Ncert Exercises & Solutions

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

Hint: use Faraday’s Laws of Electrolysis

Step 1:

Given,

Current=5 A

Time=20 x 60=1200 s

∴

Charge=current x time

= 5 x 1200

=6000 C

Step 2:

According to the reaction,

{Ni}^{2 +}_{(aq)} + 2 e^{-} \to {Ni}_{(s)}

58.7 g

Nickel deposited by 2 x 96487 C=58.71 g

Therefore, nickel deposited by 6000 C=

\frac{58.71 \times 6000}{2 \times 96487} g

=1.825 g

Hence, 1.825 g of nickel will be deposited at the cathode.

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