Given the balanced reaction below; write out the balanced ionic equation and the balanced net ionic equation. Include phase labels and charges where appropriate.
Cu(s) + Zn(NO3)2 (aq) → Cu(NO3)2 (aq) + Zn(s)
To write the balanced ionic equation and net ionic equation for the given reaction, let's first identify the species that are dissociated in the solution.
The balanced equation provided is:
Cu(s) + Zn(NO3)2 (aq) → Cu(NO3)2 (aq) + Zn(s)
In the reaction, Cu(s) is a solid (a) while Zn(NO3)2 (aq) and Cu(NO3)2 (aq) are aqueous (aq) solutions. Zn(s) is also a solid (s).
Now, let's write the ionic equation by first dissociating the compounds that are soluble in aqueous solution:
Cu(s) → Cu^2+ (aq) + 2e- (1)
Zn(NO3)2 (aq) → Zn^2+ (aq) + 2NO3^- (2)
Cu(NO3)2 (aq) → Cu^2+ (aq) + 2NO3^- (3)
Zn(s) → Zn^2+ (aq) + 2e- (4)
Equations (1) and (4) represent the oxidation half-reactions, while equations (2) and (3) represent the reduction half-reactions.
Now, let's balance the charges and electrons:
2Cu(s) → 2Cu^2+ (aq) + 4e- (1)
Zn(NO3)2 (aq) → Zn^2+ (aq) + 2NO3^- (2)
Cu(NO3)2 (aq) → Cu^2+ (aq) + 2NO3^- (3)
2Zn(s) → 2Zn^2+ (aq) + 4e- (4)
To write the net ionic equation, we need to eliminate the spectator ions, which are the ions present on both sides of the equation without undergoing a chemical change. In this case, the NO3^- ions are spectator ions.
The net ionic equation is:
2Cu(s) + 2Zn^2+ (aq) → 2Cu^2+ (aq) + 2Zn(s)
This equation shows only the species that undergo chemical changes during the reaction.
In summary:
The balanced ionic equation is:
2Cu(s) + Zn(NO3)2 (aq) → 2Cu^2+ (aq) + 2NO3^- (aq) + 2Zn(s)
The balanced net ionic equation is:
2Cu(s) + 2Zn^2+ (aq) → 2Cu^2+ (aq) + 2Zn(s)