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⁻.

c. 75.7

i think that is the right