3cu(s) + 8 hno3(aq) + 3 cu(no3)2(aq) + 2no(9) + 4h20() c) if 5.58 g of copper(ii) nitrate, cu(no3)2, is eventually obtained, how many moles of nitric acid, hno3, were used in the experiment?

0.0793 mol.

Explanation:

Refer to a modern periodic table for relative atomic mass data:

Formula mass of copper(II) nitrate, :

.

Number of moles of copper(II) nitrate produced:

.

The ratio between the coefficient of and that of in the balanced equation is:

.

In other words,

.

h let me think about that