Marshall's acid `(H_(2)S_(2)O_(8))` or peroxodisulphuric acid is prepared by the electrolytic oxidation of mmol`H_(2)SO_(4)` as `:`
`2H_(2)SO_(4) rarr H_(2)S_(2)O_(8)+2H^(o+)+2e^(-)`
`O_(2)(g)` and `H_(2)(g)` are obtained as byproducts. In such electrolysis `4.48L` of `H_(2)(g)` and `1.12L` or `O_(2)(g)` were produced at `STP`. The weight of `H_(2)S_(2)O_(8)` formed is
`a. 9.7g" "b.19.4g" "c.14.5g" "d.29.1g`

Explanation

To solve the problem of calculating the weight of Marshall's acid (H₂S₂O₈) formed during the electrolysis of H₂SO₄, we can follow these steps:

### Step 1: Determine Moles of Gases Produced
We know the volumes of hydrogen (H₂) and oxygen (O₂) produced during the electrolysis:
- Volume of H₂ = 4.48 L
- Volume of O₂ = 1.12 L

Using the ideal gas law at STP (Standard Temperature and Pressure), where 1 mole of gas occupies 22.4 L, we can calculate the moles of each gas.
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