Why does nitric acid not react with metal?

Al doesn't dissolve in nitric acid.

The reason is quite obvious. When Al come in contact with nitric acid, the upper layer, which comes into the contact of acid first, oxidizes into Al2O3.

This layer remains at the metal piece dropped in acid, and protects the inner Al from the acid. This happens because the layer is already oxidised and can't be oxidised further. Moreover Al2O3 doesn't react with acid. So the passive layer of Al2O3 prevents the reaction between Al and nitric acid.

When metals( Cu, Na, Zn) react with mineral acids like dil HCL and H2SO4, hydrogen gas is evolved.

Nitric acid is an acid that decomposes very quickly.

When metals react with mineral acids except nitric acid, the respective salt and H2 gas is evolved.

How do you confirm that the gas released is hydrogen?

When you introduce a burning splinter the gas will burn with a pop sound.

That’s all!!!!

Nitric acid does not react with metal because it is a strong oxidising agent and form the layer .

So nitric acid doesn't react with metal.

It’s easy - the reaction in question involves the oxidation of a metal which in the case of nitric acid is being driven by nitrate -a much stronger (more active) oxidant than is the hydrogen (aka “hydronium ion”) associated with both it and other strong acids such hydrochloric or sulfuric acid . Consequently, the products of that reaction include the reduced forms of nitrate, N2, N2O, NO & NO2, not the reduced form of the hydronium ion, hydrogen gas.

Usually when a metal reacts with an acid, hydrogen is released but in the case of nitric acid, it is not so. The reason is that the hydrogen which is released is oxidesed by the oxygen given out as nitric acid is a very strong oxidizing agent and it forms water. the water is the hydrogen which has been oxidised.

Solid nonmetals like carbon, phosphorus, sulphur and iodine react with concentrated nitric acid in very hot condition.

C + 4HNO3 → CO2 + 4NO2 + 2H2O

S + 6HNO3 → H2SO4 + 6NO2 + 2H2O

P + 5HNO3 → H3PO4 + 5NO2 + H2O

I2 + 10HNO3 → 2HIO3 +10NO2 + 4H2O

These are redox reactions in which each nonmetal is oxidised to its respective higher oxide/oxoacid by the acid and the latter is reduced to nitrogen dioxide (NO2).

But it does dissolve in nitric acid. (I have done it a few times as part of a phos anodize demo tank prep.)

Check your sources b4 u post. Save from making your cheeks so pink.

Very Very Generalized statement

Nitric acid does react with metals, in different conditions

Copper reacts with HNO3 in following ways

Cu + 4HNO3——————-> Copper Nitrate+ NO2+water

Dil HNO3 reacts to give nitrous oxide

Tin too reacts. So we cant say that all metals don't react

Why can nitric acid not react with aluminium?

Aluminium normally has a thin, colorless coating of its oxide, which is essentially inert chemically. (Such a coating is called a protective oxide.)
The nitric acid can’t attack the metal under its “armor coating”.
If the metal were scratched while it was in the acid, so that there was a break in the oxide, then corrosion would begin.

Magnesium and manganese react with cold, very dilute nitric acid to give oxidized product and hydrogen.

Mg +2HNO3➡Mg(NO3) 2 +H2

Mn+2HNO3➡Mn(NO3) 2+H2

Copper,zinc and iron react with dilute nitric acid to give oxidized product, water and nitric oxide.

3Cu +8HNO3➡Cu(NO3) 2+4H2O+ 2NO

3Zn+8HNO3➡Zn(NO3) 2+4H2O+2NO

3Fe +8HNO3➡Fe(NO3) 2+4H2O+2NO

Nitric acid(HNO3) is a strong oxidising agent.
The Hydrogen gas produced during its reaction with metal gets oxidised to H2O, hence no hydrogen gas is produced.
Instead it evolves nitric oxides such as NO2,NO etc.

For Eg:
Cu(s) + 4HNO3(aq)--->Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l)