Use the equation below to determine how many moles of silver nitrate (AgNO3) are needed to produce 6.75 moles of copper (II) nitrate (CU (NO3) 2) upon reacting with excess copper (Cu).

2AgNO3 (aq) + Cu (s) à 2Ag (s) + Cu (NO3) 2 (aq).

A. 2.80 mole AgNO3

B. 5.65 mole AgNO3

C. 10.75 mole AgNO3

D. 13.50 mole

1) Balanced chemical reaction:

2AgNO3 (aq) + Cu (s) - - > 2Ag (s) + Cu (NO3) 2 (aq).

2) Theoretical molar ratios

2 mol AgNO3 : 1 mol Cu : 2 mol Ag : 1 mol Cu (NO3) 2

3) Molar proportion with the unknown:

x mol AgNO3 / 6.75 mol Cu (NO3) 2 = 2 mol AgNO3 / 1 mol Cu (NO3) 2

=> x = 6.75 mol Cu (NO3) 2 * 2 mol AgNO3 / 1 mol Cu (NO3) 2

=> x = 13.50 mol AgNO3

Answer: option D. 13.50 mole