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 E°cell for the cell for the reaction 2 Ga(s)+ 3 Sn4+(aq)→ 3 Sn2+(aq)+2 Ga3+(aq). The standard reduction potentials are as follows: Ga3+(aq)+ 3 e− → Ga(s) E° = -0.55 V Sn4+(aq)+ 2 e− → Sn2+(aq) E° = 0.15V

A) 0.70 V B) 0.40 V C) 0.33 V D) -0.40 V E) −0.70 V A) 0.70 V B) 0.40 V C) 0.33 V D) -0.40 V E) −0.70 V

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

Claculate the mass of chromium that can be deposited by electrolysis of an aqueous solution of chromium(III)sulfate,Cr2(SO4)3,for 180 min using a constant current of 11.0 A.Assume 100% current efficiency.(F = 96485 C/mol)

A) 0.356 g B) 21.3 g C) 192.1 g D) 0.187 g E) 32.0 g A) 0.356 g B) 21.3 g C) 192.1 g D) 0.187 g E) 32.0 g

Calculate the standard reduction potential for the given reaction at 25 °C. AuCl4-(aq)+ 3 e- → Au(s)+ 4 Cl-(aq) The thermodynamic information is as follows: Au3+(aq)+ 3 e- → Au(s) E° = +1.50 V Au3+(aq)+ 4 Cl-(aq)→ AuCl4-(aq) Kf = 2.3 × 1025

A) -1.28 V B) -0.50 V C) +1.00 V D) +1.28 V E) +3.85 V A) -1.28 V B) -0.50 V C) +1.00 V D) +1.28 V E) +3.85 V

Calculate for the electrochemical cell Ag(s)| AgCl(s)| Cl-(aq,1.0 M)|| Cu2+(aq,1.0 M)| Cu(s). The standard reduction potentials are as follows: Cu2+(aq)+ 2 e- → Cu(s) E° = +0.337 V AgCl(s)+ e- → Ag(s)+ Cl-(aq) E° = +0.222 V

A) -0.115 V B) -0.107 V C) +0.115 V D) +0.452 V E) +0.559 V A) -0.115 V B) -0.107 V C) +0.115 V D) +0.452 V E) +0.559 V

Calculate the copper(II)ion concentration at 25 °C in the cell Zn(s)| Zn2+(aq,1.0 M)|| Cu2+(aq)| Cu(s)if the measured cell potential is 1.06 V.The standard cell potential is 1.10 V.

A) 0.21 M B) 1.0 M C) 0.045 M D) 1.0 M.. E) 1.0 M. A) 0.21 M B) 1.0 M C) 0.045 M D) 1.0 M.. E) 1.0 M.

Exam 20: Principles of Chemical Reactivity: Electron Transfer Reactions

Calculate the value of the reaction quotient,Q,for the voltaic cell constructed from the following two half-reactions when the Zn²⁺ion concentration is 0.0110 M and the Ag⁺ ion concentration is 1.27 M? → →

(Multiple Choice)

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Question 41

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 42

Calculate E°_cell for the cell for the reaction 2 Ga(s)+ 3 Sn⁴⁺(aq)→ 3 Sn²⁺(aq)+2 Ga³⁺(aq). The standard reduction potentials are as follows: Ga³⁺(aq)+ 3 e− → Ga(s) E° = -0.55 V Sn⁴⁺(aq)+ 2 e− → Sn²⁺(aq) E° = 0.15V

(Multiple Choice)

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Question 43

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

(Short Answer)

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Question 44

When a secondary battery provides electrical energy,it is acting as a voltaic cell.When the battery is recharging,it is operating as a(n)_____ cell.

(Short Answer)

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Question 45

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 46

Claculate the mass of chromium that can be deposited by electrolysis of an aqueous solution of chromium(III)sulfate,Cr₂(SO₄)₃,for 180 min using a constant current of 11.0 A.Assume 100% current efficiency.(F = 96485 C/mol)

(Multiple Choice)

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Question 47

Calculate the standard reduction potential for the given reaction at 25 °C. AuCl₄^-(aq)+ 3 e^- → Au(s)+ 4 Cl^-(aq) The thermodynamic information is as follows: Au³⁺(aq)+ 3 e^- → Au(s) E° = +1.50 V Au³⁺(aq)+ 4 Cl^-(aq)→ AuCl₄^-(aq) K_f = 2.3 × 10²⁵

(Multiple Choice)

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Question 48

Calculate for the electrochemical cell Ag(s)| AgCl(s)| Cl^-(aq,1.0 M)|| Cu²⁺(aq,1.0 M)| Cu(s). The standard reduction potentials are as follows: Cu²⁺(aq)+ 2 e^- → Cu(s) E° = +0.337 V AgCl(s)+ e^- → Ag(s)+ Cl^-(aq) E° = +0.222 V

(Multiple Choice)

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Question 49

Calculate the charge,in coulombs,is required to deposit 1.5 g of solid magnesium from a solution of Mg²⁺(aq)ion.

(Multiple Choice)

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Question 50

In an electrolytic cell,reduction occurs at the _ and oxidation occurs at the _.

(Short Answer)

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Question 51

Write balanced reduction and oxidation half-reactions for the processes that occur at the cathode and anode of a fuel cell used in NASA's space shuttles.

(Essay)

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Question 52

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 53

Gold and platinum are commonly used as inert electrodes in laboratory experiments.In commercial applications,such as batteries,_____ is more commonly used as an inert electrodes because it is far less expensive.

(Short Answer)

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Question 54

If the = -0.362 V for a given electrochemical cell at 25 °C,calculate the pH of the solution at the cathode. Pt | H₂(g,1.0 atm)| H⁺(aq,1.00 M)|| H⁺(aq)| H₂(g,1.0 atm)| Pt

(Multiple Choice)

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Question 55

A current of 12.0 A is passed through molten magnesium chloride for 14.0 h.How many moles of magnesium metal can be produced from this electrolysis?

(Multiple Choice)

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Question 56

Which of the following species are likely to behave as oxidizing agents? Li(s),H₂(g),MnO₄^-(aq),and Cl^-(aq)

(Multiple Choice)

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Question 57

Explain the function of a salt bridge in a voltaic cell.

(Essay)

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Question 58

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( )+ 2 e^- → Hg( )+ 2 OH^-(aq) If 2.3 × 10^-5 amperes flows continuously for 1200 days,calculate the mass of mercury,Hg( ),produced.

(Multiple Choice)

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Question 59

Calculate the copper(II)ion concentration at 25 °C in the cell Zn(s)| Zn²⁺(aq,1.0 M)|| Cu²⁺(aq)| Cu(s)if the measured cell potential is 1.06 V.The standard cell potential is 1.10 V.

(Multiple Choice)

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Question 60

Showing 41 - 60 of 86

Exam 20: Principles of Chemical Reactivity: Electron Transfer Reactions

Calculate the value of the reaction quotient,Q,for the voltaic cell constructed from the following two half-reactions when the Zn2+ion concentration is 0.0110 M and the Ag+ ion concentration is 1.27 M? → →

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?

Calculate E°cell for the cell for the reaction 2 Ga(s)+ 3 Sn4+(aq)→ 3 Sn2+(aq)+2 Ga3+(aq). The standard reduction potentials are as follows: Ga3+(aq)+ 3 e− → Ga(s) E° = -0.55 V Sn4+(aq)+ 2 e− → Sn2+(aq) E° = 0.15V ​

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

When a secondary battery provides electrical energy,it is acting as a voltaic cell.When the battery is recharging,it is operating as a(n)_____ cell.

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)

Claculate the mass of chromium that can be deposited by electrolysis of an aqueous solution of chromium(III)sulfate,Cr2(SO4)3,for 180 min using a constant current of 11.0 A.Assume 100% current efficiency.(F = 96485 C/mol)

Calculate the standard reduction potential for the given reaction at 25 °C. AuCl4-(aq)+ 3 e- → Au(s)+ 4 Cl-(aq) The thermodynamic information is as follows: Au3+(aq)+ 3 e- → Au(s) E° = +1.50 V Au3+(aq)+ 4 Cl-(aq)→ AuCl4-(aq) Kf = 2.3 × 1025

Calculate for the electrochemical cell Ag(s)| AgCl(s)| Cl-(aq,1.0 M)|| Cu2+(aq,1.0 M)| Cu(s). The standard reduction potentials are as follows: Cu2+(aq)+ 2 e- → Cu(s) E° = +0.337 V AgCl(s)+ e- → Ag(s)+ Cl-(aq) E° = +0.222 V

Calculate the charge,in coulombs,is required to deposit 1.5 g of solid magnesium from a solution of Mg2+(aq)ion.

In an electrolytic cell,reduction occurs at the _____ and oxidation occurs at the _____.

Write balanced reduction and oxidation half-reactions for the processes that occur at the cathode and anode of a fuel cell used in NASA's space shuttles.

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)?

Gold and platinum are commonly used as inert electrodes in laboratory experiments.In commercial applications,such as batteries,_____ is more commonly used as an inert electrodes because it is far less expensive.

If the = -0.362 V for a given electrochemical cell at 25 °C,calculate the pH of the solution at the cathode. Pt | H2(g,1.0 atm)| H+(aq,1.00 M)|| H+(aq)| H2(g,1.0 atm)| Pt

A current of 12.0 A is passed through molten magnesium chloride for 14.0 h.How many moles of magnesium metal can be produced from this electrolysis?

Which of the following species are likely to behave as oxidizing agents? Li(s),H2(g),MnO4-(aq),and Cl-(aq)

Explain the function of a salt bridge in a voltaic cell.

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( )+ 2 e- → Hg( )+ 2 OH-(aq) If 2.3 × 10-5 amperes flows continuously for 1200 days,calculate the mass of mercury,Hg( ),produced.

Calculate the copper(II)ion concentration at 25 °C in the cell Zn(s)| Zn2+(aq,1.0 M)|| Cu2+(aq)| Cu(s)if the measured cell potential is 1.06 V.The standard cell potential is 1.10 V.

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

Filters

Calculate the value of the reaction quotient,Q,for the voltaic cell constructed from the following two half-reactions when the Zn²⁺ion concentration is 0.0110 M and the Ag⁺ ion concentration is 1.27 M? → →

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?

Calculate E°_cell for the cell for the reaction 2 Ga(s)+ 3 Sn⁴⁺(aq)→ 3 Sn²⁺(aq)+2 Ga³⁺(aq). The standard reduction potentials are as follows: Ga³⁺(aq)+ 3 e− → Ga(s) E° = -0.55 V Sn⁴⁺(aq)+ 2 e− → Sn²⁺(aq) E° = 0.15V

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)

Claculate the mass of chromium that can be deposited by electrolysis of an aqueous solution of chromium(III)sulfate,Cr₂(SO₄)₃,for 180 min using a constant current of 11.0 A.Assume 100% current efficiency.(F = 96485 C/mol)

Calculate the standard reduction potential for the given reaction at 25 °C. AuCl₄^-(aq)+ 3 e^- → Au(s)+ 4 Cl^-(aq) The thermodynamic information is as follows: Au³⁺(aq)+ 3 e^- → Au(s) E° = +1.50 V Au³⁺(aq)+ 4 Cl^-(aq)→ AuCl₄^-(aq) K_f = 2.3 × 10²⁵

Calculate for the electrochemical cell Ag(s)| AgCl(s)| Cl^-(aq,1.0 M)|| Cu²⁺(aq,1.0 M)| Cu(s). The standard reduction potentials are as follows: Cu²⁺(aq)+ 2 e^- → Cu(s) E° = +0.337 V AgCl(s)+ e^- → Ag(s)+ Cl^-(aq) E° = +0.222 V

Calculate the charge,in coulombs,is required to deposit 1.5 g of solid magnesium from a solution of Mg²⁺(aq)ion.

In an electrolytic cell,reduction occurs at the _ and oxidation occurs at the _.

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)?

If the = -0.362 V for a given electrochemical cell at 25 °C,calculate the pH of the solution at the cathode. Pt | H₂(g,1.0 atm)| H⁺(aq,1.00 M)|| H⁺(aq)| H₂(g,1.0 atm)| Pt

Which of the following species are likely to behave as oxidizing agents? Li(s),H₂(g),MnO₄^-(aq),and Cl^-(aq)

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( )+ 2 e^- → Hg( )+ 2 OH^-(aq) If 2.3 × 10^-5 amperes flows continuously for 1200 days,calculate the mass of mercury,Hg( ),produced.

Calculate the copper(II)ion concentration at 25 °C in the cell Zn(s)| Zn²⁺(aq,1.0 M)|| Cu²⁺(aq)| Cu(s)if the measured cell potential is 1.06 V.The standard cell potential is 1.10 V.