Question

complete each of the following reactions and write the balanced molecular and net ionic equations for each reaction and identify the reaction type. For any redox reactions, show the oxidations numbers, identify the substance oxidized and the substance reduced, the oxidizing agent, and the reducing agent, and write the half reactions for oxidation and reduction.

a. Lead II nitrate and sodium iodide react to form products

b. Aluminum hydroxide is neutralized by sulfuric acid

c. sulfur burns in oxygen to make sulfur dioxide

Answer 1

SOLN A

Molecular:

Pb(NO₃)₂(aq) + 2 NaI(aq) => PbI₂(s) + 2 NaNO₃(aq)

Complete ionic:

Pb²⁺(aq) + 2 NO₃^-(aq) + 2 Na⁺(aq) + 2 I^-(aq)

=> PbI₂(s) + 2 Na⁺(aq) + 2 NO₃^-(aq)

Net ionic:

Pb²⁺(aq) + 2 I^-(aq) => PbI₂(s)

Reaction Type : Simple displacement reaction

SOLN B

Molecular equation 2A (OH), 18 + 3 Hy sou (29) ► Aug (504), (aq) + 6H₂O(l) Total ionic equation -2 Al(OH), (3) & 64* (o) + 359, ² (aq) → 2 Alt (as) - 4 3504 (aq) + 6Holes Net ionic equation 2 Al(OH), (s) + 6H² (aq) → 2 Aets (aq) + 6H₂0 (1)

SOLN C

S + O2 -----> SO2

This is not an ionic reaction. It is redox reaction

S is i n 0 oxidation state in elemental form whereas in SO2 it is in +4 oxidation state hence it is oxidized hence it is a reducing agent

whereeas O2 is in 0 oxidataion state whereas in SO2 it is in -2 oxidation state hence it is reduced hence it is a oxidizing agent

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