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A solution of Ni(NO 3 ) 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]

Correct answer

2

Step-by-step 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 : Ni NO 3 2 aq + 2 H + + 2 e - ⟶ Ni + 2 HNO 3 2 F 5 8 . 7 g 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 10 5 C Molar mass of nickel = 58.7g mol -1 1.93 x 10 5 C of charge produces nickel = 58.7g 6000 C of charge produces nickel = 5 8 . 7 g × 6 0 0 0 C 1 . 9 3 × 1 0 5 C = 1 . 8 2 g

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