Question 1

The redox reaction of peroxydisulfate with iodide has been used for many years as part of the iodine clock reaction which introduces students to kinetics. If E°_cell = 1.587 V and E° of the cathode half-cell is 0.536 V, what is E° of the anode half-cell? S₂O₈^2-(aq) + 2H⁺ + 2I^-(aq) → 2HSO₄^-(aq) + I₂(aq)

Accepted Answer

E°_cell = E°_cathode + E°_anode1.587 V = 0.536 V + E°_anodeE°_anode = 1.587 V - 0.536 V = 1.051 V

Question 2

Examine the following half-reactions and select the strongest oxidizing agent among the species listed. Cr²⁺(aq) + 2e^- Cr(s) E° = -0.913 V Fe²⁺(aq) + 2e^- Fe(s) E° = -0.447 V Sr²⁺(aq) + 2e^- Sr(s) E° = -2.89 V Co²⁺(aq) + 2e^- Co(s) E° = -0.28 V

Accepted Answer

The answer of Examine the following half-reactions and select the...

Question 3

A voltaic cell has a standard cell potential equal to 0.74 V. If the standard electrode (reduction) potential for the anode is -0.22 V, what is the standard electrode potential for the cathode?

Accepted Answer

The answer of A voltaic cell has a standard cell...

Question 4

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)

Accepted Answer

Using the equation E°cell = E°cathode - E°anode, we can rearrange to solve for E°anode: 
E°anode = E°cathode - E°cell 
E°anode = 0.34 V - 0.62 V 
E°anode = -0.28 V 
Therefore, the answer is A) -0.28 V.

Question 5

Which of the following conditions is most likely to apply to a fully-charged secondary cell?

Accepted Answer

The answer of Which of the following conditions is most...

Question 6

When metal A is placed in a solution of metal ions B²⁺, a reaction occurs between A and B²⁺, and metal ions A²⁺ appear in the solution. When metal B is placed in acid solution, gas bubbles form on its surface. When metal A is placed in a solution of metal ions C²⁺, no reaction occurs. Which of the following reactions would not occur spontaneously?

Accepted Answer

The answer of When metal A is placed in a...

Question 7

Examine the following half-reactions and select the strongest reducing agent among the species listed. HgO(s) + H2O(l) + 2e^- Hg(l) + 2OH^-(aq) E°= 0.0977 V Zn(OH)₂(s) + 2e^- Zn(s) + 2OH^-(aq) E° = -1.25 V Ag₂O(s) + H₂O(l) + 2e^- Ag(s) + 2OH^-(aq) E° = 0.342 V B(OH)₃(aq) + 7H⁺(aq) + 8e^- BH4^-(aq) + 3H₂O(l) E° = -0.481 V

Accepted Answer

The strongest reducing agent is the species that will have the most negative E° value. Among the given half-reactions, Zn(s) has the most negative E° value of -1.25 V, indicating that it is the strongest reducing agent.

Question 8

Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. Co³⁺(aq) + e^- Co²⁺(aq) E° = 1.82 V MnO₄^-(aq) + 2H₂O(l) + 3e^- MnO₂(s) + 4OH^-(aq) E° = 0.59 V Overall reaction: MnO₄^-(aq) + 2H₂O(l) + 3Co²⁺(aq) → MnO₂(s) + 3Co³⁺(aq) + 4OH^-(aq)

Accepted Answer

The answer of Calculate E°cell and indicate whether the overall...

Question 9

What is the E°_cell for the cell represented by the combination of the following half-reactions? ClO₄(aq) + 8H(aq) + 8e Cl-(aq) + 4H₂O(l) E° = 1.389 V VO₂(aq) + 2H(aq) + e^- j VO(aq) + H₂O(l) E° = 0.991 V

Accepted Answer

The answer of What is the E°_cell for the cell...

Question 10

A voltaic cell can be prepared from copper and tin. What is the E°_cell for the cell that forms from the following half-reactions? Cu²⁺(aq) + 2e- Cu(s) E° = 0.34 V Sn⁴⁺(aq) + 2e- Sn²⁺(aq) E° = 0.13 V

Accepted Answer

The answer of A voltaic cell can be prepared from...

Question 11

Calculate E°_cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. H₂O₂(aq) + 2H⁺(aq) + 2e^- 2H₂O(l) E° = 1.77 V Fe³⁺ (aq) + e^- Fe²⁺(aq) E° = 0.77 V Overall reaction: 2Fe³⁺(aq) + 2H₂O(l) → H₂O₂(aq) + 2H⁺(aq) + 2Fe²⁺(aq)

Accepted Answer

To calculate E°_cell, we need to use the formula: E°_cell = E° cathode - E° anode The cathode is the reduction half-reaction (Fe³⁺ + e^- → Fe²⁺) with an E° of 0.77 V. The anode is the oxidation half-reaction (2H₂O → H₂O₂ + 2H+ + 2e-) with an E° of 1.77 V. Plugging in the values: E°_cell = 0.77 V - 1.77 V = -1.00 V Since E°_cell is negative, the overall reaction is nonspontaneous.

Question 12

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

Accepted Answer

The notation shows Al(s) on the left side and Co(s) on the right side, indicating that Al is the anode (oxidation) and Co is the cathode (reduction). Therefore, Al is the reducing agent, and Co is the oxidizing agent.

Question 13

Examine the following half-reactions and select the strongest oxidizing agent among the substances. [PtCl₄]^2-(aq) + 2e^- Pt(s) + 4Cl^-(aq) E° = 0.755 V RuO₄(s) + 8H⁺(aq) + 8e^- Ru(s) + 4H₂O(l) E° = 1.038 V FeO₄^2-(aq) + 8H⁺(aq) + 3e^- Fe³⁺(aq) + 4H₂O(l) E° = 2.07 V H₄XeO₆(aq) + 2H⁺(aq) + 2e^- XeO₃(aq) + 3H₂O(l) E° = 2.42 V

Accepted Answer

The strongest oxidizing agent is the one with the highest positive reduction potential. In this case, H₄XeO₆(aq) has the highest reduction potential of 2.42 V, making it the strongest oxidizing agent.

Question 14

Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. I₂(s) + 2e^- 2I^-(aq) E° = 0.53 V Cr³⁺(aq) + 3e^- Cr(s) E° = -0.74 V Overall reaction: 2Cr(s) + 3I₂(s) → 2Cr³⁺(aq) + (aq) + 6I^-(aq)

Accepted Answer

The answer of Calculate E°cell and indicate whether the overall...

Question 15

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)

Accepted Answer

The answer of Calculate E°_cell and indicate whether the...

Question 16

Examine the following half-reactions and select the weakest oxidizing agent among the species listed. AuBr₄(aq) + 3e^- Au(s) + 4Br^-(aq) E° = 0.854 V Mn²⁺(aq) + 2e^- Mn(s) E° = -1.185 V K⁺(aq) + e^- K(s) E° = -2.931 V F₂O(aq) + 2H⁺(aq) + 4e^- 2F^-(aq) + H₂O(l) E° = 2.153 V

Accepted Answer

The weaker the reduction potential, the stronger the oxidizing agent. Since potassium has the most negative reduction potential (-2.931V), it is the weakest oxidizing agent among the species listed.

Question 17

What is the E°_cell for the cell represented by the combination of the following half-reactions? 2Hg²⁺(aq) + 2e- Hg₂²⁺(aq) E° = 0.92 V Cr³⁺(aq) + 3e- Cr(s) E° = -0.74 V

Accepted Answer

The answer of What is the E°_cell for the cell...

Question 18

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

Accepted Answer

The answer of Examine the following half-reactions and select the...

Question 19

The line notation, Pt | H₂(g) | H⁺(aq) || Cu²⁺(aq) | Cu(s), indicates that

Accepted Answer

The answer of The line notation, Pt | H₂(g) |...

Question 20

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) + SO₄^2-(aq) E° = 0.613 V

Accepted Answer

The answer of Examine the following half-reactions and select the...

Quiz 21: Electrochemistry Chemical Change and Electrical Work

Examine the following half-reactions and select the strongest oxidizing agent among the species listed. Cr²⁺(aq) + 2e^- Cr(s) E° = -0.913 V Fe²⁺(aq) + 2e^- Fe(s) E° = -0.447 V Sr²⁺(aq) + 2e^- Sr(s) E° = -2.89 V Co²⁺(aq) + 2e^- Co(s) E° = -0.28 V

A voltaic cell has a standard cell potential equal to 0.74 V. If the standard electrode (reduction) potential for the anode is -0.22 V, what is the standard electrode potential for the cathode?

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 of the following conditions is most likely to apply to a fully-charged secondary cell?

What is the E°_cell for the cell represented by the combination of the following half-reactions? ClO₄(aq) + 8H(aq) + 8e Cl-(aq) + 4H₂O(l) E° = 1.389 V VO₂(aq) + 2H(aq) + e^- j VO(aq) + H₂O(l) E° = 0.991 V

A voltaic cell can be prepared from copper and tin. What is the E°_cell for the cell that forms from the following half-reactions? Cu²⁺(aq) + 2e- Cu(s) E° = 0.34 V Sn⁴⁺(aq) + 2e- Sn²⁺(aq) E° = 0.13 V

Calculate E°_cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. H₂O₂(aq) + 2H⁺(aq) + 2e^- 2H₂O(l) E° = 1.77 V Fe³⁺ (aq) + e^- Fe²⁺(aq) E° = 0.77 V Overall reaction: 2Fe³⁺(aq) + 2H₂O(l) → H₂O₂(aq) + 2H⁺(aq) + 2Fe²⁺(aq)

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

Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. I₂(s) + 2e^- 2I^-(aq) E° = 0.53 V Cr³⁺(aq) + 3e^- Cr(s) E° = -0.74 V Overall reaction: 2Cr(s) + 3I₂(s) → 2Cr³⁺(aq) + (aq) + 6I^-(aq)

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)

Examine the following half-reactions and select the weakest oxidizing agent among the species listed. AuBr₄(aq) + 3e^- Au(s) + 4Br^-(aq) E° = 0.854 V Mn²⁺(aq) + 2e^- Mn(s) E° = -1.185 V K⁺(aq) + e^- K(s) E° = -2.931 V F₂O(aq) + 2H⁺(aq) + 4e^- 2F^-(aq) + H₂O(l) E° = 2.153 V

What is the E°_cell for the cell represented by the combination of the following half-reactions? 2Hg²⁺(aq) + 2e- Hg₂²⁺(aq) E° = 0.92 V Cr³⁺(aq) + 3e- Cr(s) E° = -0.74 V

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

The line notation, Pt | H₂(g) | H⁺(aq) || Cu²⁺(aq) | Cu(s) , indicates that

Quiz 21: Electrochemistry Chemical Change and Electrical Work

Examine the following half-reactions and select the strongest oxidizing agent among the species listed. Cr2+(aq) + 2e- Cr(s) E° = -0.913 V Fe2+(aq) + 2e- Fe(s) E° = -0.447 V Sr2+(aq) + 2e- Sr(s) E° = -2.89 V Co2+(aq) + 2e- Co(s) E° = -0.28 V

A voltaic cell has a standard cell potential equal to 0.74 V. If the standard electrode (reduction) potential for the anode is -0.22 V, what is the standard electrode potential for the cathode?

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 of the following conditions is most likely to apply to a fully-charged secondary cell?

Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. Co3+(aq) + e- Co2+(aq) E° = 1.82 V MnO4-(aq) + 2H2O(l) + 3e- MnO2(s) + 4OH-(aq) E° = 0.59 V Overall reaction: MnO4-(aq) + 2H2O(l) + 3Co2+(aq) → MnO2(s) + 3Co3+(aq) + 4OH-(aq)

What is the E°cell for the cell represented by the combination of the following half-reactions? ClO4(aq) + 8H(aq) + 8e Cl-(aq) + 4H2O(l) E° = 1.389 V VO2(aq) + 2H(aq) + e- j VO(aq) + H2O(l) E° = 0.991 V

A voltaic cell can be prepared from copper and tin. What is the E°cell for the cell that forms from the following half-reactions? Cu2+(aq) + 2e- Cu(s) E° = 0.34 V Sn4+(aq) + 2e- Sn2+(aq) E° = 0.13 V

Calculate E° cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. H2O2(aq) + 2H+(aq) + 2e- 2H2O(l) E° = 1.77 V Fe3+ (aq) + e- Fe2+(aq) E° = 0.77 V Overall reaction: 2Fe3+(aq) + 2H2O(l) → H2O2(aq) + 2H+(aq) + 2Fe2+(aq)

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

Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. I2(s) + 2e- 2I-(aq) E° = 0.53 V Cr3+(aq) + 3e- Cr(s) E° = -0.74 V Overall reaction: 2Cr(s) + 3I2(s) → 2Cr3+(aq) + (aq) + 6I-(aq)

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)

Examine the following half-reactions and select the weakest oxidizing agent among the species listed. AuBr4(aq) + 3e- Au(s) + 4Br-(aq) E° = 0.854 V Mn2+(aq) + 2e- Mn(s) E° = -1.185 V K+(aq) + e- K(s) E° = -2.931 V F2O(aq) + 2H+(aq) + 4e- 2F-(aq) + H2O(l) E° = 2.153 V

What is the E°cell for the cell represented by the combination of the following half-reactions? 2Hg2+(aq) + 2e- Hg22+(aq) E° = 0.92 V Cr3+(aq) + 3e- Cr(s) E° = -0.74 V

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

The line notation, Pt | H2(g) | H+(aq) || Cu2+(aq) | Cu(s) , indicates that

Examine the following half-reactions and select the strongest oxidizing agent among the species listed. Cr²⁺(aq) + 2e^- Cr(s) E° = -0.913 V Fe²⁺(aq) + 2e^- Fe(s) E° = -0.447 V Sr²⁺(aq) + 2e^- Sr(s) E° = -2.89 V Co²⁺(aq) + 2e^- Co(s) E° = -0.28 V

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)

What is the E°_cell for the cell represented by the combination of the following half-reactions? ClO₄(aq) + 8H(aq) + 8e Cl-(aq) + 4H₂O(l) E° = 1.389 V VO₂(aq) + 2H(aq) + e^- j VO(aq) + H₂O(l) E° = 0.991 V

A voltaic cell can be prepared from copper and tin. What is the E°_cell for the cell that forms from the following half-reactions? Cu²⁺(aq) + 2e- Cu(s) E° = 0.34 V Sn⁴⁺(aq) + 2e- Sn²⁺(aq) E° = 0.13 V

Calculate E°_cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. H₂O₂(aq) + 2H⁺(aq) + 2e^- 2H₂O(l) E° = 1.77 V Fe³⁺ (aq) + e^- Fe²⁺(aq) E° = 0.77 V Overall reaction: 2Fe³⁺(aq) + 2H₂O(l) → H₂O₂(aq) + 2H⁺(aq) + 2Fe²⁺(aq)

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

Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. I₂(s) + 2e^- 2I^-(aq) E° = 0.53 V Cr³⁺(aq) + 3e^- Cr(s) E° = -0.74 V Overall reaction: 2Cr(s) + 3I₂(s) → 2Cr³⁺(aq) + (aq) + 6I^-(aq)

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)

Examine the following half-reactions and select the weakest oxidizing agent among the species listed. AuBr₄(aq) + 3e^- Au(s) + 4Br^-(aq) E° = 0.854 V Mn²⁺(aq) + 2e^- Mn(s) E° = -1.185 V K⁺(aq) + e^- K(s) E° = -2.931 V F₂O(aq) + 2H⁺(aq) + 4e^- 2F^-(aq) + H₂O(l) E° = 2.153 V

What is the E°_cell for the cell represented by the combination of the following half-reactions? 2Hg²⁺(aq) + 2e- Hg₂²⁺(aq) E° = 0.92 V Cr³⁺(aq) + 3e- Cr(s) E° = -0.74 V

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

The line notation, Pt | H₂(g) | H⁺(aq) || Cu²⁺(aq) | Cu(s) , indicates that