Three litres of 0.5 M `K_(2)Cr_(2)O_(7)` soluton have to be completely reduced in th acidic medium. The number of faradays of electricity required will be.

Three litres of 0.5 M `K_(2)Cr_(2)O_(7)` soluton have to be completely

1.	Three litres of 0.5 M `K_(2)Cr_(2)O_(7)` soluton have to be completely reduced in th acidic medium. The number of faradays of electricity required will be.
Answer» 3L of 0.5 M `K_(2)Cr_(2)O_(7)` solution will contain `0.5xx3=1.5` moles of `K_(2)Cr_(2)O_(7)`. The reduction reaction is `Cr_(2)O_(7)^(2-)+14H^(+)+6e^(-)toCr^(3+)+7H_(2)O` thus, 1 mole of `Cr_(2)O_(7)^(2-)` requires 6 F of electricity. `therefore1.5` mole will require electricity=9F.

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Three litres of 0.5 M `K_(2)Cr_(2)O_(7)` soluton have to be completely reduced in th acidic medium. The number of faradays of electricity required will be.

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