What is the quantity of electricity (in Coulo | vedclass

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(B) The number of moles of $AgNO_3$ is calculated as: $n = M 	imes V(L) = 1 \ M 	imes 0.25 \ L = 0.25 \ mol$.The reduction reaction is: $Ag^+ + e^-

Vedclass · Accepted Answer

$24125$

Vedclass · Answer

(B) The number of moles of $AgNO_3$ is calculated as: $n = M 	imes V(L) = 1 \ M 	imes 0.25 \ L = 0.25 \ mol$.The reduction reaction is: $Ag^+ + e^- ightarrow Ag(s)$.Since $1 \ mol$ of $Ag^+$ requires $1 \ mol$ of electrons $(1 \ Faraday = 96500 \ C)$ to deposit $1 \ mol$ of $Ag$,the electricity required for $0.25 \ mol$ is:$Q = n 	imes F = 0.25 \ mol 	imes 96500 \ C/mol = 24125 \ C$.

What is the quantity of electricity (in Coulombs) required to deposit all the silver from $250 \ mL$ of $1 \ M \ AgNO_3$ solution?

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