Question

13) Consider the reaction below where 0.794 g of copper fully reacts, consuming 250.0 mL of AgNO3. What must have been the molarity of the AgNO3? 2 AgNO3 (aq) + Cu (s)  Cu(NO3)2 (aq) + 2 Ag (s)

Answer 1

013) Ceils) + 2Ag NO ₂ cap) → Cu (NO3)₂ (aq) + 2Agg of mass no. of cu reacted = 0. T94 g. mates of cu reacted - Given more Molar mass 0.7948 63.546 gmott 0.0125 mol. . no. of moles of cu 0.0125 motes = = 2(no of moles of AgNO3). 2 (no, of motes of Ang . No. of moles of AgNO3 - 0.0125 mol - 0.006 mol. . Molarity of Ano son no. of moles of Agnoz U o volume of soln 0.006 mot 1000 mLY 250.0 mL - molly 0.024 M . Molarity of Ag NO3 soln = 0.024M