A solution of Ni(NO_{3})_{2} is electrolysed | vedclass

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(A) Given:Current $(I) = 5 \, A$Time $(t) = 20 \, minutes = 20 	imes 60 = 1200 \, s$Charge $(Q) = I 	imes t = 5 	imes 1200 = 6000 \, C$The electrod

Vedclass · Accepted Answer

$1.825$

Vedclass · Answer

(A) Given:Current $(I) = 5 \, A$Time $(t) = 20 \, minutes = 20 	imes 60 = 1200 \, s$Charge $(Q) = I 	imes t = 5 	imes 1200 = 6000 \, C$The electrode reaction for the deposition of $Ni$ is:$Ni^{2+} + 2e^{-} 	o Ni$From the reaction,$2 \, mol$ of electrons are required to deposit $1 \, mol$ of $Ni$.$2 	imes 96487 \, C$ of charge deposits $58.71 \, g$ of $Ni$.Mass of $Ni$ deposited by $6000 \, C = \frac{58.71 	imes 6000}{2 	imes 96487} \, g$$= 1.825 \, g$Thus,$1.825 \, g$ of $Ni$ is deposited at the cathode.

$A$ solution of $Ni(NO_{3})_{2}$ is electrolysed between platinum electrodes using a current of $5 \, A$ for $20 \, minutes$. What mass of $Ni$ is deposited at the cathode (in $, g$)?

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