Indicate whether each of the following chemical conversions requires an oxidizing agent (o), a reducing agent (r), or neither (n). a) no31- nh3 b) po33- po43- c) agcl ag1+ + cl1- list the letter of your answers in order and separated by commas. for example, o, r,n

The answer is: R, O, N

Explanation:

Oxidizing agent is a chemical species that carries out the oxidation of another chemical species and gets reduced itself .

Whereas, reducing agent is a chemical species that carries out the reduction of another chemical species and gets oxidized itself .

a)  NO₃⁻ → NH₃

In the nitrate ion ( NO₃⁻), the oxidation state of the nitrogen (N) atom is +5.

Whereas, the oxidation state of the nitrogen (N) atom in ammonia (NH₃) is -3.

Thus in this reaction, nitrogen atom is getting reduced from +5 to -3 oxidation state.

Therefore, it requires a reducing agent (R).

b) PO₃³⁻ → PO₄³⁻

In the phosphite ion ( PO₃³⁻), the oxidation state of the phosphorus (P) atom is +3.

Whereas, the oxidation state of the phosphorus (P) atom in phosphate ion (PO₄³⁻) is +5.

Thus in this reaction, phosphorus atom is getting oxidized from +3 to +5 oxidation state.

Therefore, it requires an oxidizing agent (O).

c)  AgCl → Ag⁺ + Cl⁻

The oxidation state of silver (Ag) atom and chlorine (Cl) atom is +1 and -1, respectively.

In this reaction, the oxidation states of silver (Ag) atom and chlorine (Cl) atom remains unchanged.

Therefore, it does not require a oxidizing agent or a reducing agent (N).

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answer:

the reaction is type of combination reaction.

explanation:

on the product side, there are 2 molecules of bonded to fe   which means one atom of fe are combined two molecules of . so, balanced chemical equation becomes :

this reaction follows the reaction type of combination reaction. a combination reaction is defined as chemical reaction in which reactants combines together to form a single product.