Question

Write balanced molecular, total ionic, and net ionic equations for the following aqueous single-displacement reactions.

(5 points) Write balanced molecular, total ionic, and net ionic equations for the following aqueous single- 3. displacement reactions. Also tell what is oxidized and what is reduced in each. aluminum + iron(l) nitrate a. Molecular: Total lonic Net lonic Reduced: Oxidized: acetic acid+ tin, which forms the tin(ll) ion in these reactions b. Molecular: Total lonic: Net lonic: Reduced: Oxidized: zinc+ gold(iIlI) chloride C. Molecular: Total lonic: Net lonic Oxidized Reduced:

Answer 1

Oxidized : A species is said to be oxidized if it losses electrons

And A species is said to be reduced if it gains electrons

5. Given reaction is:

Molecular: Al (s) + Fe(NO₃)₂(aq) ---> Al(NO₃)₂(aq) + Fe(s)

Ionic: Al(s) + Fe²⁺(aq) + 2NO₃^-(aq) ---> Al²⁺(aq) + 2NO₃^-(aq) + Fe(s)

Total Ionic : Al(s) + Fe²⁺(aq) ---> Al²⁺(aq) + Fe(s)

Oxidized = Al

Reduced = Fe²⁺

6. Molecular: 2CH₃COOH(aq) + Sn(s) ---> Sn(CH₃COO)₂(aq) + H₂(g)

Ionic: 2CH₃COOH(aq) + Sn(s) ---> Sn²⁺(aq) + 2CH₃COO^-(aq) + H₂(g)

Net Ionic:  2CH₃COOH(aq) + Sn(s) ---> Sn²⁺(aq) + 2CH₃COO^-(aq) + H₂(g)

Oxidized: Sn

Reduced : CH₃COH

7. Complete reaction is:

Molecular: AuCl₃(aq) + 3Ag(s) ---> 3AgCl (s) + Au (s)

Total Ionic: Au³⁺(aq) + 3Cl^-(aq) + 3Ag(s) ---> 3AgCl(s) + Au(s)

Net Ionic: Au³⁺(aq) + 3Cl^-(aq) + 3Ag(s) ---> 3AgCl(s) + Au(s)

Oxidized: Ag

Reduced : Au