The standard reduction potentials for a reaction are as follows: Pb2+(aq) + 2 e- ? Pb(s) E° = -0.126 V PbSO4(s) + 2 e- ? Pb(s) + SO42-(aq) E° = -0.355 V Calculate the Ksp for lead(II)sulfate (PbSO4) at 25 °C.

A) 3.4 × 10-28 B) 1.8 × 10-8 C) 5.6 × 10-5 D) 5.6 × 107 E) 2.9 × 1037 A) 3.4 × 10-28 B) 1.8 × 10-8 C) 5.6 × 10-5 D) 5.6 × 107 E) 2.9 × 1037

Calculate the standard cell potential ( $E _ { \text {cell } } ^ { \circ }$ ) for the reaction 2 Ag(s) + Co2+(aq) ? 2 Ag+(aq) + Co(s). The standard reduction potentials are as follows: Ag+(aq) + e-? Ag(s) E° = 0.8 V Co2+(aq) +2 e-? Co(s) E° = -0.277 V

A) -1.077 V B) 1.077 V C) -1.877 V D) 1.877 V E) 1.323 V A) -1.077 V B) 1.077 V C) -1.877 V D) 1.877 V E) 1.323 V

Calculate the equilibrium constant for the following reaction at 25 °C, 2 IO3-(aq) + 5 Hg( $\ell$ ) + 12 H+(aq) ? I2(s) + 5 Hg2+(aq) + 6 H2O( $\ell$ ) The standard reduction potentials are as follows: IO3-(aq) + 6 H+(aq) + 5 e- ? I2(s) + 3 H2O( $\ell$ ) E° = +1.20 V Hg2+(aq) + 2 e- ? Hg( $\ell$ ) E° = +0.86 V

A) 3 × 10-58 B) 6 × 105 C) 3 × 1011 D) 6 × 1028 E) 3 × 1057 A) 3 × 10-58 B) 6 × 105 C) 3 × 1011 D) 6 × 1028 E) 3 × 1057

Write a balanced half-reaction for the reduction of CrO42-(aq) to Cr(OH)3(s) in a basic solution.

A) CrO42-(aq) + 3 OH-(aq) + 3 e- ? Cr(OH)3(s) + 2 O2(g) B) CrO42-(aq) + 3 H+(aq) + 3 e- ? Cr(OH)3(s) C) CrO42-(aq) + 3 H+(aq) ? Cr(OH)3(s) + 2 e- D) CrO42-(aq) + 4 H2O( $\ell$ ) + 3 e- ? Cr(OH)3(s) + 5 OH-(aq) E) CrO42-(aq) + 3 OH-(aq) ? Cr(OH)3(s) + 2 O2(g) A) CrO42-(aq) + 3 OH-(aq) + 3 e- ? Cr(OH)3(s) + 2 O2(g) B) CrO42-(aq) + 3 H+(aq) + 3 e- ? Cr(OH)3(s) C) CrO42-(aq) + 3 H+(aq) ? Cr(OH)3(s) + 2 e- D) CrO42-(aq) + 4 H2O( $\ell$ ) + 3 e- ? Cr(OH)3(s) + 5 OH-(aq) E) CrO42-(aq) + 3 OH-(aq) ? Cr(OH)3(s) + 2 O2(g)

Calculate the cell potential at 25 °C for the following overall reaction. Zn2+(aq) + 2 Fe2+(aq) → Zn(s) + 2 Fe3+(aq) [Zn2+] = 1.50 × 10-4 M, [Fe3+] = 0.0200 M, and [Fe2+] = 0.0100 M. The standard reduction potentials are as follows: Zn2+(aq) + 2 e- → Zn(s) E° = -0.763 V Fe3+(aq) + e- → Fe2+(aq) E° = +0.771 V

A) -1.665 V B) -1.534 V C) -1.439 V D) -0.008 V E) +0.008 V A) -1.665 V B) -1.534 V C) -1.439 V D) -0.008 V E) +0.008 V

Exam 20: Principles of Chemical Reactivity: Electron Transfer Reactions

Calculate E_cell for the following electrochemical cell at 25°C. The standard cell potential, E°_cell, is 0.460 V. Cu(s) | Cu²⁺(aq, 0.016 M) || Ag⁺(aq, 0.11 M) | Ag(s)

(Multiple Choice)

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Question 41

Write a balanced net ionic equation for the overall reaction represented by the following cell notation. Al(s) | Al³⁺(aq) || Cl₂(g) | Cl-(aq) | Pt(s)

(Multiple Choice)

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Question 42

Calculate $E _ { \text {cell } } ^ { \circ }$ 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 43

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 44

An SHE electrode has been assigned a standard reduction potential, E°, of 0.00 volts. Which of the following reactions will occur at this electrode?

(Multiple Choice)

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Question 45

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 46

One Faraday is defined as the:

(Multiple Choice)

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Question 47

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 48

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 49

The standard reduction potentials for a reaction are as follows: Pb²⁺(aq) + 2 e^- ? Pb(s) E° = -0.126 V PbSO₄(s) + 2 e^- ? Pb(s) + SO₄^2-(aq) E° = -0.355 V Calculate the K_sp for lead(II)sulfate (PbSO₄) at 25 °C.

(Multiple Choice)

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Question 50

Given the following two half-reactions, write the overall reaction in the direction in which it is product-favored, and calculate the standard cell potential. Pb²⁺(aq) + 2 e^- ? Pb(s) E° = -0.126 V Fe³⁺(aq) + e^- ? Fe²⁺(s) E° = +0.771 V

(Multiple Choice)

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Question 51

The unit for electromotive force, emf, is the volt. 1 volt is equal to _____.

(Multiple Choice)

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Question 52

Calculate the standard cell potential ( $E _ { \text {cell } } ^ { \circ }$ ) for the reaction 2 Ag(s) + Co²⁺(aq) ? 2 Ag⁺(aq) + Co(s). The standard reduction potentials are as follows: Ag⁺(aq) + e^-? Ag(s) E° = 0.8 V Co²⁺(aq) +2 e^-? Co(s) E° = -0.277 V

(Multiple Choice)

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Question 53

Calculate the equilibrium constant for the following reaction at 25 °C, 2 IO₃^-(aq) + 5 Hg( $\ell$ ) + 12 H⁺(aq) ? I₂(s) + 5 Hg²⁺(aq) + 6 H₂O( $\ell$ ) The standard reduction potentials are as follows: IO₃^-(aq) + 6 H⁺(aq) + 5 e^- ? I₂(s) + 3 H₂O( $\ell$ ) E° = +1.20 V Hg²⁺(aq) + 2 e^- ? Hg( $\ell$ ) E° = +0.86 V

(Multiple Choice)

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Question 54

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 55

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 56

Write a balanced half-reaction for the reduction of CrO₄^2-(aq) to Cr(OH)₃(s) in a basic solution.

(Multiple Choice)

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Question 57

Balance the following half-reaction occurring in a basic solution. MnO₂(s) → Mn(OH)₂(s)

(Multiple Choice)

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Question 58

For the electrochemical cell Cu(s) | Cu²⁺ || Ag⁺ | Ag(s), the standard cell potential is 0.46 V. A cell using these reagents was made, and the observed potential was 0.26 V at 25 ^oC. Which of the following is a possible explanation for the observed voltage?

(Multiple Choice)

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Question 59

Calculate the cell potential at 25 °C for the following overall reaction. Zn²⁺(aq) + 2 Fe²⁺(aq) → Zn(s) + 2 Fe³⁺(aq) [Zn²⁺] = 1.50 × 10^-4 M, [Fe³⁺] = 0.0200 M, and [Fe²⁺] = 0.0100 M. The standard reduction potentials are as follows: Zn²⁺(aq) + 2 e^- → Zn(s) E° = -0.763 V Fe³⁺(aq) + e^- → Fe²⁺(aq) E° = +0.771 V

(Multiple Choice)

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Question 60

Showing 41 - 60 of 83

Exam 20: Principles of Chemical Reactivity: Electron Transfer Reactions

Calculate Ecell for the following electrochemical cell at 25°C. The standard cell potential, E°cell, is 0.460 V. Cu(s) | Cu2+(aq, 0.016 M) || Ag+(aq, 0.11 M) | Ag(s) ​

Write a balanced net ionic equation for the overall reaction represented by the following cell notation. Al(s) | Al3+(aq) || Cl2(g) | Cl-(aq) | Pt(s)

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.

An SHE electrode has been assigned a standard reduction potential, E°, of 0.00 volts. Which of the following reactions will occur at this electrode?

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

One Faraday is defined as the:

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

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?

The standard reduction potentials for a reaction are as follows: Pb2+(aq) + 2 e- ? Pb(s) E° = -0.126 V PbSO4(s) + 2 e- ? Pb(s) + SO42-(aq) E° = -0.355 V Calculate the Ksp for lead(II)sulfate (PbSO4) at 25 °C.

Given the following two half-reactions, write the overall reaction in the direction in which it is product-favored, and calculate the standard cell potential. Pb2+(aq) + 2 e- ? Pb(s) E° = -0.126 V Fe3+(aq) + e- ? Fe2+(s) E° = +0.771 V

The unit for electromotive force, emf, is the volt. 1 volt is equal to _____.

Calculate the standard cell potential ( Ecell ∘E _ { \text {cell } } ^ { \circ }Ecell ∘​ ) for the reaction 2 Ag(s) + Co2+(aq) ? 2 Ag+(aq) + Co(s). The standard reduction potentials are as follows: Ag+(aq) + e-? Ag(s) E° = 0.8 V Co2+(aq) +2 e-? Co(s) E° = -0.277 V

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

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)

Write a balanced half-reaction for the reduction of CrO42-(aq) to Cr(OH)3(s) in a basic solution.

Balance the following half-reaction occurring in a basic solution. MnO2(s) → Mn(OH)2(s)

For the electrochemical cell Cu(s) | Cu2+ || Ag+ | Ag(s), the standard cell potential is 0.46 V. A cell using these reagents was made, and the observed potential was 0.26 V at 25 oC. Which of the following is a possible explanation for the observed voltage?

Basic Concepts of Chemistry

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Calculate E_cell for the following electrochemical cell at 25°C. The standard cell potential, E°_cell, is 0.460 V. Cu(s) | Cu²⁺(aq, 0.016 M) || Ag⁺(aq, 0.11 M) | Ag(s)

Write a balanced net ionic equation for the overall reaction represented by the following cell notation. Al(s) | Al³⁺(aq) || Cl₂(g) | Cl-(aq) | Pt(s)

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

The standard reduction potentials for a reaction are as follows: Pb²⁺(aq) + 2 e^- ? Pb(s) E° = -0.126 V PbSO₄(s) + 2 e^- ? Pb(s) + SO₄^2-(aq) E° = -0.355 V Calculate the K_sp for lead(II)sulfate (PbSO₄) at 25 °C.

Given the following two half-reactions, write the overall reaction in the direction in which it is product-favored, and calculate the standard cell potential. Pb²⁺(aq) + 2 e^- ? Pb(s) E° = -0.126 V Fe³⁺(aq) + e^- ? Fe²⁺(s) E° = +0.771 V

Calculate the standard cell potential ( $E _ { \text {cell } } ^ { \circ }$ ) for the reaction 2 Ag(s) + Co²⁺(aq) ? 2 Ag⁺(aq) + Co(s). The standard reduction potentials are as follows: Ag⁺(aq) + e^-? Ag(s) E° = 0.8 V Co²⁺(aq) +2 e^-? Co(s) E° = -0.277 V

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

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)

Write a balanced half-reaction for the reduction of CrO₄^2-(aq) to Cr(OH)₃(s) in a basic solution.

Balance the following half-reaction occurring in a basic solution. MnO₂(s) → Mn(OH)₂(s)

For the electrochemical cell Cu(s) | Cu²⁺ || Ag⁺ | Ag(s), the standard cell potential is 0.46 V. A cell using these reagents was made, and the observed potential was 0.26 V at 25 ^oC. Which of the following is a possible explanation for the observed voltage?