A current of `1.50` A was passed through an electrolytic cell containing `AgNO_3` solution with inert electrodes. The weight of silver deposited was `1.50g`. How long did the current flow ? (Molar mass of `Ag=108 g " mol "^(-1), 1F=96500C " mol" ^(-1)`).

A current of `1.50` A was passed through an electrolytic cell containi

1.	A current of `1.50` A was passed through an electrolytic cell containing `AgNO_3` solution with inert electrodes. The weight of silver deposited was `1.50g`. How long did the current flow ? (Molar mass of `Ag=108 g " mol "^(-1), 1F=96500C " mol" ^(-1)`).
Answer» Current (F)` =1.50A` `W=1.50g` `t=?` Molar mass (M)`=108//mol` `1F=96500C//mol` `W=ZIT=("Equiy weight")/(96500)xxIxxT" "[Eq. weight =(108)/(I)]` `1.50=(108)/(96500)xx1.50xxt` `t=(96500)/(108)=893.52Sec`.

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A current of `1.50` A was passed through an electrolytic cell containing `AgNO_3` solution with inert electrodes. The weight of silver deposited was `1.50g`. How long did the current flow ? (Molar mass of `Ag=108 g " mol "^(-1), 1F=96500C " mol" ^(-1)`).

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