Question 1

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 2

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

Accepted Answer

In a voltaic cell, the cathode is positive because it is where reduction occurs and electrons flow towards it. In an electrolytic cell, the cathode is negative because it is connected to the negative terminal of the power source, forcing electrons onto it for reduction.

Question 3

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the iodide ion will be _____. I^-(aq) + NO₃^-(aq) $\to$ NO(g) + I₂(s) (acidic solution)

Accepted Answer

In acidic solution, the balanced redox reaction is: 6 I^- + 2 NO₃^- + 4 H⁺ → 2 NO + 3 I₂ + 2 H₂O. The coefficient for the iodide ion is 6.

Question 4

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

Accepted Answer

CuO(s) is the oxidizing agent and copper is reduced.

Question 5

Consider the following balanced redox reaction Mn²⁺(aq) + S₂O₈^2-(aq) + 2H₂O(l) $\to$ MnO₂(s) + 4H⁺(aq) + 2SO₄^2-(aq) Which of the following statements is true?

Accepted Answer

Mn²⁺(aq) is the reducing agent and is oxidized to MnO₂(s), increasing its oxidation state from +2 to +4.

Question 6

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for zinc will be _____. Zn(s) + ReO₄^-(aq) $\to$ Re(s) + Zn²⁺(aq) (acidic solution)

Accepted Answer

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

Question 7

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) $\to$ Al₂O₃(s) + S^2-(aq) + H₂O(l)

Accepted Answer

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

Question 8

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

Accepted Answer

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

Question 9

Consider the reaction CuO(s) + H₂(g) $\to$ Cu(s) + H₂O(l) In this reaction, which substances are the oxidant and reductant, respectively?

Accepted Answer

CuO is the oxidant because it gains electrons (is reduced) to form Cu, and H₂ is the reductant because it loses electrons (is oxidized) to form H₂O.

Question 10

Consider the following redox equation Mn(OH)₂(s) + MnO₄^-(aq) $\to$ MnO₄^2-(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, OH⁻ ions are added to balance the charge and mass. The balanced equation requires 6 OH⁻ ions on the reactant side to balance the oxygen and hydrogen atoms.

Question 11

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 answer of A voltaic cell prepared using zinc and...

Question 12

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 13

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 balanced equation for the spontaneous reaction in the voltaic cell is 3Ni²⁺(aq) + 2Al(s) → 2Al³⁺(aq) + 3Ni(s), which correctly balances the charges and atoms.

Question 14

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

Accepted Answer

The free energy change, ΔG, is negative for a voltaic cell as it releases energy, whereas ΔG is positive for an electrolytic cell as energy is required to drive the non-spontaneous reaction. Statement A is incorrect as the anode will lose weight in a voltaic cell due to oxidation. Statement B is incorrect as oxidation occurs at the anode and reduction occurs at the cathode for both cells. Statement D is incorrect as in an electrolytic cell, the electrons in the external wire flow from anode to cathode. Therefore, the only correct statement is C.

Question 15

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. In this case, silver ions (Ag⁺) are being reduced to Ag(s), so the correct choice is D, where Ag(s) is produced at the cathode.

Question 16

Which one of the following is not a redox reaction?

Accepted Answer

The answer of Which one of the following is not...

Question 17

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 a good conductor of electricity and is chemically inert. Zinc, copper, iron and sodium are all active metals that can be used as active electrodes in electrochemical cells.

Question 18

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 19

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, meaning that electrons are lost. Looking at the cell notation, the anode is on the left side, where aluminum is listed first. The half-reactions listed for A and B both involve aluminum, but A is the correct choice because it shows aluminum losing electrons and forming ions in solution.

Question 20

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) $\to$ Sn(OH)₆^2-(aq) + Bi(s) (basic solution)

Accepted Answer

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

Quiz 21: Electrochemistry: Chemical Change and Electrical Work

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?

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the iodide ion will be _____. I^-(aq) + NO₃^-(aq) $\to$ NO(g) + I₂(s) (acidic solution)

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

Consider the following balanced redox reaction Mn²⁺(aq) + S₂O₈^2-(aq) + 2H₂O(l) $\to$ MnO₂(s) + 4H⁺(aq) + 2SO₄^2-(aq) Which of the following statements is true?

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for zinc will be _____. Zn(s) + ReO₄^-(aq) $\to$ 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) $\to$ Al₂O₃(s) + S^2-(aq) + H₂O(l)

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

Consider the reaction CuO(s) + H₂(g) $\to$ Cu(s) + H₂O(l) In this reaction, which substances are the oxidant and reductant, respectively?

Consider the following redox equation Mn(OH) ₂(s) + MnO₄^-(aq) $\to$ MnO₄^2-(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?

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 one of the following statements about electrochemical cells is correct?

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?

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?

Which one of the following is not a redox reaction?

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

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) ?

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?

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) $\to$ Sn(OH) ₆^2-(aq) + Bi(s) (basic solution)

Quiz 21: Electrochemistry: Chemical Change and Electrical Work

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?

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

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

Consider the following balanced redox reaction Mn2+(aq) + S2O82-(aq) + 2H2O(l) →\to→ MnO2(s) + 4H+(aq) + 2SO42-(aq) Which of the following statements is true?

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for zinc will be _____. Zn(s) + ReO4-(aq) →\to→ 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) →\to→ Al2O3(s) + S2-(aq) + H2O(l)

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

Consider the reaction CuO(s) + H2(g) →\to→ Cu(s) + H2O(l) In this reaction, which substances are the oxidant and reductant, respectively?

Consider the following redox equation Mn(OH) 2(s) + MnO4-(aq) →\to→ 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?

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 one of the following statements about electrochemical cells is correct?

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?

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?

Which one of the following is not a redox reaction?

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

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) ?

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?

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) →\to→ Sn(OH) 62-(aq) + Bi(s) (basic solution)

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for the iodide ion will be _____. I^-(aq) + NO₃^-(aq) $\to$ NO(g) + I₂(s) (acidic solution)

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

Consider the following balanced redox reaction Mn²⁺(aq) + S₂O₈^2-(aq) + 2H₂O(l) $\to$ MnO₂(s) + 4H⁺(aq) + 2SO₄^2-(aq) Which of the following statements is true?

When the following redox equation is balanced with smallest whole number coefficients, the coefficient for zinc will be _____. Zn(s) + ReO₄^-(aq) $\to$ 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) $\to$ Al₂O₃(s) + S^2-(aq) + H₂O(l)

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

Consider the reaction CuO(s) + H₂(g) $\to$ Cu(s) + H₂O(l) In this reaction, which substances are the oxidant and reductant, respectively?

Consider the following redox equation Mn(OH) ₂(s) + MnO₄^-(aq) $\to$ MnO₄^2-(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?

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?

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?

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?

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) $\to$ Sn(OH) ₆^2-(aq) + Bi(s) (basic solution)