Question 1

Examine the following half-reactions and select the strongest oxidizing agent among the species listed.

Accepted Answer

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

Question 2

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) $\to$ Cu(s) + Co²⁺(aq)

Accepted Answer

E°cell = E°cathode - E°anode
0.62 V = 0.34 V - E°anode
E°anode = -0.28 V

Question 3

What is the value of the equilibrium constant for the cell reaction below at 25°C? E°_cell = 0.30 V Sn²⁺(aq) + Fe(s) Sn(s) + Fe²⁺(aq)

Accepted Answer

The answer of What is the value of the equilibrium...

Question 4

Examine the following half-reactions and select the strongest oxidizing agent among the substances.

Accepted Answer

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

Question 5

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 6

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 7

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 8

A battery is considered "dead" when

Accepted Answer

The answer of A battery is considered "dead" when
...

Question 9

A 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 cell can be prepared from copper...

Question 10

What is the E°_cell for the cell represented by the combination of the following half-reactions?

Accepted Answer

First, we need to write the overall reaction by balancing the number of electrons transferred: 2Fe2+(aq) + Cl2(g) → 2Fe3+(aq) + 2Cl−(aq) Next, we can find the standard reduction potentials (E°) for each half-reaction using a reference table. Fe3+(aq) + e− → Fe2+(aq) E° = 0.77 V Cl2(g) + 2e− → 2Cl−(aq) E° = 1.36 V Then, we can calculate the overall standard potential using the formula: E°cell = E°reduction (cathode) - E°reduction (anode) E°cell = 0.77 V - 1.36 V = -0.59 V Since the given half-reaction is the reduction potential for Fe2+ to Fe3+, we need to flip the sign to get the oxidation potential for Fe3+ to Fe2+. E°_cell = -E°Fe2+/Fe3+ = 0.59 V However, the question is asking for the absolute value of E°_cell, which is 0.59 V. Therefore, the correct answer is D) 1.66 V (absolute value of -0.59 V).

Question 11

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^- VO⁺(aq) + H₂O(l) E°= 0.991 V

Accepted Answer

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

Question 12

Calculate E^°_cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. reaction: 2Cr(s) + 3I₂(s) $\to$ 2Cr³⁺(aq) + (aq) + 6I^-(aq)

Accepted Answer

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

Question 13

Examine the following half-reactions and select the weakest oxidizing agent among the species listed.

Accepted Answer

In order for a species to be a good oxidizing agent, it must have a high tendency to gain electrons (i.e. be reduced). The half-reaction for potassium (K) in option C is K+ + e- → K, which has a reduction potential of -2.92 V. This is the least favorable reduction potential, meaning that potassium has the lowest tendency to gain electrons and therefore is the weakest oxidizing agent.

Question 14

Calculate E°_cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. Overall reaction: 4Al(s) + 3O₂(g) + 12H⁺(aq) $\to$ 4Al³⁺(aq) + 6H₂O(l)

Accepted Answer

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

Question 15

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

Since no reaction occurs between metal A and C²⁺, it is unlikely that a reaction between metal B and C²⁺ would occur. Therefore, Choice C would not occur spontaneously.

Question 16

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) $\to$ 2HSO₄^-(aq) + I₂(aq)

Accepted Answer

The answer of The redox reaction of peroxydisulfate with iodide...

Question 17

Examine the following half-reactions and select the strongest reducing agent among the species listed.

Accepted Answer

The strongest reducing agent will have the highest potential to lose electrons and be oxidized. This means that we need to look for the half-reaction with the most negative reduction potential. From the given options, we can see that the reduction potential of the Zn2+(aq) + 2e- --> Zn(s) half-reaction is the most negative at -0.76 V. Therefore, Zn(s) is the strongest reducing agent among the species listed.

Question 18

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

Accepted Answer

In a galvanic cell, the anode undergoes oxidation and the cathode undergoes reduction. The line notation shows that Al is on the left-hand side of the double vertical line, indicating it is the anode and undergoing oxidation. The presence of the (aq) notation after the Co²⁺ ions indicates that they are in solution and being reduced at the cathode (Co). Therefore, Al is the reducing agent and Choice C is correct.

Question 19

Calculate the potential of a voltaic cell (E°_cell) if it is required to do 5.43 × 10^-3 kJ of work when a charge of 2.50 C is transferred.

Accepted Answer

The answer of Calculate the potential of a voltaic cell...

Question 20

Given that E° for X + e^- F$\to$ Y is greater than E° for A + 2e^- $\to$ B, it is correct to say that, under standard conditions

Accepted Answer

The answer of Given that E° for X + e^-...

Quiz 21: Electrochemistry: Chemical Change and Electrical Work

Examine the following half-reactions and select the strongest oxidizing agent among the species listed.

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) $\to$ Cu(s) + Co²⁺(aq)

What is the value of the equilibrium constant for the cell reaction below at 25°C? E°_cell = 0.30 V Sn²⁺(aq) + Fe(s) Sn(s) + Fe²⁺(aq)

Examine the following half-reactions and select the strongest oxidizing agent among the substances.

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

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

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?

A battery is considered "dead" when

A 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

What is the E°_cell for the cell represented by the combination of the following half-reactions?

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^- VO⁺(aq) + H₂O(l) E°= 0.991 V

Examine the following half-reactions and select the weakest oxidizing agent among the species listed.

Examine the following half-reactions and select the strongest reducing agent among the species listed.

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

Calculate the potential of a voltaic cell (E°_cell) if it is required to do 5.43 × 10^-3 kJ of work when a charge of 2.50 C is transferred.

Given that E° for X + e^- F $\to$ Y is greater than E° for A + 2e^- $\to$ B, it is correct to say that, under standard conditions

Quiz 21: Electrochemistry: Chemical Change and Electrical Work

Examine the following half-reactions and select the strongest oxidizing agent among the species listed.

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) →\to→ Cu(s) + Co2+(aq)

What is the value of the equilibrium constant for the cell reaction below at 25°C? E°cell = 0.30 V Sn2+(aq) + Fe(s) Sn(s) + Fe2+(aq)

Examine the following half-reactions and select the strongest oxidizing agent among the substances.

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

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

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?

A battery is considered "dead" when

A 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

What is the E°cell for the cell represented by the combination of the following half-reactions?

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- VO+(aq) + H2O(l) E° = 0.991 V

Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. reaction: 2Cr(s) + 3I2(s) →\to→ 2Cr3+(aq) + (aq) + 6I-(aq)

Examine the following half-reactions and select the weakest oxidizing agent among the species listed.

Calculate E°cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. Overall reaction: 4Al(s) + 3O2(g) + 12H+(aq) →\to→ 4Al3+(aq) + 6H2O(l)

Examine the following half-reactions and select the strongest reducing agent among the species listed.

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

Calculate the potential of a voltaic cell (E°cell) if it is required to do 5.43 × 10-3 kJ of work when a charge of 2.50 C is transferred.

Given that E° for X + e- F →\to→ Y is greater than E° for A + 2e- →\to→ B, it is correct to say that, under standard conditions

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) $\to$ Cu(s) + Co²⁺(aq)

What is the value of the equilibrium constant for the cell reaction below at 25°C? E°_cell = 0.30 V Sn²⁺(aq) + Fe(s) Sn(s) + Fe²⁺(aq)

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

A 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

What is the E°_cell for the cell represented by the combination of the following half-reactions?

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^- VO⁺(aq) + H₂O(l) E°= 0.991 V

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

Calculate the potential of a voltaic cell (E°_cell) if it is required to do 5.43 × 10^-3 kJ of work when a charge of 2.50 C is transferred.

Given that E° for X + e^- F $\to$ Y is greater than E° for A + 2e^- $\to$ B, it is correct to say that, under standard conditions