Which of the following statements is true concerning the electrochemical cell Zn(s) | Zn2+(aq, 1.0 M) || Ca2+(aq, 1.0 M) | Ca(s) The standard reduction potentials are given follows: Zn2+(aq) + 2 e− → Zn(s); E° = -0.76 V Ca2+(aq) + 2 e− → Ca(s); E° = -2.87 V

A) The standard cell potential is -3.63 V. B) The standard cell potential is -2.11 V. C) The standard cell potential is -2.11 V.. D) The standard cell potential is -3.63 V.. E) The standard cell potential is 2.11 V. A) The standard cell potential is -3.63 V. B) The standard cell potential is -2.11 V. C) The standard cell potential is -2.11 V.. D) The standard cell potential is -3.63 V.. E) The standard cell potential is 2.11 V.

Calculate ΔrG° for the disproportionation reaction of copper(I) ion (Cu+) at 25 °C. 2 Cu+(aq) → Cu2+(aq) + Cu(s) The standard reduction potentials are as follows: Cu+(aq) + e- → Cu(s) E° = +0.518 V Cu2+(aq) + 2 e- → Cu(s) E° = +0.337 V

A) -165 kJ/mol⋅rxn B) -135 kJ/mol⋅rxn C) -34.9 kJ/mol⋅rxn D) +17.5 kJ/mol⋅rxn E) +135 kJ/mol⋅rxn A) -165 kJ/mol⋅rxn B) -135 kJ/mol⋅rxn C) -34.9 kJ/mol⋅rxn D) +17.5 kJ/mol⋅rxn E) +135 kJ/mol⋅rxn

The standard reduction potentials are as follows: Cr3+(aq) + 3 e- → Cr(s); E° = -0.74 V Fe2+(aq) + 2 e- → Fe(s); E° = -0.41 V Calculate the standard Gibbs free energy change for the following reaction. 2 Cr(s) + 3 Fe2+ → 3 Fe(s) + 2 Cr3+(aq)

A) 191 kJ B) 63.7 kJ C) -504 kJ D) -191 kJ E) 1060 kJ A) 191 kJ B) 63.7 kJ C) -504 kJ D) -191 kJ E) 1060 kJ

Batteries used in watches contain mercury(II) oxide. As the current flows, mercury(II) oxide is reduced to mercury according to the following reaction: HgO(s) + H2O( $\ell$ ) + 2 e- ? Hg( $\ell$ ) + 2 OH-(aq) If 2.3 × 10-5 amperes flows continuously for 1200 days, calculate the mass of mercury, Hg( $\ell$ ), produced.

A) 2.5 g B) 5.0 g C) 9.9 g D) 13 g E) 15 g A) 2.5 g B) 5.0 g C) 9.9 g D) 13 g E) 15 g

The standard cell potential of the given electrochemical cell is 0.19 V. Pt | Sn4+(aq, 1.0 M), Sn2+(aq, 1.0 M) || Cu2+(aq, 0.200 M) | Cu Which of the following factors will increase the measured cell potential of the given electrochemical cell?

A) Switching from a platinum to a graphite anode B) Increasing the size of the anode C) Decreasing the concentration of Cu2+ D) Increasing the concentration of Sn4+ E) Decreasing the temperature of the cell A) Switching from a platinum to a graphite anode B) Increasing the size of the anode C) Decreasing the concentration of Cu2+ D) Increasing the concentration of Sn4+ E) Decreasing the temperature of the cell

Calculate Ecell for the following electrochemical cell at 25 °C Pt(s) | H2(g, 1.00 atm) | H+(aq, 1.00 M) || Sn2+(aq, 0.350 M), Sn4+(aq, 0.020 M) | Pt(s) The standard reduction potentials are as follows: Sn4+(aq) + 2 e- → Sn2+(s) E° = +0.15 V 2 H+(aq) + 2 e- → H2(g) E° = 0.00 V

A) -0.19 V B) +0.08 V C) +0.11 V D) +0.19 V E) +0.22 V A) -0.19 V B) +0.08 V C) +0.11 V D) +0.19 V E) +0.22 V

Exam 20: Principles of Chemical Reactivity: Electron Transfer Reactions

Which of the following statements is true concerning the electrochemical cell Zn(s) | Zn²⁺(aq, 1.0 M) || Ca²⁺(aq, 1.0 M) | Ca(s) The standard reduction potentials are given follows: Zn²⁺(aq) + 2 e− → Zn(s); E° = -0.76 V Ca²⁺(aq) + 2 e− → Ca(s); E° = -2.87 V

(Multiple Choice)

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Question 21

Which of the following statements is true concerning the voltaic cell shown below?

(Multiple Choice)

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Question 22

Which of the following is true for a product-favored reaction at equilibrium?

(Multiple Choice)

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Question 23

Write a balanced half-reaction for the reduction of hydrogen peroxide to water in an acidic solution.

(Multiple Choice)

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Question 24

For the following cell reaction, the standard cell potential is 1.34 V. To determine the cell potential at nonstandard conditions, what is the value that should be used for n in the Nernst equation? $2 \mathrm { MnO } _ { 4 } ^ { - } ( \mathrm { aq } ) + 5 \mathrm { H } _ { 2 } \mathrm { SO } _ { 3 } ( \mathrm { aq } ) \rightarrow 2 \mathrm { Mn } ^ { 2 + } ( \mathrm { aq } ) + 5 \mathrm { SO } _ { 4 } ^ { 2 - } ( \mathrm { aq } ) + 4 \mathrm { H } ^ { + } ( \mathrm { aq } ) + 3 \mathrm { H } _ { 2 } \mathrm { O } ( \mathrm { l } )$

(Multiple Choice)

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Question 25

Calculate Δ_rG° for the disproportionation reaction of copper(I) ion (Cu⁺) at 25 °C. 2 Cu⁺(aq) → Cu²⁺(aq) + Cu(s) The standard reduction potentials are as follows: Cu⁺(aq) + e^- → Cu(s) E° = +0.518 V Cu²⁺(aq) + 2 e^- → Cu(s) E° = +0.337 V

(Multiple Choice)

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Question 26

Which of the following statements concerning voltaic cells is not true?

(Multiple Choice)

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Question 27

Which of the following is the cell notation for a cell in which the hydrogen electrode is the anode and the cathode half-reaction is Co³⁺(aq) + e− → Co²⁺(aq)?

(Multiple Choice)

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Question 28

The standard reduction potentials are as follows: Cr³⁺(aq) + 3 e^- → Cr(s); E° = -0.74 V Fe²⁺(aq) + 2 e^- → Fe(s); E° = -0.41 V Calculate the standard Gibbs free energy change for the following reaction. 2 Cr(s) + 3 Fe²⁺ → 3 Fe(s) + 2 Cr³⁺(aq)

(Multiple Choice)

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Question 29

Balance the following half-reaction occurring in an acidic solution. NO₃^-(aq) → NO(aq)

(Multiple Choice)

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Question 30

Batteries used in watches contain mercury(II) oxide. As the current flows, mercury(II) oxide is reduced to mercury according to the following reaction: HgO(s) + H₂O( $\ell$ ) + 2 e^- ? Hg( $\ell$ ) + 2 OH^-(aq) If 2.3 × 10^-5 amperes flows continuously for 1200 days, calculate the mass of mercury, Hg( $\ell$ ), produced.

(Multiple Choice)

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Question 31

The standard cell potential of the given electrochemical cell is 0.19 V. Pt | Sn⁴⁺(aq, 1.0 M), Sn²⁺(aq, 1.0 M) || Cu²⁺(aq, 0.200 M) | Cu Which of the following factors will increase the measured cell potential of the given electrochemical cell?

(Multiple Choice)

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Question 32

According to the cell notation below, which of the following species is undergoing reduction? Ni | Ni²⁺(aq) || Mn²⁺(aq) | MnO₂(s) | Pt(s)

(Multiple Choice)

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Question 33

What half-reaction occurs at the cathode during the electrolysis of molten potassium bromide?

(Multiple Choice)

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Question 34

If ?_rG° for the following reaction is -22.2 kJ/mol-rxn, calculate $E _ { \text {cell } } ^ { \circ }$ for the following reaction: Cu²⁺(aq) + 2 Ag(s) + 2 Cl^-(aq) ? Cu(s) + 2 AgCl(s)

(Multiple Choice)

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Question 35

The cell potential of the following electrochemical cell is determined by using an unspecified concentration of acid. Calculate the pH of the acid solution, given that the measured cell potential is -0.431 V and the anode reduction potential (E°) is 0.222 V at 25 °C. Ag(s) | AgCl(s) | Cl−(aq, 1.0 M) || H⁺(aq) | H₂(g, 1.0 atm) | Pt(s)

(Multiple Choice)

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Question 36

Calculate E_cell for the following electrochemical cell at 25 °C Pt(s) | H₂(g, 1.00 atm) | H⁺(aq, 1.00 M) || Sn²⁺(aq, 0.350 M), Sn⁴⁺(aq, 0.020 M) | Pt(s) The standard reduction potentials are as follows: Sn⁴⁺(aq) + 2 e^- → Sn²⁺(s) E° = +0.15 V 2 H⁺(aq) + 2 e^- → H₂(g) E° = 0.00 V

(Multiple Choice)

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Question 37

The use of electrical energy to produce chemical change is known as _____. An example of this process is the reduction of sodium chloride, NaCl( $\ell$ ), to produce solid sodium.

(Short Answer)

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Question 38

Which of the following statements is true for the following reaction, assuming the given reaction proceeds in the forward direction? Fe³⁺(aq) + Co(s) → Fe²⁺(aq) + Co²⁺(aq)

(Multiple Choice)

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Question 39

Which of the following equations represents the Nernst equation?

(Multiple Choice)

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Question 40

Showing 21 - 40 of 83

Exam 20: Principles of Chemical Reactivity: Electron Transfer Reactions

Which of the following statements is true concerning the electrochemical cell Zn(s) | Zn2+(aq, 1.0 M) || Ca2+(aq, 1.0 M) | Ca(s) The standard reduction potentials are given follows: Zn2+(aq) + 2 e− → Zn(s); E° = -0.76 V Ca2+(aq) + 2 e− → Ca(s); E° = -2.87 V

Which of the following statements is true concerning the voltaic cell shown below?

Which of the following is true for a product-favored reaction at equilibrium?

Write a balanced half-reaction for the reduction of hydrogen peroxide to water in an acidic solution.

Calculate ΔrG° for the disproportionation reaction of copper(I) ion (Cu+) at 25 °C. 2 Cu+(aq) → Cu2+(aq) + Cu(s) The standard reduction potentials are as follows: Cu+(aq) + e- → Cu(s) E° = +0.518 V Cu2+(aq) + 2 e- → Cu(s) E° = +0.337 V

Which of the following statements concerning voltaic cells is not true?

Which of the following is the cell notation for a cell in which the hydrogen electrode is the anode and the cathode half-reaction is Co3+(aq) + e− → Co2+(aq)?

The standard reduction potentials are as follows: Cr3+(aq) + 3 e- → Cr(s); E° = -0.74 V Fe2+(aq) + 2 e- → Fe(s); E° = -0.41 V Calculate the standard Gibbs free energy change for the following reaction. 2 Cr(s) + 3 Fe2+ → 3 Fe(s) + 2 Cr3+(aq)

Balance the following half-reaction occurring in an acidic solution. NO3-(aq) → NO(aq)

The standard cell potential of the given electrochemical cell is 0.19 V. Pt | Sn4+(aq, 1.0 M), Sn2+(aq, 1.0 M) || Cu2+(aq, 0.200 M) | Cu Which of the following factors will increase the measured cell potential of the given electrochemical cell?

According to the cell notation below, which of the following species is undergoing reduction? Ni | Ni2+(aq) || Mn2+(aq) | MnO2(s) | Pt(s)

What half-reaction occurs at the cathode during the electrolysis of molten potassium bromide?

If ?rG° for the following reaction is -22.2 kJ/mol-rxn, calculate Ecell ∘E _ { \text {cell } } ^ { \circ }Ecell ∘​ for the following reaction: Cu2+(aq) + 2 Ag(s) + 2 Cl-(aq) ? Cu(s) + 2 AgCl(s)

Calculate Ecell for the following electrochemical cell at 25 °C Pt(s) | H2(g, 1.00 atm) | H+(aq, 1.00 M) || Sn2+(aq, 0.350 M), Sn4+(aq, 0.020 M) | Pt(s) The standard reduction potentials are as follows: Sn4+(aq) + 2 e- → Sn2+(s) E° = +0.15 V 2 H+(aq) + 2 e- → H2(g) E° = 0.00 V

The use of electrical energy to produce chemical change is known as _____. An example of this process is the reduction of sodium chloride, NaCl( ℓ\ellℓ ), to produce solid sodium.

Which of the following statements is true for the following reaction, assuming the given reaction proceeds in the forward direction? Fe3+(aq) + Co(s) → Fe2+(aq) + Co2+(aq)

Which of the following equations represents the Nernst equation?

Basic Concepts of Chemistry

Lets Review: the Tools of Quantitative Chemistry

Atoms, Molecules, and Ions

Chemical Reactions

Stoichiometry: Quantitative Information About Chemical Reactions

Principles of Chemical Reactivity: Energy and Chemical Reactions

The Structure of Atoms

The Structure of Atoms and Periodic Trends

Bonding and Molecular Structure

Bonding and Molecular Structure Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

The Solid State

Solutions and Their Behavior

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Chemical Reactivity: Equilibria

Principles of Chemical Reactivity: the Chemistry of Acids and Bases

Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Principles of Chemical Reactivity: Entropy and Free Energy

Environmental Chemistry: Earths Environment, Energy, and Sustainability

The Chemistry of the Main Group Elements

The Chemistry of the Transition Elements

Carbon: Not Just Another Element

Biochemistry

Nuclear Chemistry

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Which of the following statements is true concerning the electrochemical cell Zn(s) | Zn²⁺(aq, 1.0 M) || Ca²⁺(aq, 1.0 M) | Ca(s) The standard reduction potentials are given follows: Zn²⁺(aq) + 2 e− → Zn(s); E° = -0.76 V Ca²⁺(aq) + 2 e− → Ca(s); E° = -2.87 V

Calculate Δ_rG° for the disproportionation reaction of copper(I) ion (Cu⁺) at 25 °C. 2 Cu⁺(aq) → Cu²⁺(aq) + Cu(s) The standard reduction potentials are as follows: Cu⁺(aq) + e^- → Cu(s) E° = +0.518 V Cu²⁺(aq) + 2 e^- → Cu(s) E° = +0.337 V

Which of the following is the cell notation for a cell in which the hydrogen electrode is the anode and the cathode half-reaction is Co³⁺(aq) + e− → Co²⁺(aq)?

The standard reduction potentials are as follows: Cr³⁺(aq) + 3 e^- → Cr(s); E° = -0.74 V Fe²⁺(aq) + 2 e^- → Fe(s); E° = -0.41 V Calculate the standard Gibbs free energy change for the following reaction. 2 Cr(s) + 3 Fe²⁺ → 3 Fe(s) + 2 Cr³⁺(aq)

Balance the following half-reaction occurring in an acidic solution. NO₃^-(aq) → NO(aq)

The standard cell potential of the given electrochemical cell is 0.19 V. Pt | Sn⁴⁺(aq, 1.0 M), Sn²⁺(aq, 1.0 M) || Cu²⁺(aq, 0.200 M) | Cu Which of the following factors will increase the measured cell potential of the given electrochemical cell?

According to the cell notation below, which of the following species is undergoing reduction? Ni | Ni²⁺(aq) || Mn²⁺(aq) | MnO₂(s) | Pt(s)

If ?_rG° for the following reaction is -22.2 kJ/mol-rxn, calculate $E _ { \text {cell } } ^ { \circ }$ for the following reaction: Cu²⁺(aq) + 2 Ag(s) + 2 Cl^-(aq) ? Cu(s) + 2 AgCl(s)

The use of electrical energy to produce chemical change is known as _____. An example of this process is the reduction of sodium chloride, NaCl( $\ell$ ), to produce solid sodium.

Which of the following statements is true for the following reaction, assuming the given reaction proceeds in the forward direction? Fe³⁺(aq) + Co(s) → Fe²⁺(aq) + Co²⁺(aq)