When a current of 0.1 , A is passed through 2 | vedclass

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(D) The number of equivalents of $Ag^+$ in $200 \, mL$ of $0.1 \, N$ $AgNO_3$ solution is given by: $Equivalents = N 	imes V(L) = 0.1 	imes 0.2 = 0.

Vedclass · Accepted Answer

$9650$

Vedclass · Answer

(D) The number of equivalents of $Ag^+$ in $200 \, mL$ of $0.1 \, N$ $AgNO_3$ solution is given by: $Equivalents = N 	imes V(L) = 0.1 	imes 0.2 = 0.02 \, eq$. Since $Ag^+$ is a monovalent ion,the number of moles of $Ag$ is equal to the number of equivalents,which is $0.02 \, mol$. To remove half of the silver,we need to deposit $0.02 / 2 = 0.01 \, mol$ of $Ag$. According to Faraday's law,the charge $Q$ required is $Q = n 	imes F$,where $n$ is the number of moles and $F$ is Faraday's constant $(96500 \, C/mol)$. $Q = 0.01 	imes 96500 = 965 \, C$. Using the relation $Q = I 	imes t$,where $I = 0.1 \, A$: $965 = 0.1 	imes t$. $t = 965 / 0.1 = 9650 \, sec$.

When a current of $0.1 \, A$ is passed through $200 \, mL$ of a $0.1 \, N$ $AgNO_3$ solution,silver is deposited. How much time in $sec$ is required to remove half of the silver from the solution?

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