3Ag(s)+4HNO3(aq)-->3AgNO3(aq)+NO(g)+2H2O(l)

Write the net ionic equation.

Alright, get ready for some chemistry clowning! The net ionic equation for this reaction can be written as:

3Ag(s) + 4H+(aq) + 3NO3-(aq) → 3Ag+(aq) + NO(g) + 2H2O(l)

Now that's a balancing act worth applauding!

To write the net ionic equation, we first need to write the balanced molecular equation for the given reaction.

The balanced molecular equation is:
3Ag(s) + 4HNO3(aq) → 3AgNO3(aq) + NO(g) + 2H2O(l)

To get the net ionic equation, we need to separate the strong electrolyte compounds into their ions:

Ag(s) does not dissociate as it is a solid and not an electrolyte.
HNO3(aq) dissociates into H+(aq) and NO3-(aq).
AgNO3(aq) dissociates into Ag+(aq) and NO3-(aq).

The net ionic equation is obtained by removing the spectator ions, which are the ions that appear on both sides of the equation unchanged:

The ions NO3-(aq) and Ag+(aq) appear on both sides of the equation unchanged, so they are spectator ions.

The net ionic equation for the given reaction is:
3Ag(s) + 4H+(aq) → NO(g) + 2H2O(l)

To write the net ionic equation, we need to first write the balanced equation for the given chemical reaction:

3Ag(s) + 4HNO3(aq) → 3AgNO3(aq) + NO(g) + 2H2O(l)

Next, we need to identify the spectator ions. Spectator ions are the ions that do not participate in the reaction and remain the same on both sides of the equation. In this case, the spectator ions are NO3^- and H+.

Now, let's remove the spectator ions from the equation to write the net ionic equation:

Net Ionic equation:
3Ag(s) + 4H+(aq) → 3Ag+(aq) + NO(g) + 2H2O(l)

Therefore, the net ionic equation for the given reaction is 3Ag(s) + 4H+(aq) → 3Ag+(aq) + NO(g) + 2H2O(l).

Ag(s) + 4H^+(aq) + 4NO3^-(aq) ==> 3Ag^+(aq) + NO(g) + 2H2O(l)