Which species on the left from the Appendix 2 is the strongest oxidising agent?
A) F₂
B) MnO₄⁻
C) PbO₂
D) Cl₂
By using the Appendix 2, which metal ion is most easily reduced to its elemental form?
A) Zn²⁺
B) Cu²⁺
C) Fe²⁺
D) Mg²⁺
Which statement about the half-reaction Br₂ + 2e⁻ ⇌ 2Br⁻ (E° = +1.07 V) is correct?
A. For the half-reaction ½Br₂ + e⁻ ⇌ Br⁻, the electrode potential E° would be +0.535 V.
B. The positive E° value means Br₂ can be easily oxidised.
C. The equation shows that Br⁻ is a relatively poor oxidising agent.
D. The voltage when Br⁻ is oxidized to Br₂ is also +1.07 V.
By using the Appendix 2, which species on the right side is the best reducing agent
A) Ca (from Ca²⁺ + 2e⁻ ⇌ Ca, E° = -2.87 V)
B) Cr (from Cr³⁺ + 3e⁻ ⇌ Cr, E° = -0.74 V)
C) Cu⁺ (from Cu²⁺ + e⁻ ⇌ Cu⁺, E° = +0.15 V)
D) Mn²⁺ (from Mn²⁺ + 2e⁻ ⇌ Mn, E° = -1.18 V)
Using standard reduction potentials, which of these species on the right side is the best reducing agent?
A) Pb (from Pb²⁺ + 2e⁻ ⇌ Pb, E° = -0.13 V)
B) Zn (from Zn²⁺ + 2e⁻ ⇌ Zn, E° = -0.76 V)
C) Fe²⁺ (from Fe³⁺ + e⁻ ⇌ Fe²⁺, E° = +0.77 V)
D) K (from K⁺ + e⁻ ⇌ K, E° = -2.92 V)
Using standard reduction potentials, which species on the left side is the best reducing agent?
A) Zn²⁺ + 2e⁻ ⇌ Zn (E° = -0.76 V)
B) Fe²⁺ + 2e⁻ ⇌ Fe (E° = -0.44 V)
C) Na⁺ + e⁻ ⇌ Na (E° = -2.71 V)
D) Mg²⁺ + 2e⁻ ⇌ Mg (E° = -2.38 V)
Using standard reduction potentials, which of these species on the left side is most easily reduced？
A) F₂ + 2e⁻ ⇌ 2F⁻ (E° = +2.87 V)
B) Cl₂ + 2e⁻ ⇌ 2Cl⁻ (E° = +1.36 V)
C) Br₂ + 2e⁻ ⇌ 2Br⁻ (E° = +1.07 V)
D) I₂ + 2e⁻ ⇌ 2I⁻ (E° = +0.54 V)
Using standard reduction potentials, which of these species on the left side is most difficult to reduce?
A) MnO₄⁻ + 8H⁺ + 5e⁻ ⇌ Mn²⁺ + 4H₂O (E° = +1.52 V)
B) Cr₂O₇²⁻ + 14H⁺ + 6e⁻ ⇌ 2Cr³⁺ + 7H₂O (E° = +1.33 V)
C) O₂ + 4H⁺ + 4e⁻ ⇌ 2H₂O (E° = +1.23 V)
D) PbO₂ + 4H⁺ + 2e⁻ ⇌ Pb²⁺ + 2H₂O (E° = +1.47 V)
Using standard reduction potentials, which species on the left side is most easily oxidised
A) Al³⁺ + 3e⁻ ⇌ Al (E° = -1.66 V)
B) K⁺ + e⁻ ⇌ K (E° = -2.92 V)
C) Ca²⁺ + 2e⁻ ⇌ Ca (E° = -2.87 V)
D) Li⁺ + e⁻ ⇌ Li (E° = -3.04 V)
Which of the standard electrode piential can be determined from the diagram belwo(Think about the direction of electron flow) )?
A) Cr²⁺ + 2e⁻ ⇌ Cr (E° = -0.91 V)
B) Mn²⁺ + 2e⁻ ⇌ Mn (E° = -1.18 V)
C) Sn⁴⁺ + 4e⁻ ⇌ Sn (E° = -0.14 V)
D) Fe³⁺ + e⁻ ⇌ Fe²⁺ (E° = +0.77 V)
In a standard electrochemical cell, electrons flow:
A) From the negative pole to the positive pole through the salt bridge.
B) From the positive pole to the negative pole through the external wire.
C) From the negative pole to the positive pole through the external wire.
D) From the positive pole to the negative polethrough the electrolyte solution.
When the Standard Hydrogen Electrode (SHE) is combined with a Mn²⁺/Mn half-cell in an electrochemical cell, which half-cell acts as the positive pole?
A) Mn²⁺/Mn half-cell
B) Standard Hydrogen Electrode (SHE)
C) Both act as the positive pole
D) Neither; the cell cannot operate
When a Zn²⁺/Zn half-cell ( E ° = − 0.76 V) is combined with a Cu²⁺/Cu half-cell ( E ° = + 0.34 V), which half-cell acts as the positive pole (cathode)?
A) Zn²⁺/Zn half-cell
B) Cu²⁺/Cu half-cell
C) Both half-cells
D) The salt bridge
When the Standard Hydrogen Electrode (SHE) is combined with a MnO₄⁻/Mn²⁺ half-cell ( E ° = + 1.51 V), which half-cell acts as the negative pole (anode)?
A) The salt bridge
B) MnO₄⁻/Mn²⁺ half-cell
C) Standard Hydrogen Electrode (SHE)
D) Both half cells
Which of the following statements best describes the difference between a galvanic cell and an electrolytic cell?
A) Galvanic cells require an external power source, while electrolytic cells do not.
B) Galvanic cells: oxidation occurs at the negative pole. In electrolytic cells: oxidation occurs at the cathode.
C) Galvanic cells convert chemical energy into electrical energy, while electrolytic cells perform the reverse process.
D) Electrons flow from the cathode to the anode in both types of cells.