A piece of copper metal is dipped into an aqueous solution of AgNO3. Which net ionic equation describes the reaction that occurs? A. Cu(s) + 2Ag+(aq) + 2NO3–(aq) → 2AgNO3(s) + Cu2+(aq) B. 2Ag+(aq) + 2NO3–(aq) → 2AgNO3(s) C. Cu(s) + 2Ag+(aq) → 2Ag(s) + Cu2+(aq) D. 2NO3–(aq) + Cu2+(aq) → Cu(s) + 2Ag(s)

Cu(s) + 2Ag+(aq) → 2Ag(s) + Cu2+(aq) (option C)

Explanation:

Step 1: the unbalanced equation

Cu(s) + AgNO3(ag) → Ag + Cu(NO3)2

Step 2: The balanced equation

Cu(s) + AgNO3(ag) → Ag + Cu(NO3)2

On the left side we have 1x NO3 (in AgNO3), on the right side we have 2x NO3, in Cu(NO3)2. To balance the amount of NO3 on both sides we have to multiply AgNO3, on the left side, by 2

Cu(s) + 2AgNO3(ag) → Ag + Cu(NO3)2

On the left side we have 2x Ag (in 2AgNO3) , on the right side we have 1x Ag. To balance the amount of Ag on both sides we have to multiply Ag, on the right side, by 2. Now the equation is balanced.

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

The net ionic equation, for which spectator ions are omitted - remember that spectator ions are those ions located on both sides of the equation - will , after canceling those spectator ions in both side (Ba^2+ and Br-), look like this:

Cu(s) + 2Ag+(aq) → 2Ag(s) + Cu2+(aq) (option C)

they are both synthetic elements

explanation:

d

the answer for sodium is 0.186

the answer for rubidium is 0.251