What is the time (in sec) required for deposi | vedclass

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(B) The reaction for the deposition of silver is: $Ag^+ + e^- ightarrow Ag(s)$.Number of moles of $Ag^+$ ions $= 	ext{Molarity} 	imes 	ext{Volume

Vedclass · Accepted Answer

$50$

Vedclass · Answer

(B) The reaction for the deposition of silver is: $Ag^+ + e^- ightarrow Ag(s)$.Number of moles of $Ag^+$ ions $= 	ext{Molarity} 	imes 	ext{Volume in Liters} = 1 \ M 	imes 0.125 \ L = 0.125 \ mol$.Since $1 \ mol$ of $Ag^+$ requires $1 \ mol$ of electrons $(1 \ F)$ for deposition,the total charge $Q$ required is $0.125 \ F$.$Q = 0.125 	imes 96500 \ C = 12062.5 \ C$.Using the formula $Q = I 	imes t$,where $I = 241.25 \ A$:$t = \frac{Q}{I} = \frac{12062.5 \ C}{241.25 \ A} = 50 \ sec$.

What is the time (in $sec$) required for depositing all the silver present in $125 \ mL$ of $1 \ M \ AgNO_3$ solution by passing a current of $241.25 \ A$? $(1 \ F = 96500 \ C)$

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