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A current of 1.50 A was through an elect...

A current of `1.50` A was 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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The correct Answer is:
893.5 s
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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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A current of 2 ampere was passed through solutions of CuSO_4 and AgNO_3 in series. 0.635 g of copper was deposited. Then the weight of silver deposited will be-

(a) A steady current of 2 amperes was passed through two electrolytic cells X and Y connected in series containing electrolytes FeSO_(4) and ZnSO_(4) until 2.8 g of Fe deposited at the cathode of cell X. How long did the current flow ? Calculate the mass of Zn deposited at the cathode of cell Y (Molar mass : Fe= 56 g mol^(-1) Zn-65.3g mol^(-1) , 1F -96500 C mol^(-1) ) (b) In the plot of molar conductivity (wedge_(m)) vs Square root of concentration (c^(1//2)) , following curves are obtained for two electrolytes. A and B: Answer the following : (i) Predict the nature of electrolytes A and B. (ii) What happens on extrapolation of wedge_(m) to concentration approaching zero for electrolytes A and B ?

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