An aqueous solution containing `Na^(+),Sn^(2+),Cl^(-)` & `SO_(4)^(2-)` ions, all at unit concentration is electrolysed between a silver anode and a platium cathode. What changes occur at the electrodes when curret is passed through the cell? Given `E_(Ag^(+)|Ag)^(0)=0.799V`,
`E_(Sn^(2+)|Cn)^(0)=-0.14V,E_(Cl_(2)|Cr^(-))^(0)=1.36V,E_(S_(2)O_(8)^(2-)|SO_(4)^(2-))=2V,E_(Sn^(4+)|Sn^(2+))^(0)=0.13V`
(A). `Sn^(2+)` is reduced and `Cl^(-)` is oxidized
(B). Ag is oxidized and `Sn^(2+)` is reduced
(C). `Sn^(2+)` is reduced and `Sn^(2+)` is oxidized
(D). `H^(+)` is reduced and `Sn^(2+)` is oxidised

Explanation

To solve the problem, we need to analyze the electrolysis process occurring in the cell with the given ions and their standard reduction potentials. Here’s a step-by-step breakdown of the solution:

### Step 1: Identify the Electrodes
In the electrolysis setup:
- **Anode**: Where oxidation occurs (loss of electrons).
- **Cathode**: Where reduction occurs (gain of electrons).

### Step 2: Determine Possible Reactions at the Anode
...