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  4. A solution of Ni(NO3)2 is electrolyzed 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) [Report your answer by rounding it upto nearset whole number]

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Q. A solution of Ni(NO3)2 is electrolyzed 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)

[Report your answer by rounding it upto nearset whole number]

NTA AbhyasNTA Abhyas 2020Electrochemistry

Solution:

Quantity of electricity used = Current in amperes x Time in second = 5A x (20 x 60) s = 6000 C

Chemical equation for the reaction during electrolysis :

image

Charge Q on n moles of electrons is given by : Q = nF

Charge required to deposit 1 mole nickel

= 2 F = 2 x 96500 C = 1.93 x 105 C

Molar mass of nickel = 58.7g mol-1

1.93 x 105 C of charge produces nickel = 58.7g

6000 C of charge produces nickel $= \frac{\left(5 8 \text{.} 7 \, \text{g}\right) \times \left(6 0 0 0 \, \text{C}\right)}{\left(1 \text{.} 9 3 \times 1 0^{5} \text{ C}\right)}$

$= 1 \text{.} 8 2 \text{ g}$