Copper(II) nitrate, represented by the chemical formula Cu(NO3)2, is a complex formed by the reaction of copper and nitric acid. This reaction is an oxidation-reduction (redox) reaction in which copper undergoes oxidation and nitrate ions undergo reduction.

Cu0 - 2 e- → CuII (oxidation)

2 NV + 2 e- → 2 NIV (reduction)

Cu acts as a reducing agent in this reaction while nitric acid acts as an oxidizing agent.

Word equation:

Copper + Nitric acid → Copper(II) nitrate + Nitrogen dioxide + Water

Input interpretation:

Cu + HNO3 → Cu(NO3)2 + NO2 + H2O

The balanced equation for this reaction is obtained by following a series of steps:

Balanced equation:

Balance the chemical equation algebraically:

Cu + HNO3 → Cu(NO3)2 + NO2 + H2O

Add stoichiometric coefficients, c1, to the reactants and products:

c1Cu + c2HNO3 → c3Cu(NO3)2 + c4NO2 + c5H2O

Set the number of atoms in the reactants equal to the number of atoms in the products for Cu, H, N, and O:

Cu: c1 = c3

H: c2 = 2c5

N: c2 = 2c3 + c4

O: 3c2 = 6c3 + 2c4 + c5

Since the coefficients are relative quantities and underdetermined, choose a coefficient to set arbitrarily. To keep the coefficients small, the arbitrary value is ordinarily one. For instance, set c1 = 1 and solve the system of equations for the remaining coefficients:

c1 = 1

c2 = 4

c3 = 1

c4 = 2

c5 = 2

Substitute the coefficients into the chemical reaction to obtain the balanced equation:

Cu + 4HNO3 → Cu(NO3)2 + 2NO2 + 2H2O