# The current of 9.65A is drawn from a Daniell cell for exactly 1h.If molar masses of Cu and Zn are $63.5gmol^{-1}$ and $6.54gmol^{-1}$,respectively,the loss in mass at anode and gain in mass at cathode,respectively,are

$\begin{array}{1 1}11.43g.11.77g\\11.77g,11.43g\\22.86g,23.54g\\23.54g,22.86g\end{array}$

Answer : $11.77g,11.43g$
The reaction occurring in Daniell cell is $Zn+Cu^{2+}\rightarrow Zn^{2+}+Cu$
Zinc is lost at anode and Cu is deposited at cathode.
Amount of current withdrawn is $(9.65A)(60\times 60s)/(96500Cmol^{-1})$,which is 0.36mol.Since two electrons are involved in the reduction and oxidation reactions,0.18mol of zn is lost at anode and 0.18mol of Cu is deposited at cathode.The masses are 11.77g and 11.43g for Zn and Cu,respectively.