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 N i is deposited at the cathode?

Given, Current = 5 A Time = 20 × 60 = 1200 s Charge Q = current i × time t in seconds = 5 × 1200 = 6000 C Now, N i 2 + a q + 2 e - → Ni s 58.7 g ⁡ To convert Ni 2 + to Ni , two moles of electrons are required. Current required = 2 F = 2 × 96500 One mole of nickel = 58.71 g Therefore, nickel deposited by 6000 C = 58.71 × 6000 2 × 96500 g = = 1 . 825 g Hence, 1.825 g of nickel will be deposited at the cathode.

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Chemistry Part I Textbook for Class XII>Chapter -1 - Electrochemistry>Intext Questions>Q 3.7

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