Perdisulphuric acid `(H_2S_2O_8)` or Marshall's acid can be prepared by the electrolytic oxidation of `H_2SO_4`. AT anode `O_2` and `H_2` are obtained as side products. After passing a current of 0.5 A for a certain time, the volume of `H_2` and `O_2` collected was found to be 10.08 and 2.24 L, respectively, at STP. What is the weight of `H_2S_2O_8` produced during the same time? Also find the duration of electrolysis (in seconds) assuming `75%` efficiency of electronysis. Give all the electronde reaction.

Explanation

To solve the problem step by step, we will follow the outlined process to determine the weight of perdisulphuric acid `(H_2S_2O_8)` produced and the duration of electrolysis.

### Step 1: Write the Electrode Reactions

**At the Anode:**
1. The oxidation of sulfate ions can be represented as:
\[
2 \text{HSO}_4^- \rightarrow \text{H}_2\text{S}_2\text{O}_8 + 2e^-
...