If 15.00g of Magnesium metal reacts with a solution containing AgNO3 to produce silver metal, how much silver is produced in moles? Show work please. :)

Answer 1

Let's first write a correctly balanced equation for this reaction:

Mg(s) + 2AgNO₃(aq) ==> 2Ag(s) + Mg(NO₃)₂(aq)

Now, using stoichiometry we can find the moles of silver (Ag) produced (assuming AgNO₃ is not limiting)

Moles of Mg present = 15.00 g Mg x 1 mol Mg/24.31 g = 0.6170 moles Mg

Moles Ag produced = 0.6170 mol Mg x 2 mol Ag/mol Mg = 1.234 moles Ag (to 4 sig.figs.)