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Standard XII

Chemistry

Faraday's First Law

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Question

A solution of $N i (N O_{3})_{2}$ is electrolysed between platinum electrodes using a current of 5 amperes for 20 min. What mass of Ni is deposited at the cathode ? (Atomic mass of Ni = 58.7)

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Solution

Quantity of elctricity used = Current in amperes $\times$ Time in second $= 5 A \times (20 \times 60) s = 6000 C$
Chemical equation for the reaction during electrolysis :
$N i (N O_{3})_{2} (a q) + 2 H^{+} + 2 e^{-} 2 F \to N i 58.7 g + 2 H N O_{3}$
Charge Q on n moles of electrons is given by : Q =nF
Charge required to deposit 1 mole nickel
$= 2 F = 2 \times 96500 C = 1.93 \times 10^{5} C$
Molar mass of nickel $= 58.7 g m o l^{- 1}$
$1.93 \times 10^{5} C o f c h a r g e p r o d u c e s n i c k e l = 58.7 g$
6000 C of charge produces nickel $= \frac{(58.7 g) \times (6000 C)}{(1.93 \times 10^{5} C)} = 1.825 g$

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Faraday's First Law

Standard XII Chemistry

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A solution of Ni(NO3)2 is electrolysed between platinum electrodes using a current of 5 amperes for 20 min. What mass of Ni is deposited at the cathode ? (Atomic mass of Ni = 58.7)

A solution of $N i (N O_{3})_{2}$ is electrolysed between platinum electrodes using a current of 5 amperes for 20 min. What mass of Ni is deposited at the cathode ? (Atomic mass of Ni = 58.7)