

What mass of copper will be deposited when 18.2 A are passed through a CuSO₄ solution for 45.0 minutes?

A voltaic cell consists of an Au/Au³⁺ electrode (E° = 1.50 V)and a Cu/Cu²⁺ electrode (E° = 0.34 V).Calculate [Au³⁺] if [Cu²⁺] = 1.20 M and E_cell = 1.13 V at 25°C.