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Nernst Equation

A current of ...

Question

A current of $9.65 A$ is passed for $3$ hours between nickel electrodes immersed in $0.5$ dm $^{3}$ solution of concentration $2$ mol dm $^{- 3}$ $N i (N O_{3})_{2}$ .
The molarity of the solution after electrolysis would be :

0.46 M

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0.92 M

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1.25 M

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0.625 M

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Solution

The correct option is C $0.92 M$
The moles of nickel initially present $= \frac{2 m o l}{1 {d m}^{3}} \times 0.5 {d m}^{3} = 1 m o l$ .
The quantity of electricity passed $= Q (C) = 9.65 A \times 10800 s = 104220 C$ .
The moles of electrons passed $= \frac{Q (C)}{96500 (\frac{C}{m o l e^{-}})} = \frac{104220 C}{96500 (\frac{C}{m o l e^{-}})} = 1.08 m o l e^{-}$ .
The moles of Ni deposited $= m o l e r a t i o \times m o l e s o f e l e c t r o n s p a s s e d = \frac{1 m o l N i}{2 m o l e^{-}} \times 1.08 m o l e^{-} = 0.54 m o l$ .
The moles of nickel remaining $= 1 m o l - 0.54 m o l = 0.46 m o l$ .
The molarity of the solution is $\frac{0.46 m o l}{0.5 {d m}^{3}} = 0.92 M .$

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