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6 April, 11:14

13. Write the following balanced reactions using cell notation. Use platinum as an inert electrode, if needed. (a) Mg (s) + Ni2 + (aq) ⟶ Mg2 + (aq) + Ni (s) (b) 2Ag + (aq) + Cu (s) ⟶ Cu2 + (aq) + 2Ag (s) (c) Mn (s) + Sn (NO3) 2 (aq) ⟶ Mn (NO3) 2 (aq) + Au (s) (d) 3CuNO3 (aq) + Au (NO3) 3 (aq) ⟶ 3Cu (NO3) 2 (aq) + Au (s)

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  1. 6 April, 11:22
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    A) Mg ₍s₎ | Mg²⁺₍aq₎║Ni²⁺₍aq₎ | Ni₍s₎

    B) Cu₍s₎ | Cu²⁺₍aq₎║ Ag⁺ | Ag⁰₍s₎

    C) Cu₍s₎ | Cu²⁺₍aq₎║ Ag⁺ | Ag⁰₍s₎

    D) Pt₍s₎ | CuNO₃₍ aq₎, Cu (NO₃) ₂₍aq₎ ║ Au (NO₃) ₃₍aq₎ | Au₍s₎

    Explanation:

    A) Mg + Ni²⁺ → Mg²⁺ + Ni

    Mg⁰→ Mg²⁺ + 2e⁻ oxidation anode

    Ni²⁺ + 2e⁻ → Ni⁰ reduction cathode

    Mg ₍s₎ | Mg²⁺₍aq₎║Ni²⁺₍aq₎ | Ni₍s₎

    anode salt bridge cathode

    B) 2 Ag⁺₍aq₎ + Cu₍s₎ → Cu²⁺₍aq₎ + 2 Ag₍s₎

    2 Ag⁺ + 2e⁻ → 2 Ag⁰ cathode

    Cu → Cu²⁺ + 2e⁻ anode

    Cu₍s₎ | Cu²⁺₍aq₎║ Ag⁺ | Ag⁰₍s₎

    anode salt bridge cathode

    C) Mn ₍s₎ + Sn (NO₃) ₂ ₍aq₎ → Mn (NO₃) ₂ ₍aq₎ + Au₍s₎

    Mn⁰ → Mn²⁺ + 2e⁻ anode

    Sn²⁺ + 2e⁻ → Sn⁰₍s₎ cathode

    Mn₍s₎ | Mn (NO₃) ₂ ₍aq₎ ║ Sn (NO₃) ₂ ₍aq₎ | Sn₍s₎

    anode salt bridge cathode

    D) 3CuNO₃₍ aq₎ + Au (NO₃) ₃₍aq₎ → 3Cu (NO₃) ₂₍aq₎ + Au₍s₎

    3Cu⁺ → 3Cu²⁺ + 3e⁻ anode

    Au³⁺ + 3e⁻ → Au⁰ cathode

    Pt₍s₎ | CuNO₃₍ aq₎, Cu (NO₃) ₂₍aq₎ ║ Au (NO₃) ₃₍aq₎ | Au₍s₎

    anode salt bridge cathode

    Semi-reactions are noted to determine oxidation and reduction. The oxidation reaction occurs at the anode and the reduction reaction at the cathode. In the case of subsections a, b, c the electrodes may be the solid metal, while in the case d the species are in an accusative medium and require the platinum electrode.
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