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)

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.

samuel de champlain. in 1608, king henry iv sponsored pierre dugua, sieur de mons and samuel de champlain as founders of the city of quebec with 28 men. this was the second permanent french settlement in the colony of canada.

a. hope i'm right

explanation: