Deck 17: Electrochemistry

Question 1

What is the name given to the experimental apparatus for generating electricity through the use of a spontaneous reaction?

A)Electrolytic cell
B)Galvanic cell
C)Redox cell
D)Cathode
E)Anode

Answer 1

Galvanic cell

Question 2

Which is not a redox reaction?

A)Al(OH)₄⁻(aq) + 4H⁺(aq) → Al³⁺(aq) + 4H₂O(l)
B)C₆H₁₂O₆(s) + 6O₂(g) → 6CO₂(g) + 6H₂O(l)
C)Na₆FeCl₈(s) + 2Na(l) → 8NaCl(s) + Fe(s)
D)2H₂O₂(aq) → 2H₂O(l) + O₂(g)
E)CO₂(g) + H₂(g) → CO(g) + H₂O(g)

Answer 2

Al(OH)₄⁻(aq) + 4H⁺(aq) → Al³⁺(aq) + 4H₂O(l)

Question 3

If a substance is reduced, it must undergo a

A)gain of electrons.
B)loss of oxygen.
C)gain of hydrogen.
D)loss of electrons.
E)gain of oxygen.

Answer 3

gain of electrons.

Question 4

Complete and balance the following redox equation.Now sum the coefficients of all species in the balanced equation.(Remember to add the coefficients that are equal to one, and to add the coefficients of any species added to the equation.) The sum of the smallest whole number coefficients is Bi(OH)₃ + SnO₂²⁻ → Bi + SnO₃²⁻ (basic solution)

A)32
B)25
C)16
D)13
E)4

Question 5

When the following redox equation is balanced with the smallest whole number coefficients, what is the coefficient of Zn(s)? Zn(s) + ReO₄⁻(aq) → Re(s) + Zn²⁺(aq) (acidic solution)

A)2
B)7
C)8
D)16
E)None of these choices is correct.

Question 6

When the following redox equation is balanced using the smallest whole-number coefficients, what is the coefficient of NO₂? Sn + HNO₃ → SnO₂ + NO₂ + H₂O (acidic solution)

A)1
B)2
C)3
D)4
E)5

Question 7

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

A)1
B)2
C)4
D)5
E)10

Question 8

When the following redox equation is balanced with the smallest whole number coefficients, what is the coefficient of Sn(OH)₃⁻? Bi(OH)₃(s) + Sn(OH)₃^-(aq) → Sn(OH)₆²⁻(aq) + Bi(s) (basic solution)

A)1
B)2
C)3
D)6
E)12

Question 9

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

A)Mn²⁺(aq) is the oxidizing agent and is reduced.
B)Mn²⁺(aq) is the oxidizing agent and is oxidized.
C)Mn²⁺(aq) is the reducing agent and is oxidized.
D)Mn²⁺(aq) is the reducing agent and is reduced.
E)Manganese does not change its oxidation number in this reaction.

Question 10

Complete and balance the following redox equation.When properly balanced using the smallest whole-number coefficients, the coefficient of S is H₂S + HNO₃ → S + NO + H₂O (acidic solution)

A)1.
B)2.
C)3.
D)5.
E)6.

Question 11

When the following redox equation is balanced with the 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)1
B)3
C)4
D)6
E)8

Question 12

When the following equation is balanced with the lowest whole number coefficients, the coefficients are:Cu(s) + H⁺(aq) + NO₃⁻(aq) → NO(g) + H₂O(l) + Cu²⁺(aq)

A)1, 2, 1, 1, 1, 1
B)3, 2, 1, 1, 1, 3
C)3, 2, 4, 2, 4, 3
D)1, 8, 2, 2, 4, 1
E)3, 8, 2, 2, 4, 3

Question 13

When the following redox equation is balanced with the smallest whole number coefficients, what is the coefficient of Sb³⁺(aq)? BrO₃⁻(aq) + Sb³⁺(aq) → Br⁻(aq) + Sb⁵⁺(aq) (acidic solution)

A)1
B)2
C)3
D)4
E)6

Question 14

Consider the reaction CuO(s) + H₂(g) → Cu(s) + H₂O(l)
In this reaction, which substances are the oxidizing agent and reducing agent, respectively?

A)CuO and H₂
B)H₂ and CuO
C)CuO and Cu
D)H₂O and H₂
E)Cu and H₂O

Question 15

What is the oxidizing agent in the (unbalanced) reaction? Cu(s) + H⁺(aq) + NO₃⁻(aq) → NO(g) + H₂O(l) + Cu²⁺(aq)

A)Cu
B)H⁺
C)NO₃⁻
D)NO
E)Cu²⁺

Question 16

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

A)CuO(s) is the oxidizing agent and copper is reduced.
B)CuO(s) is the oxidizing agent and copper is oxidized.
C)CuO(s) is the reducing agent and copper is oxidized.
D)CuO(s) is the reducing agent and copper is reduced.
E)CuO(s) is the oxidizing agent and N₂(g) is the reducing agent.

Question 17

Complete and balance the following redox equation using the set of smallest whole numbers coefficients.What is the sum of the coefficients? HI + HNO₃ → I₂ + NO (acidic solution)

A)5
B)7
C)14
D)17
E)None of these choices is correct.

Question 18

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

A)4, reactant side
B)4, product side
C)6, reactant side
D)6, product side
E)8, reactant side

Question 19

A certain electrochemical cell has for its cell reaction: Zn + HgO → ZnO + Hg
Which is the half-reaction occurring at the anode?

A)HgO + 2e⁻ → Hg + O²⁻
B)Zn²⁺+ 2e⁻ → Zn
C)Zn → Zn²⁺ + 2e⁻
D)ZnO + 2e⁻ → Zn

Question 20

What is the purpose of a salt bridge in an electrochemical cell?

A)A salt bridge provides electrical contact between the electrodes that make up the cell.
B)A salt bridge carries electrons between the cathode and anode.
C)A salt bridge insulates the two electrodes.
D)A salt bridge allows the electrolyte solution to siphon from one side of the cell to the other so the levels remain
Equal.
E)A salt bridge allows electrolyte to flow from one half-cell to the other in order to maintain electroneutrality.

Question 21

Based on the following electrochemical cell, which statement is ? Half-Reaction E° (V) Al³⁺(aq) + 3e^- →
−1)66
Al(s)
Cd²⁺(aq) + 2e^- →
−0)40
Cd(s)

A)Al(s) is oxidized and is the anode.
B)Al(s) is oxidized and is the cathode.
C)Cd(s) is oxidized and is the anode.
D)Cd(s) is oxidized and is the cathode.
E)No reaction occurs because E°_cell < 0.

Question 22

Which element is associated with the term "galvanized"?

A)Ga
B)Zn
C)Cd
D)Hg
E)Pb

Question 23

Aluminum does not corrode in the same manner as iron does, because

A)aluminum does not react with oxygen gas.
B)a protective layer of aluminum oxide forms on the metal surface.
C)aluminum is harder to oxidize than iron.
D)iron gives cathodic protection to aluminum.
E)the electrical circuit cannot be completed on an aluminum surface.

Question 24

Which is the half-reaction at the cathode in a lead storage battery?

A)Pb(s)+ PbO₂(s) + 4H⁺(aq) + 2SO₄^2-(aq) → 2PbSO₄(s) + 2H₂O(l)
B)PbO₂(s) + 4H⁺(aq) + 2SO₄²⁻(aq) + 2e⁻ → PbSO₄(s) + 2H₂O(l)
C)Pb(s) + SO₄²⁻(aq) → PbSO₄(s) + 2e⁻
D)Pb(s) → Pb(s) + 2e⁻
E)H₂(g) → 2H⁺(aq) + 2e⁻

Question 25

Which is the half-reaction at the anode in a lead storage battery?

A)Pb(s) + PbO₂(s) + 4H⁺(aq) + 2SO₄²⁻(aq) → 2PbSO₄(s) + 2H₂O(l)
B)PbO₂(s) + 4H⁺(aq) + 2SO₄²⁻(aq) + 2e⁻ → PbSO₄(s) + 2H₂O(l)
C)Pb(s) + SO₄^2-(aq) → PbSO₄(s) + 2e⁻
D)Pb(s) → Pb(s) + 2e⁻
E)H₂(g) → 2H⁺(aq) + 2e⁻

Question 26

Iron objects such as storage tanks and underground pipelines can be protected from corrosion by connecting them through a wire to a piece of

A)Pb.
B)Ag.
C)Sn.
D)Mg.
E)Cu.

Question 27

Which is the correct cell notation for the following reaction? Au³⁺(aq) + Al(s) → Al³⁺(aq) + Au(s)

A)Al³⁺(aq)|Al(s)||Au³⁺(aq)|Au(s)
B)Al(s)|Al³⁺(aq)||Au³⁺(aq)|Au(s)
C)Al³⁺(aq)|Au³⁺(aq)||Al(s)|Au(s)
D)Al³⁺(aq)|Au(s)||Au³⁺(aq)|Al(s)
E)Au(s)|Al(s)||Au³⁺(aq)|Al³⁺(aq)

Question 28

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

A)Al(s) → Al³⁺(aq) + 3e⁻
B)Al³⁺(aq) + 3e⁻ → Al(s)
C)Ni(s) → Ni²⁺(aq) + 2e⁻
D)Ni²⁺(aq) + 2e⁻ → Ni(s)
E)Ni(s) + Ni²⁺(aq) → Al(s) + Al³⁺(aq)

Question 29

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

A)Cu(s) → Cu²⁺(aq) + 2e⁻
B)Cu²⁺(aq) + 2e⁻→ Cu(s)
C)Ag(s) → Ag⁺(aq) + e⁻
D)Ag⁺(aq) + e⁻ → Ag(s)
E)Cu(s) + 2Ag⁺(aq) → Cu²⁺(aq) + 2Ag(s)

Question 30

Which electrochemical cell pictured below corresponds to the following cell diagram?
Cr(s) | Cr³⁺(aq, 1.0 M) || Sn²⁺(aq, 1.0 M) | Sn(s)

A)
B)
C)
D)
E)