An electrolytic cell contains a solution of `Ag_(2)SO_(4)` and have platinum electrodes. A current is passed until 1.6gm of `O_(2)` has been liberated at anode. The amount of silver deposited at cathode would beA. 107.88 gmB. 1.6 gmC. 0.8 gmD. 21.60 gm

An electrolytic cell contains a solution of `Ag_(2)SO_(4)` and have pl

1.	An electrolytic cell contains a solution of `Ag_(2)SO_(4)` and have platinum electrodes. A current is passed until 1.6gm of `O_(2)` has been liberated at anode. The amount of silver deposited at cathode would beA. 107.88 gmB. 1.6 gmC. 0.8 gmD. 21.60 gm
Answer» Correct Answer - D At cathode: `Ag^(+)+e^(-)toAg` At anode: `2OH^(-)tH_(2)O+(1)/(2)O_(2)+2e^(-)` `E_(Ag)=(108)/(1)=108,E_(O_(2))=((1)/(2)xx32)/(2)=8` `(W_(Ag))/(E_(Ag))=(W_(O_(2)))/(E_(O_(2))),W_(Ag)=(1.6xx108)/(8)=21.6gm`

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An electrolytic cell contains a solution of `Ag_(2)SO_(4)` and have platinum electrodes. A current is passed until 1.6gm of `O_(2)` has been liberated at anode. The amount of silver deposited at cathode would beA. 107.88 gmB. 1.6 gmC. 0.8 gmD. 21.60 gm

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