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(D) Given that the applied voltage is $2 \ V$,which is greater than the standard reduction potentials of both $Ag^+$ $(0.80 \ V)$ and $Au^+$ $(1.69 \

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silver and gold in proportion to their atomic weights

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(D) Given that the applied voltage is $2 \ V$,which is greater than the standard reduction potentials of both $Ag^+$ $(0.80 \ V)$ and $Au^+$ $(1.69 \ V)$,both metal ions will be reduced at the cathode.According to Faraday's laws of electrolysis,the number of gram equivalents of the substances deposited is equal to the total charge passed through the solution.$gmeq \ Ag = gmeq \ Au$Since $gmeq = \frac{	ext{mass}}{	ext{equivalent weight}}$,we have:$\frac{Wt_{Ag}}{Eqwt_{Ag}} = \frac{Wt_{Au}}{Eqwt_{Au}}$Therefore,the ratio of the masses of silver and gold deposited is equal to the ratio of their equivalent weights,which is proportional to their atomic weights (since both are monovalent ions,$n=1$):$\frac{Wt_{Ag}}{Wt_{Au}} = \frac{Atwt_{Ag}}{Atwt_{Au}}$

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