3Cu(s) + 8HNO\(_3\)(aq)  → 3Cu(NO\(_3\))\(_2\)(aq) + 4H\(_2\)O(l) + 2NO(g)
In the equation above, copper is

Derek644222

2 years ago

3Cu(s) + 8HNO3(aq) → 3Cu(NO3)2(aq) + 4H2O(l) + 2NO(g)



Copper (Cu) starts in its elemental state (Cu(s)) on the left side of the equation and ends up in the +2 oxidation state in copper(II) nitrate (Cu(NO3)2)
on the right side.

The oxidation state of copper changes from 0 to +2. This means that copper has lost electrons during the reaction, which is characteristic of a reducing agent.

A reducing agent is a substance that undergoes oxidation by losing electrons and thereby causes another substance to be reduced. In this reaction, copper acts as the reducing agent because it loses electrons (undergoes oxidation) while causing the nitric acid (HNO3) to be reduced to nitrogen dioxide (NO) and water (H2O).

Therefore, copper (Cu) is classified as a reducing agent in this reaction.

HighestscorerLawy

1 year ago

Just use OIL RIG(Oxidatioon Involves Loss of electrons and Reduction Involves Gaining of electrons .

chijioke7

7 years ago

Copper is oxidised in the reaction, and reducing agents are the ones that are oxidised

Award0001

2 years ago

just be careful to note that Oxidation and reduction has up to 3 definitions...

the definition that matches this particular question is "oxidation is addition of electronegative and removal of electropositive"

Normally reducing agents are oxidized so A is the answer

agadido

3 years ago

But the removal of hydrogen nauu, it's supposed to be C

egbonjosh

8 years ago

oxidation=reducing agent

samlaz

2 years ago

Wrong question

godstamtam

7 years ago

Oxidation is Addition of hydrogen nd removal of oxygen
While
Reduction is the addition of oxygen nd removal of hydrogen