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Charge and Current

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Question

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

1.622 gm

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1.722 gm

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1.822 gm

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1.922 gm

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Solution

The correct option is C 1.822 gm
$N i^{2 +} + 2 e^{-} \to N i$
$t = 20 m i n = 20 \times 60 s e c$
$n = 2$
$i = 5 A$
Atomic Mass of $N i = 58.7$

$m = \frac{A t o m i c M a s s}{n \times F} \times i \times t$

$= \frac{58.7}{2 \times 96500} \times 20 \times 60 \times 5$

$= \frac{352200}{2 \times 96500} = 1.824$

The mass of $N i$ deposited at the cathode is $1.824 g$

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Similar questions

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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A solution of Ni(NO3)2 is electrolyzed between platinum electrodes using a current of 5 amperes for 20 minutes. What mass of Ni is deposited at the cathode?

The correct option is C 1.822 gmNi2++2e−→Nit=20 min=20×60 secn=2i=5 AAtomic Mass of Ni=58.7m=Atomic Massn×F×i×t=58.72×96500×20×60×5=3522002×96500=1.824The mass of Ni deposited at the cathode is 1.824 g

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