Chemistry, 15.11.2019 06:31 oudithe3

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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Answer from: yuvin

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.

Answer from: Quest

Because electrons have negligible mass, to account for the mass of the isotope, there must be 16 neutrons, 16 neutrally charged, massive, fundamental particles present in the sulfur nucleus. and thus finally, if we have the 32s2− ion, there are 18 electrons, 16 protons, and 16 neutrons.

Answer from: Quest

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13. write the following balanced reactions using cell notation. use platinum as an inert electrode,...

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