Copper reacts with hydrogen nitrate to produce copper (II) nitrate, nitrogen monoxide and water

The reaction of copper with hydrogen nitrate to produce copper (II) nitrate, nitrogen monoxide, and water can be represented by the following balanced chemical equation:

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

Here's the step-by-step process:

1. Copper (Cu) reacts with hydrogen nitrate (HNO3), also known as nitric acid. This is a redox reaction, where copper is oxidized and nitric acid is reduced.

2. The copper metal loses two electrons to become copper (II) ions (Cu2+). This is represented by the equation: Cu(s) → Cu2+(aq) + 2e-

3. The nitric acid gains these electrons to become nitrogen monoxide (NO) and water (H2O). This is represented by the equation: 2HNO3(aq) + 3e- → NO(g) + H2O(l) + 2NO3-(aq)

4. The copper (II) ions (Cu2+) and nitrate ions (NO3-) combine to form copper (II) nitrate (Cu(NO3)2).

5. The overall reaction is: 3 Cu(s) + 8 HNO3(aq) → 3 Cu(NO3)2(aq) + 2 NO(g) + 4 H2O(l)

This reaction is exothermic, meaning it releases heat. It also produces a brown gas (nitrogen monoxide) and a blue solution (copper (II) nitrate).