Hydrogen peroxide can be prepared by successive reaction:
`2NH_(4)HSO_(4) rarr H_(2)+(NH_(4))_(2)S_(2)O_(8)`
`(NH_(4))_(2)S_(2)O_(8)+2H_(2)O rarr 2NH_(4)HSO_(4)+H_(2)O_(2)`
The first reaction is an electrolytic reaction the second is steam distillation. what amount ofcurrent would have to be used in first reaction to produce enough intermediate to yield 100g pure `H_(2)O_(2)` per hour ? Assume `50%` anode current efficiency.

Explanation

To solve the problem of determining the amount of current required in the first reaction to produce enough intermediate to yield 100 g of pure H2O2 per hour, we can follow these steps:

### Step 1: Determine the Equivalent Weight of H2O2
The equivalent weight (Z) of H2O2 can be calculated using the formula:
\[ Z = \frac{\text{Molar mass}}{n} \]
Where:
- Molar mass of H2O2 = 34 g/mol
- n (the number of electrons transferred per molecule of H2O2) = 2 (since the oxidation state of oxygen changes from -2 to -1).
...