A solution is prepared by dissolving 32.0 g of NiSO4 in water. What current would be needed to deposit all of the nickel in 5.0 hours?

A) 1.1 A B) 2.2 A C) 3.3 A D) 4.4 A E) 5.5 A A) 1.1 A B) 2.2 A C) 3.3 A D) 4.4 A E) 5.5 A

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

A) 0.040 M B) 0.24 M C) 1.1 M D) 1.8 M E) none of the above A) 0.040 M B) 0.24 M C) 1.1 M D) 1.8 M E) none of the above

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 reactions occurs at the anode?

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

The line notation, Pt | H2(g) | H+(aq) || Cu2+(aq) | Cu(s), indicates that

A) copper metal is a product of the cell reaction. B) hydrogen gas (H2) is a product of the cell reaction. C) Cu is the anode. D) Pt is the cathode. E) Cu2+ is the reducing agent. A) copper metal is a product of the cell reaction. B) hydrogen gas (H2) is a product of the cell reaction. C) Cu is the anode. D) Pt is the cathode. E) Cu2+ is the reducing agent.

Exam 21: Electrochemistry: Chemical Change and Electrical Work

A concentration cell is based on the aqueous reaction Cu²⁺(1.00 M)  Cu²⁺(0.0100 M) Calculate the potential of this cell if it operates at 25.0°C.

(Short Answer)

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Question 21

In the electrolyte of an electrochemical cell, current is carried by anions moving toward the anode and cations moving in the opposite direction.

(True/False)

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Question 22

Which, if any, of the following metals would not be capable of acting as a sacrificial anode when used with iron E°_Fe = -0.44 V; all E° values refer to the M²⁺/M half-cell reactions.

(Multiple Choice)

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Question 23

A solution is prepared by dissolving 32.0 g of NiSO₄ in water. What current would be needed to deposit all of the nickel in 5.0 hours?

(Multiple Choice)

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Question 24

A battery is considered "dead" when

(Multiple Choice)

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Question 25

Which, if any, of the following metals would be capable of acting as a sacrificial anode when used with iron pipe? E°_Fe = -0.44 V; all E° values refer to the M²⁺/M half-cell reactions.

(Multiple Choice)

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Question 26

A voltaic cell has a standard cell potential equal to 0.74 V. If the standard electrode (reduction) potential for the anode is - 0.22 V, what is the standard electrode potential for the cathode?

(Multiple Choice)

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Question 27

A buried iron pipe can be protected against corrosion by connecting it to a rod of copper.

(True/False)

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Question 28

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

(Multiple Choice)

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Question 29

Consider the following redox equation Mn(OH)₂(s) + MnO₄^-(aq)  MnO₄^2-(aq) (basic solution) When the equation is balanced with smallest whole number coefficients, what is the coefficient for OH^-(aq) and on which side of the equation is OH^-(aq) present?

(Multiple Choice)

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Question 30

In one or two short sentences each, explain what is meant by the following terms. a. galvanic or voltaic cell b. electrolytic cell c. salt bridge d. secondary battery or cell e. primary battery or cell f. glass electrode

(Essay)

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Question 31

In the electrolysis of aqueous sodium sulfate at electrodes of platinum, predict the products of the cell reaction.

(Multiple Choice)

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Question 32

In the absence of oxygen, iron will rust as long as moisture is present.

(True/False)

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Question 33

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 reactions occurs at the anode?

(Multiple Choice)

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Question 34

A much-studied cell in electrochemistry has the following cell notation: Ag(s)  AgCl(s)  HCl(aq)  H₂(g)  Pt(s) Bearing in mind that HCl(aq) consists of H⁺(aq) and Cl^-(aq), and that this solution is in contact with both electrodes (there is no salt bridge), write down balanced equations for a. the anode half-reaction. b. the cathode half-reaction. c. the cell reaction.

(Essay)

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Question 35

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

(True/False)

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Question 36

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

(Multiple Choice)

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Question 37

The line notation, Pt | H₂(g) | H⁺(aq) || Cu²⁺(aq) | Cu(s), indicates that

(Multiple Choice)

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Question 38

A secondary cell (battery) can operate either as a galvanic or an electrolytic cell.

(True/False)

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Question 39

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?

(Multiple Choice)

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Question 40

Showing 21 - 40 of 102

Exam 21: Electrochemistry: Chemical Change and Electrical Work

A concentration cell is based on the aqueous reaction Cu2+(1.00 M)  Cu2+(0.0100 M) Calculate the potential of this cell if it operates at 25.0°C.

In the electrolyte of an electrochemical cell, current is carried by anions moving toward the anode and cations moving in the opposite direction.

Which, if any, of the following metals would not be capable of acting as a sacrificial anode when used with iron E°Fe = -0.44 V; all E° values refer to the M2+/M half-cell reactions.

A solution is prepared by dissolving 32.0 g of NiSO4 in water. What current would be needed to deposit all of the nickel in 5.0 hours?

A battery is considered "dead" when

Which, if any, of the following metals would be capable of acting as a sacrificial anode when used with iron pipe? E°Fe = -0.44 V; all E° values refer to the M2+/M half-cell reactions.

A voltaic cell has a standard cell potential equal to 0.74 V. If the standard electrode (reduction) potential for the anode is - 0.22 V, what is the standard electrode potential for the cathode?

A buried iron pipe can be protected against corrosion by connecting it to a rod of copper.

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

Consider the following redox equation Mn(OH)2(s) + MnO4-(aq)  MnO42-(aq) (basic solution) When the equation is balanced with smallest whole number coefficients, what is the coefficient for OH-(aq) and on which side of the equation is OH-(aq) present?

In one or two short sentences each, explain what is meant by the following terms. a. galvanic or voltaic cell b. electrolytic cell c. salt bridge d. secondary battery or cell e. primary battery or cell f. glass electrode

In the electrolysis of aqueous sodium sulfate at electrodes of platinum, predict the products of the cell reaction.

In the absence of oxygen, iron will rust as long as moisture is present.

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 reactions occurs at the anode?

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

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

The line notation, Pt | H2(g) | H+(aq) || Cu2+(aq) | Cu(s), indicates that

A secondary cell (battery) can operate either as a galvanic or an electrolytic cell.

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

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A concentration cell is based on the aqueous reaction Cu²⁺(1.00 M)  Cu²⁺(0.0100 M) Calculate the potential of this cell if it operates at 25.0°C.

Which, if any, of the following metals would not be capable of acting as a sacrificial anode when used with iron E°_Fe = -0.44 V; all E° values refer to the M²⁺/M half-cell reactions.

A solution is prepared by dissolving 32.0 g of NiSO₄ in water. What current would be needed to deposit all of the nickel in 5.0 hours?

Which, if any, of the following metals would be capable of acting as a sacrificial anode when used with iron pipe? E°_Fe = -0.44 V; all E° values refer to the M²⁺/M half-cell reactions.

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

Consider the following redox equation Mn(OH)₂(s) + MnO₄^-(aq)  MnO₄^2-(aq) (basic solution) When the equation is balanced with smallest whole number coefficients, what is the coefficient for OH^-(aq) and on which side of the equation is OH^-(aq) present?

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 reactions occurs at the anode?

The line notation, Pt | H₂(g) | H⁺(aq) || Cu²⁺(aq) | Cu(s), indicates that