250 mL of a waste solution obtained from the | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(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 \

Vedclass · Accepted Answer

silver and gold in proportion to their atomic weights

Vedclass · Answer

(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,$n=1$):$\frac{Wt_{Ag}}{Wt_{Au}} = \frac{Atwt_{Ag}}{Atwt_{Au}}$

Similar Questions

The number of moles of electrons required to deposit $1 \, g$ equivalent of aluminium $(At. \, wt. = 27)$ from a solution of aluminium chloride will be

Copper is to be electrodeposited on a nickel block of $(20 \times 5) \ cm^2$ area by using $CuSO_4$ as electrolyte. How much quantity of electricity is needed to deposit a $3.6 \ \mu m$ layer of copper (in $C$)? [Atomic weight of $Cu = 63.5 \ g \ mol^{-1}$,Density of $Cu = 8.9 \ g/cm^3$]

If $96500 \ C$ of electricity liberates one gram equivalent of any substance,the time taken for a current of $0.15 \ A$ to deposit $20 \ mg$ of copper from a solution of copper sulphate is (Chemical equivalent of copper = $32$).

How much time (in $sec$) is required to coat a metal surface of $80 \, cm^2$ with a $0.005 \, mm$ thick layer of silver from a silver nitrate solution using a current of $3 \, A$? (Density of silver $= 10.5 \, g \, cm^{-3}$)

What mass of silver (Atomic mass = $108 \text{ g/mol}$) is deposited by a quantity of electricity that displaces $5600 \text{ mL}$ of $O_2$ gas at $STP$ (in $\text{ g}$)?

Vedclass Test Series

Exam Paper Generator

Online Exam Module