Copper reacts with silver nitrate through single replacement.

a. if 2.25 g of silver are produced from the reaction, how many moles of copper(ii) nitrate are also produced?
b. how many moles of each reactant are required in this reaction?

Part a) 0.0104 moles copper(II) nitrate.Part b)

            i) 0.0418 mole Cu

            ii) 0.0209 mol Ag NO₃

Explanation:

1) Balanced chemical reaction (single replacement):

In a single replacement reaction a more acitve metal (Cu) replaces a less active metal (Ag)

Cu + 2 Ag NO₃ → Cu (NO₃)₂ + 2 Ag

2) Mole ratio:

1 mole Cu : 2 mole Ag NO₃ : 2 mole Ag

3) Moles of Ag

n = mass in grams / atomic massatomic mass of Ag: 107.868 g/moln = 2.25 g / 107.868 g/mol = 0.0209 mol Ag

4) Moles of copper(II) nitrate:

Set the proportion using the mole ratio:2 mole Ag / 1 mole Cu (NO₃)₂ = 0.0209 mole Ag / xSolve: x = 0.0209 / 2 mole Cu (NO₃)₂ =  0.0104 moles Cu(NO₃)₂

That is the answer of part a: 0.0104 moles copper(II) nitrate.

5) Moles of each reactant

i) Cu:

Set a proportion using the theoretical mole ratio

        1 mole Cu / 2 mole Ag = x / 0.0209 mol Ag

Solve for x: x = 0.0209 / 2 mole Cu = 0.0418 mole Cu

ii) Ag NO₃

Set a proportion using the teoretical mole ratio

   

       2 mole Ag NO₃ / 2 mole Ag = x / 0.0209 mole Ag

Solve for x: x = 0.0209 mol Ag NO₃

The answer is 323 g.