The value of E°cell for the reaction 2Cr3+(aq) + 6Hg(l) → 2Cr(s) + 3Hg22+(aq) Is 1.59 V. Calculate ΔG° for the reaction.

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

Consider the nonaqueous cell reaction 2Na(l) + FeCl2(s) ⇄ 2NaCl(s) + Fe(s) For which E°cell = 2.35 V at 200°C. ΔG° at this temperature is

A) 453 kJ. B) −453 kJ. C) 907 kJ. D) −907 kJ. E) None of these choices are correct. A) 453 kJ. B) −453 kJ. C) 907 kJ. D) −907 kJ. E) None of these choices are correct.

Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. O2(g) + 4H+(aq) + 4e− ⇄ 2H2O(l) E° = 1.229 V Al3+(aq) + 3e− ⇄ Al(s) E° = −1.662 V Overall reaction: 4Al(s) + 3O2(g) + 12H+(aq) → 4Al3+(aq) + 6H2O(l)

A) E° cell = −2.891 V, nonspontaneous B) E° cell = −2.891 V, spontaneous C) E° cell = 2.891 V, nonspontaneous D) E° cell = 2.891 V, spontaneous E) None of these choices are correct. A) E° cell = −2.891 V, nonspontaneous B) E° cell = −2.891 V, spontaneous C) E° cell = 2.891 V, nonspontaneous D) E° cell = 2.891 V, spontaneous E) None of these choices are correct.

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

A) Co is the reducing agent. B) Co 2+ ions are oxidized. C) Al is the reducing agent. D) Al 3+ is the reducing agent. E) aluminum metal is the cathode. A) Co is the reducing agent. B) Co 2+ ions are oxidized. C) Al is the reducing agent. D) Al 3+ is the reducing agent. E) aluminum metal is the cathode.

Examine the following half-reactions and select the weakest reducing agent among the substances. Cr(OH)3(s) + 3e− ⇄ Cr(s) + 3OH−(aq) E° = −1.48 V SnO2(s) + 2H2O(l) + 4e− ⇄ Sn(s) + 4OH−(aq) E° = −0.945 V MnO2(s) + 4H+(aq) + 2e− ⇄ Mn2+(aq) + 2H2O(l) E° = 1.224 V Hg2SO4(s) + 2e− ⇄ 2Hg(l) + SO42−(aq) E° = 0.613 V

A) Cr( s) B) Sn( s) C) Mn 2+( aq) D) Hg( l) E) OH −( aq) A) Cr( s) B) Sn( s) C) Mn 2+( aq) D) Hg( l) E) OH −( aq)

A current of 250. A flows for 24.0 hours at an anode where the reaction occurring is Mn2+(aq) + 2H2O(l) → MnO2(s) + 4H+(aq) + 2e− What mass of MnO2 is deposited at this anode?

A) 19.5 kg B) 12.9 kg C) 4.87 kg D) 2.43 kg E) None of these choices are correct. A) 19.5 kg B) 12.9 kg C) 4.87 kg D) 2.43 kg E) None of these choices are correct.

Examine the following half-reactions and select the strongest reducing agent among the species listed. PbI2(s) + 2e− ⇄ Pb(s) + 2I−(aq) E° = −0.365 V Ca2+(aq) + 2e− ⇄ Ca(s) E° = −2.868 V Pt2+(aq) + 2e− ⇄ Pt(s) E° = 1.18 V Br2(l) + 2e− ⇄ 2Br−(aq) E° = 1.066 V

A) Pb( s) B) Ca( s) C) Pt( s) D) Br −( aq) E) Pt 2+( aq) A) Pb( s) B) Ca( s) C) Pt( s) D) Br −( aq) E) Pt 2+( aq)

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 ΔG° for the reaction at 25°C.

A) −15.1 kJ B) −34.7 kJ C) 15.1 kJ D) 34.7 kJ E) None of these choices are correct. A) −15.1 kJ B) −34.7 kJ C) 15.1 kJ D) 34.7 kJ E) None of these choices are correct.

Two cells are connected in series, so that the same current flows through two electrodes where the following half-reactions occur Cu2+(aq) + 2e− → Cu(s) and Ag+(aq) + e− → 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?

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

Exam 21: Electrochemistry: Chemical Change and Electrical Work

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

(Multiple Choice)

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Question 81

The value of E°_cell for the reaction 2Cr³⁺(aq) + 6Hg(l) → 2Cr(s) + 3Hg₂²⁺(aq) Is 1.59 V. Calculate ΔG° for the reaction.

(Multiple Choice)

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Question 82

Consider the nonaqueous cell reaction 2Na(l) + FeCl₂(s) ⇄ 2NaCl(s) + Fe(s) For which E°_cell = 2.35 V at 200°C. ΔG° at this temperature is

(Multiple Choice)

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Question 83

Calculate E°_cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. O₂(g) + 4H⁺(aq) + 4e⁻⇄ 2H₂O(l) E° = 1.229 V Al³⁺(aq) + 3e⁻ ⇄ Al(s) E° = −1.662 V Overall reaction: 4Al(s) + 3O₂(g) + 12H⁺(aq) → 4Al³⁺(aq) + 6H₂O(l)

(Multiple Choice)

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Question 84

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

(True/False)

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Question 85

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

(Multiple Choice)

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Question 86

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for Sn(OH)₃⁻will be Bi(OH)₃(s) + Sn(OH)₃(aq) → Sn(OH)₆²⁻(aq) + Bi(s) (basic solution)

(Multiple Choice)

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Question 87

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) → Cu(s) + Co²⁺(aq)

(Multiple Choice)

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Question 88

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

(Multiple Choice)

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Question 89

Electrons are produced at the cathode of a voltaic cell.

(True/False)

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Question 90

Examine the following half-reactions and select the weakest reducing agent among the substances. Cr(OH)₃(s) + 3e⁻ ⇄ Cr(s) + 3OH⁻(aq) E° = −1.48 V SnO₂(s) + 2H₂O(l) + 4e⁻ ⇄ Sn(s) + 4OH⁻(aq) E° = −0.945 V MnO₂(s) + 4H⁺(aq) + 2e⁻ ⇄ Mn²⁺(aq) + 2H₂O(l) E° = 1.224 V Hg₂SO₄(s) + 2e⁻ ⇄ 2Hg(l) + SO₄²⁻(aq) E° = 0.613 V

(Multiple Choice)

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Question 91

A battery is considered "dead" when

(Multiple Choice)

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Question 92

In a fuel cell, an external source of electrical power is used to drive a nonspontaneous reaction in which a fuel is produced.

(True/False)

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Question 93

A current of 250. A flows for 24.0 hours at an anode where the reaction occurring is Mn²⁺(aq) + 2H₂O(l) → MnO₂(s) + 4H⁺(aq) + 2e⁻ What mass of MnO₂ is deposited at this anode?

(Multiple Choice)

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Question 94

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

(Multiple Choice)

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Question 95

Which of the following types of electrochemical cell is most likely to find use in the future as a power source for electric vehicles?

(Multiple Choice)

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Question 96

Examine the following half-reactions and select the strongest reducing agent among the species listed. PbI₂(s) + 2e⁻ ⇄ Pb(s) + 2I⁻(aq) E° = −0.365 V Ca²⁺(aq) + 2e⁻ ⇄ Ca(s) E° = −2.868 V Pt²⁺(aq) + 2e⁻ ⇄ Pt(s) E° = 1.18 V Br₂(l) + 2e⁻ ⇄ 2Br⁻(aq) E° = 1.066 V

(Multiple Choice)

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Question 97

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 ΔG° for the reaction at 25°C.

(Multiple Choice)

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Question 98

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

(True/False)

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Question 99

Two cells are connected in series, so that the same current flows through two electrodes where the following half-reactions occur Cu²⁺(aq) + 2e⁻ → Cu(s) and Ag⁺(aq) + e⁻ → 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?

(Multiple Choice)

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Question 100

Showing 81 - 100 of 101

Exam 21: Electrochemistry: Chemical Change and Electrical Work

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

The value of E°cell for the reaction 2Cr3+(aq) + 6Hg(l) → 2Cr(s) + 3Hg22+(aq) Is 1.59 V. Calculate ΔG° for the reaction.

Consider the nonaqueous cell reaction 2Na(l) + FeCl2(s) ⇄ 2NaCl(s) + Fe(s) For which E°cell = 2.35 V at 200°C. ΔG° at this temperature is

Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. O2(g) + 4H+(aq) + 4e− ⇄ 2H2O(l) E° = 1.229 V Al3+(aq) + 3e− ⇄ Al(s) E° = −1.662 V Overall reaction: 4Al(s) + 3O2(g) + 12H+(aq) → 4Al3+(aq) + 6H2O(l)

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

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

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for Sn(OH)3− will be Bi(OH)3(s) + Sn(OH)3(aq) → Sn(OH)62−(aq) + Bi(s) (basic solution)

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) → Cu(s) + Co2+(aq)

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

Electrons are produced at the cathode of a voltaic cell.

A battery is considered "dead" when

In a fuel cell, an external source of electrical power is used to drive a nonspontaneous reaction in which a fuel is produced.

A current of 250. A flows for 24.0 hours at an anode where the reaction occurring is Mn2+(aq) + 2H2O(l) → MnO2(s) + 4H+(aq) + 2e− What mass of MnO2 is deposited at this anode?

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

Which of the following types of electrochemical cell is most likely to find use in the future as a power source for electric vehicles?

Examine the following half-reactions and select the strongest reducing agent among the species listed. PbI2(s) + 2e− ⇄ Pb(s) + 2I−(aq) E° = −0.365 V Ca2+(aq) + 2e− ⇄ Ca(s) E° = −2.868 V Pt2+(aq) + 2e− ⇄ Pt(s) E° = 1.18 V Br2(l) + 2e− ⇄ 2Br−(aq) E° = 1.066 V

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 ΔG° for the reaction at 25°C.

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

Keys to the Study of Chemistry: Definitions, Units, and Problem Solving

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 Reaction Direction

The Elements in Nature and Industry

Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

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

The value of E°_cell for the reaction 2Cr³⁺(aq) + 6Hg(l) → 2Cr(s) + 3Hg₂²⁺(aq) Is 1.59 V. Calculate ΔG° for the reaction.

Consider the nonaqueous cell reaction 2Na(l) + FeCl₂(s) ⇄ 2NaCl(s) + Fe(s) For which E°_cell = 2.35 V at 200°C. ΔG° at this temperature is

Calculate E°_cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. O₂(g) + 4H⁺(aq) + 4e⁻⇄ 2H₂O(l) E° = 1.229 V Al³⁺(aq) + 3e⁻ ⇄ Al(s) E° = −1.662 V Overall reaction: 4Al(s) + 3O₂(g) + 12H⁺(aq) → 4Al³⁺(aq) + 6H₂O(l)

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

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for Sn(OH)₃⁻will be Bi(OH)₃(s) + Sn(OH)₃(aq) → Sn(OH)₆²⁻(aq) + Bi(s) (basic solution)

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) → Cu(s) + Co²⁺(aq)

A current of 250. A flows for 24.0 hours at an anode where the reaction occurring is Mn²⁺(aq) + 2H₂O(l) → MnO₂(s) + 4H⁺(aq) + 2e⁻ What mass of MnO₂ is deposited at this anode?

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

Examine the following half-reactions and select the strongest reducing agent among the species listed. PbI₂(s) + 2e⁻ ⇄ Pb(s) + 2I⁻(aq) E° = −0.365 V Ca²⁺(aq) + 2e⁻ ⇄ Ca(s) E° = −2.868 V Pt²⁺(aq) + 2e⁻ ⇄ Pt(s) E° = 1.18 V Br₂(l) + 2e⁻ ⇄ 2Br⁻(aq) E° = 1.066 V

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 ΔG° for the reaction at 25°C.