Question 1

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

Accepted Answer

To find the cell potential, we need to first identify the oxidation and reduction half-reactions. In this case, we have:

Oxidation half-reaction: EF1F1F1S1 -> EF1F1F10S1U1B1 + 1e-
Reduction half-reaction: EF1F1F1S1 + 2H+ + 2e- -> TB7799 (no need to include the 00)

Next, we need to determine the standard reduction potentials (E°) for each half-reaction. These values can be found in a standard reduction potential table. Using the NIST Chemistry WebBook, we find:

EF1F1F1S1 + H+ + e- -> EF1F1F1S1U1B1        E° = -0.575 V
EF1F1F1S1 + 2H+ + 2e- -> TB7799                  E° = -0.403 V

The next step is to calculate the cell potential (Ecell) using the formula:

Ecell = E°(reduction) - E°(oxidation)

Ecell = E°(TB7799) - E°(EF1F1F1S1 + H+ + e-)
Ecell = (-0.403 V) - (-0.575 V)
Ecell = 0.172 V

However, we need to take into account the stoichiometry of the half-reactions. The reduction half-reaction involves the transfer of 2 electrons, while the oxidation half-reaction involves the transfer of only 1 electron. To balance the electrons, we can multiply the oxidation half-reaction by 2:

2EF1F1F1S1 -> 2EF1F1F10S1U1B1 + 2e-

Now the number of electrons transferred is the same in both half-reactions. In the equation for Ecell, we also need to multiply E°(oxidation) by 2:

Ecell = E°(reduction) - 2 × E°(oxidation)

Ecell = (-0.403 V) - 2 × (-0.575 V)
Ecell = 1.666 V (rounded to three significant figures)

Therefore, the answer is D) 1.66 V.

Question 2

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

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

A cell can be prepared from copper and tin. What is the E$\degree$_cell for the cell that forms from the following half-reactions?

Accepted Answer

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

Question 5

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

Accepted Answer

The strongest oxidizing agent is the one that undergoes reduction the most easily. In this case, we need to look for the half-reaction with the highest reduction potential (E0) value. According to the standard reduction potential table, the half-reaction H₄XeO₆(aq) has the highest reduction potential value, making it the strongest oxidizing agent.

Question 6

The voltaic cell made up of cobalt, copper and their M²⁺ ions, has E $\degree$_cell = 0.62 V. If E $\degree$ of the cathode half-cell is 0.34 V, what is E $\degree$ of the anode half-cell? Cu²⁺(aq) + Co(s) $\rightarrow$ Cu(s) + Co²⁺(aq)

Accepted Answer

The given voltaic cell can be represented as follows:

Cu(s) | Cu2+(aq) || Co2+(aq) | Co(s)

where the anode half-cell is Co2+(aq) | Co(s) and the cathode half-cell is Cu2+(aq) | Cu(s).

Using the given EF1F1F1S1F1F1F10 value of the cell, we can write:

EF1F1F1S1F1F1F10 = EF1F1F1S1F1F1F10(cathode) - EF1F1F1S1F1F1F10(anode)

0.62 V = 0.34 V - EF1F1F1S1F1F1F10(anode)

EF1F1F1S1F1F1F10(anode) = -0.28 V

Therefore, the answer is A) -0.28 V.

Question 7

Calculate E$\degree$_cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. Overall reaction:

Accepted Answer

The answer of Calculate E$\degree$_cell and indicate whether the overall...

Question 8

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 9

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

Accepted Answer

In the given notation, the vertical line indicates the boundary between the two half-cells, where the left side represents the anode (oxidation) and the right side represents the cathode (reduction). The anode releases electrons and oxidizes, while the cathode accepts electrons and reduces. In this case, aluminum is on the left side and Co is on the right side, indicating that aluminum is being oxidized and Co is being reduced. Therefore, Aluminum is the reducing agent (gives up electrons) and Co is the oxidizing agent (receives electrons). Choice A and B are incorrect as Co is the oxidizing agent, not the reducing agent, and Co²⁺ ions are being reduced, not oxidized. Similarly, Choice D is incorrect as Al³⁺ is not the reducing agent; instead, it is being oxidized as it releases electrons. Choice E is also incorrect as the notation does not provide information about which metal is the cathode; it only indicates the ion present in the cathode compartment.

Question 10

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

Accepted Answer

The answer of What is the E$\degree$_cell for the cell...

Question 11

Examine the following half-reactions and select the weakest reducing agent among the substances.

Accepted Answer

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

Question 12

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

Accepted Answer

A stronger reducing agent has a greater tendency to lose electrons and get oxidized. Among the given half-reactions, Zn(s) has the most negative standard reduction potential, indicating a greater tendency to lose electrons and get oxidized. Therefore, Zn(s) is the strongest reducing agent.

Question 13

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$\degree$_cell = 1.587 V and E$\degree$of the cathode half-cell is 0.536 V, what is E$\degree$ of the anode half-cell?

Accepted Answer

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

Question 14

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 15

Calculate E$\degree$_cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. Overall reaction:

Accepted Answer

We need to calculate the cell potential from the given standard reduction potentials:
EF1F1F1S1 + e- → EF1F1F1S1F1F1F10------------------ E°= +0.77 V
S1O22- + H2O + 2e- → 2OH- + SO42- --------------- E°= +0.20 V

Now, we write the overall equation by reversing the oxidation reaction:
EF1F1F1S1 + S1O22- + 2H2O → EF1F1F1S1F1F1F10 + 2OH- + SO42-

We can then add the individual E° values to determine the overall cell potential:
EF1F1F1S1 + S1O22- + 2H2O → EF1F1F1S1F1F1F10 + 2OH- + SO42-
E°cell = E°cathode - E°anode
E°cell = (+0.20 V) - (+0.77 V)
E°cell = -0.57 V

Since the calculated E°cell is negative, the overall reaction is non-spontaneous. Therefore, option A is the correct answer.

Question 16

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

Accepted Answer

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

Question 17

Calculate E$\degree$_cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. Overall reaction:

Accepted Answer

The answer of Calculate E$\degree$_cell and indicate whether the overall...

Question 18

Calculate E $\degree$_cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. Overall reaction: 2Cr(s) + 3I₂(s) $\rightarrow$ 2Cr³⁺(aq) + (aq) + 6I¯(aq)

Accepted Answer

The answer of Calculate E $\degree$_cell and indicate whether the...

Question 19

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

This choice involves the placement of metal B in a solution of metal ions C²⁺, which according to the given information, does not result in a reaction. Thus, the reaction in choice C would not occur spontaneously.

Question 20

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...

Quiz 21: Electrochemistry: Chemical Change and Electrical Work

What is the E $\degree$ _cell for the cell represented by the combination of the following half-reactions? $What is the E \degree <sub>cell</sub> for the cell represented by the combination of the following half-reactions? A) -0.18 V B) 0.18 V C) 1.28 V D) 1.66 V E) 2.12 V$

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

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?

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

The voltaic cell made up of cobalt, copper and their M²⁺ ions, has E $\degree$ _cell = 0.62 V. If E $\degree$ of the cathode half-cell is 0.34 V, what is E $\degree$ of the anode half-cell? Cu²⁺(aq) + Co(s) $\rightarrow$ Cu(s) + Co²⁺(aq)

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

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

Examine the following half-reactions and select the weakest reducing agent among the substances.

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

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

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

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

Quiz 21: Electrochemistry: Chemical Change and Electrical Work

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

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

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 cell can be prepared from copper and tin. What is the E °\degree° cell for the cell that forms from the following half-reactions?

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

The voltaic cell made up of cobalt, copper and their M2+ ions, has E °\degree° cell = 0.62 V. If E °\degree° of the cathode half-cell is 0.34 V, what is E °\degree° of the anode half-cell? Cu2+(aq) + Co(s) →\rightarrow→ Cu(s) + Co2+(aq)

Calculate E °\degree° cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. Overall reaction:

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

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

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

Examine the following half-reactions and select the weakest reducing agent among the substances.

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

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 °\degree° cell = 1.587 V and E °\degree° of the cathode half-cell is 0.536 V, what is E °\degree° of the anode half-cell?

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

Calculate E °\degree° cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. Overall reaction:

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

Calculate E °\degree° cell and indicate whether the overall reaction shown is spontaneous or nonspontaneous. Overall reaction:

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

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

What is the E $\degree$ _cell for the cell represented by the combination of the following half-reactions? $What is the E \degree <sub>cell</sub> for the cell represented by the combination of the following half-reactions? A) -0.18 V B) 0.18 V C) 1.28 V D) 1.66 V E) 2.12 V$

The voltaic cell made up of cobalt, copper and their M²⁺ ions, has E $\degree$ _cell = 0.62 V. If E $\degree$ of the cathode half-cell is 0.34 V, what is E $\degree$ of the anode half-cell? Cu²⁺(aq) + Co(s) $\rightarrow$ Cu(s) + Co²⁺(aq)

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

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