Y13 electrode potentials and redox exam MC

Which one of the following is the electronic configuration of the strongest reducing agent?

• 1s² 2s² 2p⁵

• 1s² 2s² 2p⁶ 3s²

• 1s² 2s² 2p⁶ 3s² 3p⁵

• 1s² 2s² 2p⁶ 3s² 3p⁶ 4s²

Which of the following shows chlorine in its correct oxidation states in the compounds shown? HCl | KClO₃ | HClO

• -1 | +3 | +1

• +1 | -5 | -1

• -1 | +5 | +1

• +1 | +5 | -1

In which one of the following reactions is the role of the reagent stated correctly?

• TiO₂ is an oxidising agent

• HNO₃ is a Brønsted-Lowry acid

• AlCl₃ is a Lewis base

• CO is a reducing agent

A cell with EMF = +2.15 V is made from two electrodes. The half-equations for the two electrodes are shown. positive electrode: PbO₂(s) + 3H⁺ (aq) + HSO₄^- (aq) + 2 e- → PbSO₄(s) + 2H₂O(l) negative electrode: PbSO₄(s) + H⁺ (aq) + 2e- → Pb(s) + HSO₄^- (aq) E° = -0.46 V What is the standard electrode potential of the PbO₂ / PbSO₄ electrode?

• -2.61 V

• -1.69 V

• +1.69 V

• +2.61 V

Which incomplete half-equation is balanced by adding two H⁺ ions and one electron to the left-hand side?

• CH₃CHO → CH₃CH₂OH

• VO²⁺ → V³⁺ + H₂O

• HNO₂ → NO + H₂O

• O₂ → H₂O₂

In which conversion is the metal reduced?

• Cr₂O₇²⁻ → CrO₄²⁻

• MnO₄²⁻ → MnO₄⁻

• TiO₂ → TiO₃²⁻

• VO³⁻ → VO²⁺

In which one of the following reactions is H₂O₂ behaving as a reducing agent?

• H₂O₂ + 2I⁻ + 2H⁺ → I₂ + 2H₂O

• H₂O₂ + 2[Co(NH₃)₆]²⁺ → 2[Co(NH₃)₆]³⁺ + 2OH⁻

• 5H₂O₂ + 2MnO₄⁻ + 6H⁺ → 2Mn²⁺ + 8H₂O + 5O₂

• 3H₂O₂ + 2[Cr(OH)₆]³⁻ → 2CrO₄²⁻ + 8H₂O + 2OH⁻

Which of these is not a redox reaction?

• A. Cu₂O + H₂SO₄ → CuSO₄ + Cu + H₂O

• B. MgO + 2HCl → MgCl₂ + H₂O

• C. SnCl₂ + HgCl₂ → Hg + SnCl₄

• D. MnO₂ + 4HCl → MnCl₂ + 2H₂O + Cl₂

In which reaction is the metal oxidised?

• 2Cu⁺ + 4I⁻ → 2CuI + I₂

• [Fe(H₂O)₆]³⁺ + Cl⁻ → [Fe(H₂O)₅(Cl)]₂+ + H₂O

• [CoCl₄]²⁻ + 6H₂O → [Co(H₂O)₆]²⁺ + 4Cl⁻

• Mg + S → MgS

In which oxide is the named element in its highest oxidation state?

• Chlorine in ClO₂

• Magnesium in MgO

• Nitrogen in N₂O₄

• Sulfur in SO₂