Question

Wat will happen if Two or three filing of copper were added to 10 ml dilute nitric acid and stirred

Answer 1

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

Observations-
b) the solution changes from colorless to red
c) a cloud of red toxic gas evolves around the beaker
d) copper is eventually completely consumed

Answer 2

From their first forays into reactivity, students perform experiments which show them that copper doesn't react with acid. One point of teaching the reactivity series is as a stepladder to the electrochemical series, so it makes sense to specifically point out to students that it's a little bit more complicated than that.

This demonstration could be introduced by reminding students of the practicals they will have done lower down the school adding metal strips to dilute hydrochloric acid, either by demonstrating it or by giving students a list of reactions to predict the outcomes of (including both hydrochloric and nitric acids).

The reaction proceeds as:

Cu(s) + 4HNO3 (aq) → Cu(NO3)2 (aq) + 2NO2 (g) + 2H2O(l)

The initial green colour is associated with the copper when ligated by nitrate ions in high concentration in the acid.* As water is added, it displaces the nitrate ions producing the characteristic blue colour in the fountain.

Following the demonstration, students can practice using the electrochemical series to predict the outcome of reactions by combining half cells (from a standard textbook) to explain how magnesium and copper react with hydrochloric and nitric acids in the way they do.
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