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

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