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

Options

A. 71.48 A
B. 35.7 A
C. 142.96 A
D. 285.93 A

Answer

A

Explanation

`2HSO_4^(-)toS_2O_8^(--)+2H^(+)+2e^(-)`
so required rate =1 mole / hr
2 mole of `e^(-)`/hr
`=(2xx96500)/(3600 sec)=(2xx965)/36A=53.61 A`
so required current =`4/3xx53.61 A=71.48 A`