1.
2Br- + Fe(OH)2Fe + Br2+ 2OH-
In the above redox reaction, use oxidation numbers to identify the element oxidized, the element reduced, the oxidizing agent and the reducing agent.
name of the element oxidized: fill in the blank 1 name of the element reduced: fill in the blank 2
formula of the oxidizing agent: formula of the reducing agent:

A reducing agent is one of the reactants in an oxidation-reduction reaction, which lowers the other reactant by releasing electrons onto it. If the reducing agent does not transmit electrons to other components during a reaction, the reduction process cannot occur.

For instance, H2(g) + F2(g) 2HF in the reaction given (g)

1 Fe + Br2 + 2OH- 2Br- + Fe(OH)2

Br in Br- has an oxidation state of - 1, but Br in Br2 has an oxidation number of 0 since the molecule is neutral.

Therefore, bromine is the element that is oxidising.

While Fe in Fe(OH)2 has an oxidation number of 0, it has an oxidation state of +2.

Iron is the element that is decreasing, then.

The term "oxidising agent" refers to a material that reduces itself while oxidising others.

Fe(OH)2 will so function as an oxidising agent.

Reducing agents are substances that inhibit the oxidation of other substances while themselves being reduced.

Br- therefore serves as a reducing agent.

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