Electrolysis of a solution of `HSO_(4)^(-1)` ions produces `S_(2)O_(8)^(2-)`. Assuming `75%` current efficiency, what current should be employed to achieve a production rate of 1 "mole" of `S_(2)O_(8)^(2-)` per hour?

What will be oxidation number of sulphur in S_2O_(8)^(2-) ion and S_(4)O_(6)^(2-) ion ?

During the electrolysis of conc H_(2)SO_(4) , it was found that H_(2)S_(2)O_(8) and O_(2) liberated in a molar ratio of 3:1 . How many moles of H_(2) were found of moles of H_(2)S_(2)O_(8) ? ( Express your answer as :3xx mol e s of H_(2), integer answer is between 0 and 5 0

During the electrolysis of conc H_(2)SO_(4) , it was found that H_(2)S_(2)O_(8) and O_(2) liberated in a molar ratio of 3:1 . How many moles of H_(2) were found of moles of H_(2)S_(2)O_(8) ? ( Express your answer as :3xx mol e s of H_(2), integer answer is between 0 and 5 0

Find the total number of H, S and 'O' atoms in the following : 5 mole H_(2)S_(2)O_(8)

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.

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.