Question 1

A voltaic cell prepared using aluminum and nickel has the following cell notation. Al(s) | Al³⁺(aq) || Ni²⁺(aq) | Ni(s) Which of the following reactions occurs at the anode?

Accepted Answer

The anode is where oxidation occurs, and according to the cell notation, the anode is represented by the left-hand side of the double vertical line. In this case, the left-hand side is the aluminum electrode. The only reaction listed that involves the oxidation of aluminum (Al) is choice A, which shows aluminum oxidizing to form Al3+ ions and releasing electrons. Therefore, choice A is the correct answer.

Question 2

Which one of the following statements about electrochemical cells is correct?

Accepted Answer

In a voltaic cell, the anode is where oxidation occurs and is labeled as the negative terminal.

Question 3

A voltaic cell prepared using zinc and iodine has the following cell notation. Zn(s) | Zn²⁺(aq) || I⁻(aq) | I₂(s) | C(graphite) Which of the following equations correctly represents the balanced, spontaneous, cell reaction?

Accepted Answer

The anode is Zn(s) | Zn²⁺(aq) and the cathode is I₂(s) | I⁻(aq) | C(graphite). The half-reactions are: Anode (oxidation): Zn(s) → Zn²⁺(aq) + 2e- Cathode (reduction): I ⁻(aq) + e- → I₂(s) When we add these two half-reactions, we get the balanced overall reaction: Zn(s) + 2I ⁻(aq) → Zn²⁺(aq) + I₂(s)

Question 4

Which of the following solids is commonly used as an inactive electrode in electrochemical cells?

Accepted Answer

Graphite is commonly used as an inactive electrode in electrochemical cells because it is chemically stable and can conduct electricity. Zinc, copper, iron, and sodium are all commonly used as active electrodes in electrochemical cells.

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

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for Sn(OH)₃⁻will be Bi(OH)₃(s) + Sn(OH)₃(aq) → Sn(OH)₆²⁻(aq) + Bi(s) (basic solution)

Accepted Answer

First, we need to identify the oxidation states of each element in the equation: Bi: +3 Sn: +2 O: -2 H: +1 We then balance the equation by following these steps: 1. Balance the atoms that appear in both the half-reactions (in this case, Bi and Sn): Bi(OH)3 + Sn(OH)2 → Sn(OH)6 2- + Bi 2. Balance the number of electrons transferred in each half-reaction by multiplying one or both by coefficients: oxidation: Bi(OH)3 → Bi + 3H2O + 3e- reduction: Sn(OH)2 + 2e- → Sn(OH)6 2- 3. Combine the half-reactions by adding them together, canceling out electrons: Bi(OH)3 + Sn(OH)2 → Sn(OH)6 2- + Bi 2Bi(OH)3 + 3Sn(OH)2 → 3Sn(OH)6 2- + 2Bi At this point, all coefficients are integers, except for the coefficient of Sn(OH)2, which is 3. To make all coefficients integers, we can multiply each coefficient by 3, giving us: 6Bi(OH)3 + 9Sn(OH)2 → 9Sn(OH)6 2- + 6Bi Dividing all coefficients by 3, we end up with the balanced equation: 2Bi(OH)3 + 3Sn(OH)2 → 3Sn(OH)6 2- + 2Bi Therefore, the coefficient for Sn(OH)2 is 3, which is equivalent to a coefficient of 6 for Sn(OH)₃⁻. However, the question is asking for the coefficient of Sn(OH)₃, not Sn(OH)2, so the answer is 3.

Question 7

Which of the following statements about voltaic and electrolytic cells is correct?

Accepted Answer

In a voltaic cell, the anode undergoes oxidation and loses weight, while the cathode undergoes reduction and gains weight. In an electrolytic cell, the opposite occurs. Oxidation occurs at the anode and reduction at the cathode. The flow of electrons in a voltaic cell is from anode to cathode, while in an electrolytic cell, an external power source forces the electrons to flow from cathode to anode. The free energy change (ΔG) is negative for a voltaic cell, meaning the reaction is spontaneous and releases energy. In an electrolytic cell, an external energy source is needed to drive the non-spontaneous reaction.

Question 8

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 9

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

Accepted Answer

In the line notation, the left side represents the anode and the right side represents the cathode. The vertical line represents the boundary between the two half-cells. The notation Al(s) | Al³⁺(aq) indicates that aluminum is being oxidized and losing electrons to form Al³⁺ ions. On the other side of the vertical line, Co²⁺(aq) | Co(s) indicates that Co is being reduced and gaining electrons to form Co metal. Therefore, Al is the reducing agent and Co is the oxidizing agent. Thus, the correct answer is choice C.

Question 10

Consider the following redox equation Mn(OH)₂(s) + MnO₄(aq) → MnO₄²⁻(aq) (basic solution) When the equation is balanced with smallest whole number coefficients, what is the coefficient for OH⁻(aq) and on which side of the equation is OH⁻(aq) present?

Accepted Answer

In a basic solution, balancing involves adding OH⁻ to both sides to neutralize H⁺ ions. The balanced equation requires 6 OH⁻ ions on the reactant side to balance the charges and atoms.

Question 11

Which one of the following pairs of substances could be used to construct a single redox electrode (i.e., they have an element in common, but in different oxidation states)?

Accepted Answer

MnO and Mn can be used to construct a single redox electrode because they have the same element, manganese, but in different oxidation states (+2 for Mn and +4 for MnO). This allows for a redox reaction to occur between the two species, making them suitable for use in a redox electrode. The other pairs of substances do not have an element in common in different oxidation states, so they cannot be used to construct a single redox electrode.

Question 12

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the iodide ion will be I⁻(aq) + NO₃⁻(aq) → NO(g) + I₂(s) (acidic solution)

Accepted Answer

In acidic solution, the balanced redox equation is 6I⁻ + 2NO₃⁻ + 8H⁺ → 2NO + 3I₂ + 4H₂O, so the coefficient for I⁻ is 6.

Question 13

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for zinc will be Zn(s) + ReO₄(aq) → Re(s) + Zn²⁺(aq) (acidic solution)

Accepted Answer

The oxidation states of Zn changes from 0 to +2 and Re changes from +7 to 0. To balance the electrons lost and gained, we need to multiply the Zn half-reaction by 7, which gives us 7Zn(s) +14H+ + ReO₄(aq) → Re(s) + 7Zn²⁺(aq) + 14H2O. Thus, the coefficient for zinc is 7.

Question 14

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the hydrogen sulfate ion will be Al(s) + HSO₄(aq) + OH⁻(aq) → Al₂O₃(s) + S²⁻(aq) + H₂O(l)

Accepted Answer

The answer of When the following redox equation is balanced...

Question 15

A voltaic cell prepared using aluminum and nickel has the following cell notation. Al(s) | Al³⁺(aq) || Ni²⁺(aq) | Ni(s) Which of the following represents the correctly balanced spontaneous reaction equation for the cell?

Accepted Answer

The correct balanced reaction equation for the given cell notation can be determined by identifying the oxidation and reduction half-reactions. In this case, the aluminum electrode is the anode and undergoes oxidation while the nickel electrode is the cathode and undergoes reduction. The half-reactions are:

Al(s) → Al3+(aq) + 3e- (oxidation)
Ni2+(aq) + 2e- → Ni(s) (reduction)

Multiplying the oxidation half-reaction by 2 and the reduction half-reaction by 3 (to balance the number of electrons transferred) gives:

2Al(s) → 2Al3+(aq) + 6e-
3Ni2+(aq) + 6e- → 3Ni(s)

Adding these two half-reactions together gives the overall reaction:

3Ni2+(aq) + 2Al(s) → 2Al3+(aq) + 3Ni(s)

which corresponds to choice B.

Question 16

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for nitrogen dioxide will be __________. I₂(s) + HNO₃(aq) → HIO₃(aq) + NO₂(g) + H₂O(l)

Accepted Answer

The answer of When the following redox equation is balanced...

Question 17

Consider the following balanced redox reaction 3CuO(s) + 2NH₃(aq) → N₂(g) + 3H₂O(l) + 3Cu(s) Which of the following statements is true?

Accepted Answer

CuO acts as the oxidizing agent because it gains electrons to form Cu(s), indicating that copper is reduced from Cu(II) to Cu(0).

Question 18

Which component of the following cell notation is the anode? P | Q || R | S

Accepted Answer

In cell notation, the anode is always written on the left side. The anode is where oxidation occurs, and in this notation, P represents the anode.

Question 19

Which of the following statements about voltaic and electrolytic cells is correct?

Accepted Answer

In a voltaic (or galvanic) cell, the cathode is positive because it is where reduction occurs and thus attracts cations from the solution, which donate electrons. In an electrolytic cell, the cathode is negative because it is connected to the negative terminal of an external power source, which drives the non-spontaneous reaction by forcing electrons into the cathode.

Question 20

A voltaic cell is prepared using copper and silver. Its cell notation is shown below. Cu(s) | Cu²⁺(aq) || Ag⁺(aq) | Ag(s) Which of the following processes occurs at the cathode?

Accepted Answer

The cathode is where reduction occurs, so we need to look for the half-reaction that involves the gain of electrons. Option D shows the reduction of silver ions to silver metal by gaining one electron, which matches the process occurring at the cathode in this cell.

Quiz 21: Electrochemistry: Chemical Change and Electrical Work

A voltaic cell prepared using aluminum and nickel has the following cell notation. Al(s) | Al³⁺(aq) || Ni²⁺(aq) | Ni(s) Which of the following reactions occurs at the anode?

Which one of the following statements about electrochemical cells is correct?

A voltaic cell prepared using zinc and iodine has the following cell notation. Zn(s) | Zn²⁺(aq) || I⁻(aq) | I₂(s) | C(graphite) Which of the following equations correctly represents the balanced, spontaneous, cell reaction?

Which of the following solids is commonly used as an inactive electrode in electrochemical cells?

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

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for Sn(OH) ₃⁻will be Bi(OH) ₃(s) + Sn(OH) ₃(aq) → Sn(OH) ₆²⁻(aq) + Bi(s) (basic solution)

Which of the following statements about voltaic and electrolytic cells is correct?

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

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

Consider the following redox equation Mn(OH) ₂(s) + MnO₄(aq) → MnO₄²⁻(aq) (basic solution) When the equation is balanced with smallest whole number coefficients, what is the coefficient for OH⁻(aq) and on which side of the equation is OH⁻(aq) present?

Which one of the following pairs of substances could be used to construct a single redox electrode (i.e., they have an element in common, but in different oxidation states) ?

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the iodide ion will be I⁻(aq) + NO₃⁻(aq) → NO(g) + I₂(s) (acidic solution)

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for zinc will be Zn(s) + ReO₄(aq) → Re(s) + Zn²⁺(aq) (acidic solution)

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the hydrogen sulfate ion will be Al(s) + HSO₄(aq) + OH⁻(aq) → Al₂O₃(s) + S²⁻(aq) + H₂O(l)

A voltaic cell prepared using aluminum and nickel has the following cell notation. Al(s) | Al³⁺(aq) || Ni²⁺(aq) | Ni(s) Which of the following represents the correctly balanced spontaneous reaction equation for the cell?

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for nitrogen dioxide will be __________. I₂(s) + HNO₃(aq) → HIO₃(aq) + NO₂(g) + H₂O(l)

Consider the following balanced redox reaction 3CuO(s) + 2NH₃(aq) → N₂(g) + 3H₂O(l) + 3Cu(s) Which of the following statements is true?

Which component of the following cell notation is the anode? P | Q || R | S

Which of the following statements about voltaic and electrolytic cells is correct?

A voltaic cell is prepared using copper and silver. Its cell notation is shown below. Cu(s) | Cu²⁺(aq) || Ag⁺(aq) | Ag(s) Which of the following processes occurs at the cathode?

Quiz 21: Electrochemistry: Chemical Change and Electrical Work

A voltaic cell prepared using aluminum and nickel has the following cell notation. Al(s) | Al3+(aq) || Ni2+(aq) | Ni(s) Which of the following reactions occurs at the anode?

Which one of the following statements about electrochemical cells is correct?

A voltaic cell prepared using zinc and iodine has the following cell notation. Zn(s) | Zn2+(aq) || I−(aq) | I2(s) | C(graphite) Which of the following equations correctly represents the balanced, spontaneous, cell reaction?

Which of the following solids is commonly used as an inactive electrode in electrochemical cells?

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

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for Sn(OH) 3− will be Bi(OH) 3(s) + Sn(OH) 3(aq) → Sn(OH) 62−(aq) + Bi(s) (basic solution)

Which of the following statements about voltaic and electrolytic cells is correct?

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

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

Consider the following redox equation Mn(OH) 2(s) + MnO4(aq) → MnO42−(aq) (basic solution) When the equation is balanced with smallest whole number coefficients, what is the coefficient for OH−(aq) and on which side of the equation is OH−(aq) present?

Which one of the following pairs of substances could be used to construct a single redox electrode (i.e., they have an element in common, but in different oxidation states) ?

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the iodide ion will be I−(aq) + NO3−(aq) → NO(g) + I2(s) (acidic solution)

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for zinc will be Zn(s) + ReO4(aq) → Re(s) + Zn2+(aq) (acidic solution)

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the hydrogen sulfate ion will be Al(s) + HSO4(aq) + OH−(aq) → Al2O3(s) + S2−(aq) + H2O(l)

A voltaic cell prepared using aluminum and nickel has the following cell notation. Al(s) | Al3+(aq) || Ni2+(aq) | Ni(s) Which of the following represents the correctly balanced spontaneous reaction equation for the cell?

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for nitrogen dioxide will be __________. I2(s) + HNO3(aq) → HIO3(aq) + NO2(g) + H2O(l)

Consider the following balanced redox reaction 3CuO(s) + 2NH3(aq) → N2(g) + 3H2O(l) + 3Cu(s) Which of the following statements is true?

Which component of the following cell notation is the anode? P | Q || R | S

Which of the following statements about voltaic and electrolytic cells is correct?

A voltaic cell is prepared using copper and silver. Its cell notation is shown below. Cu(s) | Cu2+(aq) || Ag+(aq) | Ag(s) Which of the following processes occurs at the cathode?

A voltaic cell prepared using aluminum and nickel has the following cell notation. Al(s) | Al³⁺(aq) || Ni²⁺(aq) | Ni(s) Which of the following reactions occurs at the anode?

A voltaic cell prepared using zinc and iodine has the following cell notation. Zn(s) | Zn²⁺(aq) || I⁻(aq) | I₂(s) | C(graphite) Which of the following equations correctly represents the balanced, spontaneous, cell reaction?

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

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for Sn(OH) ₃⁻will be Bi(OH) ₃(s) + Sn(OH) ₃(aq) → Sn(OH) ₆²⁻(aq) + Bi(s) (basic solution)

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

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

Consider the following redox equation Mn(OH) ₂(s) + MnO₄(aq) → MnO₄²⁻(aq) (basic solution) When the equation is balanced with smallest whole number coefficients, what is the coefficient for OH⁻(aq) and on which side of the equation is OH⁻(aq) present?

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the iodide ion will be I⁻(aq) + NO₃⁻(aq) → NO(g) + I₂(s) (acidic solution)

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for zinc will be Zn(s) + ReO₄(aq) → Re(s) + Zn²⁺(aq) (acidic solution)

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the hydrogen sulfate ion will be Al(s) + HSO₄(aq) + OH⁻(aq) → Al₂O₃(s) + S²⁻(aq) + H₂O(l)

A voltaic cell prepared using aluminum and nickel has the following cell notation. Al(s) | Al³⁺(aq) || Ni²⁺(aq) | Ni(s) Which of the following represents the correctly balanced spontaneous reaction equation for the cell?

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for nitrogen dioxide will be __________. I₂(s) + HNO₃(aq) → HIO₃(aq) + NO₂(g) + H₂O(l)

Consider the following balanced redox reaction 3CuO(s) + 2NH₃(aq) → N₂(g) + 3H₂O(l) + 3Cu(s) Which of the following statements is true?

A voltaic cell is prepared using copper and silver. Its cell notation is shown below. Cu(s) | Cu²⁺(aq) || Ag⁺(aq) | Ag(s) Which of the following processes occurs at the cathode?