Electrolytic oxidation of `H_2SO_4` gives rise to the formation of persulphuric acid, `H_2S_2O_8`.
`2H_2SO_4 to H_2S_2O_8 + 2H^(+) + 2e`
If 4 litres of `O_2` and 11.2 litres of `H_2` were produced at NTP, determine the mass of `H_2S_2O_8` produced.

Explanation

To determine the mass of persulphuric acid (H₂S₂O₈) produced from the electrolytic oxidation of sulfuric acid (H₂SO₄), we can follow these steps:

### Step 1: Understand the Reaction
The given reaction is:
\[ 2 \text{H}_2\text{SO}_4 \rightarrow \text{H}_2\text{S}_2\text{O}_8 + 2 \text{H}^+ + 2 e^- \]

### Step 2: Calculate the Moles of Hydrogen and Oxygen Produced
At Normal Temperature and Pressure (NTP), 1 mole of any gas occupies 22.4 liters.
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