If we were to add a piece of solid Cu to an aqueous solution (in water) of silver nitrate, the Silver would be replaced in a single replacement reaction forming aqueous copper (II) nitrate and solid silver. How much silver, in grams, is produced if 15.00 grams of Cu is added to the solution of silver nitrate

50.9 g of Ag

Explanation:

Reaction is:

Cu (s) + 2AgNO₃(aq)  →  2Ag (s) + Cu(NO₃)₂ (aq)

1 mol of Cu react to 2 moles of silver nitrate in order to produce 2 moles of solid silver and 1 mol of copper (II) nitrate.

We assume, the silver nitrate in excess.

We determine moles of copper → 15 g . 1mol / 63.55 g = 0.236 moles

Ratio is 1:2. 1 mol of copper produce 2 moles of silver

0.236 moles of Cu will produce (0.236 . 2) / 1 = 0.472 moles of Ag

We deterine mass of silver:

0.472 mol . 107.87 g /mol = 50.9 g

Option (c) is the correct answer.

Explanation:

The given reaction equation is as follows.

The oxidation-reduction half reactions will be as follows.

Oxidation :

Reduction:

By balancing the above half reactions, oxidation-half reaction will be as follows.

Whereas reduction-half reaction will remain the same.

Hence, it shows that each copper atom is losing one electron to combine with a sulfur atom.

Therefore, we can conclude that each copper atom loses one (1) electron.