A concentration cell consists of two Zn/Zn2+ electrodes. The electrolyte in compartment A is 0.10 M Zn(NO3)2 and in compartment B is 0.60 M Zn(NO3)2. What is the voltage of the cell at 25$\degree$C?

A) 0.010 V B) 0.020 V C) 0.023 V D) 0.046 V E) None of these choices is correct. A) 0.010 V B) 0.020 V C) 0.023 V D) 0.046 V E) None of these choices is correct.

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

A) 2 *101 B) 1 *101 C) 1 D) 1 *10¯1 E) 5 *10¯2 A) 2 *101 B) 1 *101 C) 1 D) 1 *10¯1 E) 5 *10¯2

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.

Calculate the potential of a voltaic cell (E$\degree$cell) if it is required to do 5.43 * 10¯3 kJ of work when a charge of 2.50 C is transferred.

A) 2.17* 103 V B) 2.17 * 10¯3 V C) 2.17 V D) 13.6 V E) 1.36 * 10¯2 V A) 2.17* 103 V B) 2.17 * 10¯3 V C) 2.17 V D) 13.6 V E) 1.36 * 10¯2 V

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?

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

A voltaic cell consists of a Ag/Ag+ electrode (E$\degree$= 0.80 V) and a Fe2+/Fe3+ electrode (E$\degree$ = 0.77 V) with the following initial molar concentrations: [Fe2+] = 0.30 M; [Fe3+] = 0.10 M; [Ag+] = 0.30 M. What is the equilibrium concentration of Fe3+? (Assume the anode and cathode solutions are of equal volume, and a temperature of 25$\degree$C.)

A) 0.030 M B) 0.043 M C) 0.085 M D) 0.11 M E) 0.17 M A) 0.030 M B) 0.043 M C) 0.085 M D) 0.11 M E) 0.17 M

Exam 21: Electrochemistry: Chemical Change and Electrical Work

What is the E $\degree$ _cell for the cell represented by the combination of the following half-reactions? $What is the E \degree cell for the cell represented by the combination of the following half-reactions?$

(Multiple Choice)

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Question 61

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

(Multiple Choice)

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Question 62

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

(True/False)

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Question 63

A concentration cell consists of two Zn/Zn²⁺ electrodes. The electrolyte in compartment A is 0.10 M Zn(NO₃)₂ and in compartment B is 0.60 M Zn(NO₃)₂. What is the voltage of the cell at 25 $\degree$ C?

(Multiple Choice)

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Question 64

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

(Multiple Choice)

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Question 65

A much-studied cell in electrochemistry has the following cell notation: 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 66

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

(True/False)

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Question 67

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

(Multiple Choice)

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Question 68

Calculate the potential of a voltaic cell (E $\degree$ _cell) if it is required to do 5.43 * 10¯³ kJ of work when a charge of 2.50 C is transferred.

(Multiple Choice)

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Question 69

Electrons are produced at the cathode of a voltaic cell.

(True/False)

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Question 70

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

(Multiple Choice)

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Question 71

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

(Essay)

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Question 72

In the shorthand notation for cells, a single vertical line represents a salt bridge.

(True/False)

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Question 73

If the electrodes of a voltaic cell are connected with an external wire, electrons will flow in this wire from the cathode to the anode.

(True/False)

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Question 74

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

(Essay)

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Question 75

Electrolytic cells utilize electrical energy to drive non-spontaneous redox reactions.

(True/False)

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Question 76

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?

(Multiple Choice)

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Question 77

A voltaic cell consists of a Ag/Ag⁺ electrode (E $\degree$ = 0.80 V) and a Fe²⁺/Fe³⁺ electrode (E $\degree$ = 0.77 V) with the following initial molar concentrations: [Fe²⁺] = 0.30 M; [Fe³⁺] = 0.10 M; [Ag⁺] = 0.30 M. What is the equilibrium concentration of Fe³⁺? (Assume the anode and cathode solutions are of equal volume, and a temperature of 25 $\degree$ C.)

(Multiple Choice)

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Question 78

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

(Multiple Choice)

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Question 79

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

(Multiple Choice)

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Question 80

Showing 61 - 80 of 102

Exam 21: Electrochemistry: Chemical Change and Electrical Work

What is the E °\degree° cell for the cell represented by the combination of the following half-reactions?

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

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

A concentration cell consists of two Zn/Zn2+ electrodes. The electrolyte in compartment A is 0.10 M Zn(NO3)2 and in compartment B is 0.60 M Zn(NO3)2. What is the voltage of the cell at 25 °\degree° C?

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

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

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

Calculate the potential of a voltaic cell (E °\degree° cell) if it is required to do 5.43 * 10¯3 kJ of work when a charge of 2.50 C is transferred.

Electrons are produced at the cathode of a voltaic cell.

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

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

In the shorthand notation for cells, a single vertical line represents a salt bridge.

If the electrodes of a voltaic cell are connected with an external wire, electrons will flow in this wire from the cathode to the anode.

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

Electrolytic cells utilize electrical energy to drive non-spontaneous redox reactions.

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?

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

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

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

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What is the E $\degree$ _cell for the cell represented by the combination of the following half-reactions? $What is the E \degree <sub>cell</sub> for the cell represented by the combination of the following half-reactions?$

A concentration cell consists of two Zn/Zn²⁺ electrodes. The electrolyte in compartment A is 0.10 M Zn(NO₃)₂ and in compartment B is 0.60 M Zn(NO₃)₂. What is the voltage of the cell at 25 $\degree$ C?

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

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

Calculate the potential of a voltaic cell (E $\degree$ _cell) if it is required to do 5.43 * 10¯³ kJ of work when a charge of 2.50 C is transferred.

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?

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