Which of the following was oxidixed in the following reaction?
2Na+2H+>2Na+ + H2

Explanation:

By definition 'oxidation' is the loss of electrons by an element and 'reduction' is the gain of electrons by an element. These are easy to remember if one remembers the acronym OIL RIG.

O => Oxidation

I  => Is

L => Loss (of electrons)

R => Reduction

I => Is

G => Gain (of electrons)

To identify the elements undergoing oxidation and reduction compare the oxidation states of reactants and products. If the element becomes more positive an electron(s) are lost => Oxidation Process. If the elements becomes more negative electron(s) are gained => Reduction Process.

For this problem ...

2Na° + 2H => 2Na⁺ + H₂

2Na° => 2Na⁺ + 2e⁻ => oxidation process b/c rxn shows electrons on right of arrow indicating loss of e⁻.

2H⁺ + 2e⁻ => H₂ => reduction process b/c rxn shows electrons on the left of arrow indicating gain of e⁻.

the answer to this question is 3.

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.