Electrolysis is a process that involves the decomposition of a compound by passing an electric current through it. In this case, we are considering the electrolysis of an aqueous solution of AgNO3 (silver nitrate) using platinum electrodes.



During electrolysis, various reactions occur at the different electrodes involved. Let's examine the reactions at the anode and cathode separately:



At the anode, oxidation occurs, leading to the release of electrons. In this case, nitrate ions (NO3-) are present in the solution, which can be oxidized. The possible reactions are:

1. 4NO3- (aq) → 2O2 (g) + 4NO2 (g) + 4e-
2. 2H2O (l) → O2 (g) + 4H+ (aq) + 4e-

From the above reactions, it is evident that oxygen gas (O2) will be formed at the anode. However, the actual reaction that takes place depends on the concentration of nitrate ions and the pH of the solution.



At the cathode, reduction occurs, resulting in the consumption of electrons. Silver ions (Ag+) are present in the aqueous solution, which can be reduced. The possible reaction is:

Ag+ (aq) + e- → Ag (s)

From this reaction, it is clear that silver metal (Ag) will be deposited at the cathode.



Considering the reactions at both electrodes, the overall process of electrolysis of AgNO3 can be summarized as follows:

At the anode: Oxygen gas (O2) is evolved.
At the cathode: Silver metal (Ag) is deposited.

Therefore, the product of electrolysis of an aqueous solution of AgNO3 using platinum electrodes is oxygen gas (O2) at the anode and silver metal (Ag) at the cathode.

It is important to note that the concentration of AgNO3 and the current applied will affect the rate of the electrolysis process. Higher concentrations of AgNO3 and higher currents would result in a faster deposition of silver metal at the cathode.