The line notation, Al(s) | Al3+(aq) || Co2+(aq) | Co(s), indicates that

A) Co is the reducing agent. B) Co2+ ions are oxidized. C) Al is the reducing agent. D) Al3+ is the reducing agent. E) aluminum metal is the cathode. A) Co is the reducing agent. B) Co2+ ions are oxidized. C) Al is the reducing agent. D) Al3+ is the reducing agent. E) aluminum metal is the cathode. C

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

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

Consider the reaction in the lead-acid cell for which E $\degree$cell = 2.04 V at 298 K. $\Delta$G $\degree$for this reaction is

A) -3.94 * 105 kJ. B) -3.94 * 102 kJ. C) -1.97*105 kJ. D) -7.87* 102 kJ. E) None of these choices is correct. A) -3.94 * 105 kJ. B) -3.94 * 102 kJ. C) -1.97*105 kJ. D) -7.87* 102 kJ. E) None of these choices is correct.

Exam 21: Electrochemistry: Chemical Change and Electrical Work

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

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(Multiple Choice)

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Question 1

Correct Answer:

Verified

The line notation, Al(s) | Al³⁺(aq) || Co²⁺(aq) | Co(s), indicates that

Free

(Multiple Choice)

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Question 2

Correct Answer:

Verified

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

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(True/False)

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Question 3

Correct Answer:

Verified

False

Examine the following half-reactions and select the strongest reducing agent among the species listed.

(Multiple Choice)

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Question 4

The following half-reactions occur in the mercury battery used in calculators. If E $\degree$ 1U1B1cell = 1.357 V, calculate the equilibrium constant for the cell reaction at 25 $\degree$ C. (Assume the stoichiometric coefficients in the cell reaction are all equal to 1.) HgO(s) + H₂O(l) + 2e¯ $The following half-reactions occur in the mercury battery used in calculators. If E \degree 1U1B1cell = 1.357 V, calculate the equilibrium constant for the cell reaction at 25 \degree C. (Assume the stoichiometric coefficients in the cell reaction are all equal to 1.) HgO(s) + H2O(l) + 2e¯ Hg(l) + 2OH¯(aq) ZnO(s) + H2O(l) + 2e¯ Zn(s) + 2OH¯(aq)$ Hg(l) + 2OH¯(aq) ZnO(s) + H₂O(l) + 2e¯ $The following half-reactions occur in the mercury battery used in calculators. If E \degree 1U1B1cell = 1.357 V, calculate the equilibrium constant for the cell reaction at 25 \degree C. (Assume the stoichiometric coefficients in the cell reaction are all equal to 1.) HgO(s) + H2O(l) + 2e¯ Hg(l) + 2OH¯(aq) ZnO(s) + H2O(l) + 2e¯ Zn(s) + 2OH¯(aq)$ Zn(s) + 2OH¯(aq)

(Multiple Choice)

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Question 5

Calculate $\Delta$ G $\degree$ for the reaction of iron(II) ions with one mole of permanganate ions. $Calculate \Delta G \degree for the reaction of iron(II) ions with one mole of permanganate ions.$

(Multiple Choice)

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Question 6

What is the value of the equilibrium constant for the cell reaction below at 25 $\degree$ C? E $\degree$ _cell = 0.30 V Sn²⁺(aq) + Fe(s) $What is the value of the equilibrium constant for the cell reaction below at 25 \degree C? E \degree cell = 0.30 V Sn2+(aq) + Fe(s) Sn(s) + Fe2+(aq)$ Sn(s) + Fe²⁺(aq)

(Multiple Choice)

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Question 7

Which of the following elements could be prepared by electrolysis of the aqueous solution shown?

(Multiple Choice)

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Question 8

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

(Multiple Choice)

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Question 9

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 10

Which one of the following is not a redox reaction?

(Multiple Choice)

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Question 11

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)?

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Question 12

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

(True/False)

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Question 13

In the electrolysis of water, how many grams of oxygen gas will be produced for every gram of hydrogen gas formed? Reaction: 2H₂O(l) $\rightarrow$ 2H₂(g) + O₂(g)

(Multiple Choice)

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Question 14

Examine the following half-reactions and select the weakest oxidizing agent among the species listed.

(Multiple Choice)

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Question 15

Which one of the following statements relating to the glass electrode is correct?

(Multiple Choice)

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Question 16

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

(Multiple Choice)

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Question 17

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

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Question 18

Consider the reaction in the lead-acid cell $Consider the reaction in the lead-acid cell for which E \degree cell = 2.04 V at 298 K. \Delta G \degree for this reaction is$ for which E $\degree$ _cell = 2.04 V at 298 K. $\Delta$ G $\degree$ for this reaction is

(Multiple Choice)

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Question 19

Predict the products of the cell reaction when a molten salt mixture of sodium bromide and calcium fluoride is electrolyzed (spectator ions are not considered to be products).

(Multiple Choice)

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Question 20

Showing 1 - 20 of 102

Exam 21: Electrochemistry: Chemical Change and Electrical Work

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

The line notation, Al(s) | Al3+(aq) || Co2+(aq) | Co(s), indicates that

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

Examine the following half-reactions and select the strongest reducing agent among the species listed.

Calculate Δ\DeltaΔ G °\degree° for the reaction of iron(II) ions with one mole of permanganate ions.

What is the value of the equilibrium constant for the cell reaction below at 25 °\degree° C? E °\degree° cell = 0.30 V Sn2+(aq) + Fe(s) Sn(s) + Fe2+(aq)

Which of the following elements could be prepared by electrolysis of the aqueous solution shown?

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

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

Which one of the following is not a redox reaction?

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)?

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

In the electrolysis of water, how many grams of oxygen gas will be produced for every gram of hydrogen gas formed? Reaction: 2H2O(l) →\rightarrow→ 2H2(g) + O2(g)

Examine the following half-reactions and select the weakest oxidizing agent among the species listed.

Which one of the following statements relating to the glass electrode is correct?

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

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

Consider the reaction in the lead-acid cell for which E °\degree° cell = 2.04 V at 298 K. Δ\DeltaΔ G °\degree° for this reaction is

Predict the products of the cell reaction when a molten salt mixture of sodium bromide and calcium fluoride is electrolyzed (spectator ions are not considered to be products).

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

The line notation, Al(s) | Al³⁺(aq) || Co²⁺(aq) | Co(s), indicates that

Calculate $\Delta$ G $\degree$ for the reaction of iron(II) ions with one mole of permanganate ions. $Calculate \Delta G \degree for the reaction of iron(II) ions with one mole of permanganate ions.$

In the electrolysis of water, how many grams of oxygen gas will be produced for every gram of hydrogen gas formed? Reaction: 2H₂O(l) $\rightarrow$ 2H₂(g) + O₂(g)

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

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

Consider the reaction in the lead-acid cell $Consider the reaction in the lead-acid cell for which E \degree <sub>cell</sub> = 2.04 V at 298 K. \Delta G \degree for this reaction is$ for which E $\degree$ _cell = 2.04 V at 298 K. $\Delta$ G $\degree$ for this reaction is