Calculate the equilibrium constant for the reaction below at 25 °C. Co(s)+ 2 Cr3+(aq)→ Co2+(aq)+ 2 Cr2+(aq) The standard reduction potentials are as follows: Co2+(aq)+ 2 e- → Co(s) E° = -0.28 V Cr3+(aq)+ e- → Cr2+(aq) E° = -0.41 V

A) 4.0 × 10-5 B) 2.5 × 104 C) 1.0 × 105 D) 1.2 × 105 E) 1.3 × 105 A) 4.0 × 10-5 B) 2.5 × 104 C) 1.0 × 105 D) 1.2 × 105 E) 1.3 × 105

Consider the following half-reactions. Ag+(aq)+ e- → Ag(s) E° = +0.80 V Cu2+(aq)+ 2 e- → Cu(s) E° = +0.34 V Pb2+(aq)+ 2 e- → Pb(s) E° = -0.13 V Fe2+(aq)+ 2 e- → Fe(s) E° = -0.44 V Al3+(aq)+ 3 e- → Al(s) E° = -1.66 V Which of the following species will oxidize lead,Pb(s)?

A) Ag+(aq)and Cu2+(aq) B) Ag(s)and Cu(s) C) Fe2+(aq)and Al3+(aq) D) Fe(s)and Al(s) E) Cu2+(aq)and Fe2+(aq) A) Ag+(aq)and Cu2+(aq) B) Ag(s)and Cu(s) C) Fe2+(aq)and Al3+(aq) D) Fe(s)and Al(s) E) Cu2+(aq)and Fe2+(aq)

Exam 20: Principles of Chemical Reactivity: Electron Transfer Reactions

Write a balanced chemical equation for the oxidation of solid cadmium by concentrated nitric acid,producing nitrogen dioxide gas and Cd²⁺(aq)ion.

(Multiple Choice)

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Question 61

If Δ_rG° for the following reaction is -22.2 kJ/mol-rxn,calculate for the following reaction: Cu²⁺(aq)+ 2 Ag(s)+ 2 Cl^-(aq)→ Cu(s)+ 2 AgCl(s)

(Multiple Choice)

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Question 62

How many moles of electrons are produced from a current of 17.0 A in 3.40 hours?

(Multiple Choice)

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Question 63

Calculate the equilibrium constant for the reaction below at 25 °C. Co(s)+ 2 Cr³⁺(aq)→ Co²⁺(aq)+ 2 Cr²⁺(aq) The standard reduction potentials are as follows: Co²⁺(aq)+ 2 e^- → Co(s) E° = -0.28 V Cr³⁺(aq)+ e^- → Cr²⁺(aq) E° = -0.41 V

(Multiple Choice)

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Question 64

If an electric current is passed through a solution of molten potassium bromide,KBr,the product at the cathode is _____.

(Short Answer)

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Question 65

Consider the following half-reactions. Ag⁺(aq)+ e^- → Ag(s) E° = +0.80 V Cu²⁺(aq)+ 2 e^- → Cu(s) E° = +0.34 V Pb²⁺(aq)+ 2 e^- → Pb(s) E° = -0.13 V Fe²⁺(aq)+ 2 e^- → Fe(s) E° = -0.44 V Al³⁺(aq)+ 3 e^- → Al(s) E° = -1.66 V Which of the following species will oxidize lead,Pb(s)?

(Multiple Choice)

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Question 66

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

(Multiple Choice)

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Question 67

Calculate for the electrochemical cell Pb(s)|PbCl₂(s)| Cl^-(aq,1.0 M)|| Fe³⁺(aq,1.0 M),Fe²⁺(aq,1.0 M)| Pt(s). The standard reduction potentials are as follows: Pb²⁺(aq)+ 2 e^- → Pb(s) E° = -0.126 V PbCl₂(s)+ 2 e^- → Pb(s)+ 2 Cl^-(aq) E° = -0.267 V Fe³⁺(aq)+ e^- → Fe²⁺(aq) E° = +0.771 V Fe²⁺(aq)+ e^- → Fe(s) E° = -0.44 V

(Multiple Choice)

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Question 68

Write a balanced net ionic equation for the overall reaction represented by the following cell notation. Cu(s)| Cu²⁺(aq)|| Mn²⁺(aq)| Mn(s)

(Multiple Choice)

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Question 69

In the given electrochemical cell,which of the following is the cathode half-reaction? Zn(s)| Zn²⁺(aq)|| Fe³⁺(aq),Fe²⁺(aq)| Pt(s)

(Multiple Choice)

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Question 70

Use the following standard reduction potentials to determine which species is the best oxidizing agent. O₂(g)+ 4 H⁺(aq)+ 4 e^- → 2 H₂O( ) E° = +1.229 V Hg₂²⁺(aq)+ 2 e^- → 2 Hg( ) E° = +0.789 V I₂(s)+ 2 e^- → 2 I^-(aq) E° = +0.535 V

(Multiple Choice)

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Question 71

A voltaic cell or galvanic cell converts chemical energy to electrical energy. for the given galvanic cell is -1.80 V. Fe²⁺(aq)+ 2 Cl^-(aq)→ Fe(s)+ Cl₂(g) Calculate the value of Δ_rG° for the reaction.

(Multiple Choice)

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Question 72

How many electrons are transferred in the given reaction? Ni + 2 HCl → Ni Cl₂ + H₂

(Multiple Choice)

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Question 73

Write a balanced net ionic equation for the reaction below in an acidic solution. Cr₂O₇^2-(aq)+ Ni(s)→ Cr³⁺(aq)+ Ni²⁺(aq)

(Multiple Choice)

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Question 74

Use the following standard reduction potentials to determine which species is the strongest reducing agent. 2 H⁺(aq)+ 2 e^- → H₂(g); 0.00 V K⁺(aq)+ e^- → K(s); -2.93 V F₂(g)+ 2 e^- → 2 F^-(aq); 2.87 V Al³⁺(aq)+ 3 e^- → Al(s); -1.66 V Pb²⁺(aq)+ 2 e^- → Pb(s); -0.13 V

(Multiple Choice)

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Question 75

Write a balanced chemical equation for the following reaction in a basic solution. ClO^-(aq)+ Cr(OH)₃(s)→ Cl^-(aq)+ CrO₄^2-(aq)

(Multiple Choice)

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Question 76

When the following oxidation-reduction reaction in acidic solution is balanced,what is the lowest whole-number coefficient for Na⁺(aq)ion? Na(s)+ Ca²⁺(aq)→ Na⁺(aq)+ Ca(s)

(Multiple Choice)

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Question 77

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

(Multiple Choice)

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Question 78

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

(Multiple Choice)

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Question 79

Balance the following oxidation-reduction reaction occurring in an acidic solution. MnO₄^-(aq)+ Cr²⁺(aq)→ Mn²⁺(aq)+ Cr³⁺(aq)

(Multiple Choice)

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Question 80

Showing 61 - 80 of 86

Exam 20: Principles of Chemical Reactivity: Electron Transfer Reactions

Write a balanced chemical equation for the oxidation of solid cadmium by concentrated nitric acid,producing nitrogen dioxide gas and Cd2+(aq)ion.

If ΔrG° for the following reaction is -22.2 kJ/mol-rxn,calculate for the following reaction: Cu2+(aq)+ 2 Ag(s)+ 2 Cl-(aq)→ Cu(s)+ 2 AgCl(s)

How many moles of electrons are produced from a current of 17.0 A in 3.40 hours?

Calculate the equilibrium constant for the reaction below at 25 °C. Co(s)+ 2 Cr3+(aq)→ Co2+(aq)+ 2 Cr2+(aq) The standard reduction potentials are as follows: Co2+(aq)+ 2 e- → Co(s) E° = -0.28 V Cr3+(aq)+ e- → Cr2+(aq) E° = -0.41 V

If an electric current is passed through a solution of molten potassium bromide,KBr,the product at the cathode is _____.

Consider the following half-reactions. Ag+(aq)+ e- → Ag(s) E° = +0.80 V Cu2+(aq)+ 2 e- → Cu(s) E° = +0.34 V Pb2+(aq)+ 2 e- → Pb(s) E° = -0.13 V Fe2+(aq)+ 2 e- → Fe(s) E° = -0.44 V Al3+(aq)+ 3 e- → Al(s) E° = -1.66 V Which of the following species will oxidize lead,Pb(s)?

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

Write a balanced net ionic equation for the overall reaction represented by the following cell notation. Cu(s)| Cu2+(aq)|| Mn2+(aq)| Mn(s)

In the given electrochemical cell,which of the following is the cathode half-reaction? Zn(s)| Zn2+(aq)|| Fe3+(aq),Fe2+(aq)| Pt(s)

Use the following standard reduction potentials to determine which species is the best oxidizing agent. O2(g)+ 4 H+(aq)+ 4 e- → 2 H2O( ) E° = +1.229 V Hg22+(aq)+ 2 e- → 2 Hg( ) E° = +0.789 V I2(s)+ 2 e- → 2 I-(aq) E° = +0.535 V

A voltaic cell or galvanic cell converts chemical energy to electrical energy. for the given galvanic cell is -1.80 V. Fe2+(aq)+ 2 Cl-(aq)→ Fe(s)+ Cl2(g) Calculate the value of ΔrG° for the reaction.

How many electrons are transferred in the given reaction? Ni + 2 HCl → Ni Cl2 + H2

Write a balanced net ionic equation for the reaction below in an acidic solution. Cr2O72-(aq)+ Ni(s)→ Cr3+(aq)+ Ni2+(aq)

Use the following standard reduction potentials to determine which species is the strongest reducing agent. 2 H+(aq)+ 2 e- → H2(g); 0.00 V K+(aq)+ e- → K(s); -2.93 V F2(g)+ 2 e- → 2 F-(aq); 2.87 V Al3+(aq)+ 3 e- → Al(s); -1.66 V Pb2+(aq)+ 2 e- → Pb(s); -0.13 V

Write a balanced chemical equation for the following reaction in a basic solution. ClO-(aq)+ Cr(OH)3(s)→ Cl-(aq)+ CrO42-(aq)

When the following oxidation-reduction reaction in acidic solution is balanced,what is the lowest whole-number coefficient for Na+(aq)ion? Na(s)+ Ca2+(aq)→ Na+(aq)+ Ca(s)

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

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

Balance the following oxidation-reduction reaction occurring in an acidic solution. MnO4-(aq)+ Cr2+(aq)→ Mn2+(aq)+ Cr3+(aq)

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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Write a balanced chemical equation for the oxidation of solid cadmium by concentrated nitric acid,producing nitrogen dioxide gas and Cd²⁺(aq)ion.

If Δ_rG° for the following reaction is -22.2 kJ/mol-rxn,calculate for the following reaction: Cu²⁺(aq)+ 2 Ag(s)+ 2 Cl^-(aq)→ Cu(s)+ 2 AgCl(s)

Calculate the equilibrium constant for the reaction below at 25 °C. Co(s)+ 2 Cr³⁺(aq)→ Co²⁺(aq)+ 2 Cr²⁺(aq) The standard reduction potentials are as follows: Co²⁺(aq)+ 2 e^- → Co(s) E° = -0.28 V Cr³⁺(aq)+ e^- → Cr²⁺(aq) E° = -0.41 V

Write a balanced net ionic equation for the overall reaction represented by the following cell notation. Cu(s)| Cu²⁺(aq)|| Mn²⁺(aq)| Mn(s)

In the given electrochemical cell,which of the following is the cathode half-reaction? Zn(s)| Zn²⁺(aq)|| Fe³⁺(aq),Fe²⁺(aq)| Pt(s)

Use the following standard reduction potentials to determine which species is the best oxidizing agent. O₂(g)+ 4 H⁺(aq)+ 4 e^- → 2 H₂O( ) E° = +1.229 V Hg₂²⁺(aq)+ 2 e^- → 2 Hg( ) E° = +0.789 V I₂(s)+ 2 e^- → 2 I^-(aq) E° = +0.535 V

A voltaic cell or galvanic cell converts chemical energy to electrical energy. for the given galvanic cell is -1.80 V. Fe²⁺(aq)+ 2 Cl^-(aq)→ Fe(s)+ Cl₂(g) Calculate the value of Δ_rG° for the reaction.

How many electrons are transferred in the given reaction? Ni + 2 HCl → Ni Cl₂ + H₂

Write a balanced net ionic equation for the reaction below in an acidic solution. Cr₂O₇^2-(aq)+ Ni(s)→ Cr³⁺(aq)+ Ni²⁺(aq)

Use the following standard reduction potentials to determine which species is the strongest reducing agent. 2 H⁺(aq)+ 2 e^- → H₂(g); 0.00 V K⁺(aq)+ e^- → K(s); -2.93 V F₂(g)+ 2 e^- → 2 F^-(aq); 2.87 V Al³⁺(aq)+ 3 e^- → Al(s); -1.66 V Pb²⁺(aq)+ 2 e^- → Pb(s); -0.13 V

Write a balanced chemical equation for the following reaction in a basic solution. ClO^-(aq)+ Cr(OH)₃(s)→ Cl^-(aq)+ CrO₄^2-(aq)

When the following oxidation-reduction reaction in acidic solution is balanced,what is the lowest whole-number coefficient for Na⁺(aq)ion? Na(s)+ Ca²⁺(aq)→ Na⁺(aq)+ Ca(s)

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

Balance the following oxidation-reduction reaction occurring in an acidic solution. MnO₄^-(aq)+ Cr²⁺(aq)→ Mn²⁺(aq)+ Cr³⁺(aq)