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Electrolysis of a solution of `HSO_4^(-)` ions produces `S_2O_2^(--)`, Assuming 75% current efficiency , what current should be employed to achieve a production rate of 1 mole of `S_2O_6^(--)` per hour ?A. 71.48 AB. 35.7 AC. 142.96 AD. 285.93 A |
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Answer» Correct Answer - A `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` |
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