The mass of silver (Molar mass of Ag: 108 g | vedclass

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Question

(A) According to Faraday's law of electrolysis,the number of equivalents of substances deposited or liberated by the same quantity of electricity are

Vedclass · Accepted Answer

$108$

Vedclass · Answer

(A) According to Faraday's law of electrolysis,the number of equivalents of substances deposited or liberated by the same quantity of electricity are equal.$Eq. 	ext{ of } Ag = Eq. 	ext{ of } O_2$For $O_2$ gas,the reaction is: $2H_2O ightarrow O_2 + 4H^+ + 4e^-$.The $n$-factor for $O_2$ is $4$.Number of moles of $O_2 = \frac{5600 \ mL}{22400 \ mL \ mol^{-1}} = 0.25 \ mol$ (using $S.T.P.$ molar volume as $22.4 \ L \ mol^{-1}$).$Eq. 	ext{ of } O_2 = 	ext{moles} 	imes n	ext{-factor} = 0.25 	imes 4 = 1$.For $Ag^+ + e^- ightarrow Ag$,the $n$-factor is $1$.$Eq. 	ext{ of } Ag = \frac{	ext{mass}}{	ext{molar mass}} 	imes n	ext{-factor} = \frac{x}{108} 	imes 1$.Equating the two: $\frac{x}{108} = 1$.$x = 108 \ g$.

The mass of silver (Molar mass of $Ag: 108 \ g \ mol^{-1}$) displaced by a quantity of electricity which displaces $5600 \ mL$ of $O_2$ at $S.T.P.$ will be . . . . . . $g$.

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