Question

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

Solution

## Given$$I = 5A$$$$Time = 20 \times 60 = 1200\,\,s$$$$\therefore Charg e = current \times time$$$$\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\, = 5 \times 1200$$$$\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\, = 6000\,\,C$$According to the reaction.$$N{i^{2 + }}\left( {aq.} \right) + 2e \to Ni\,\left( s \right)$$$$Nickel\,\,deposite\,by\, (2 \times 96487)\,C = 58.7\,\,g$$$$\therefore Nickel\,deposite\,by\ 6000\,C = \dfrac{{58.7 \times 6000}}{{2 \times 96487}}$$$$\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\, \quad= 1.825\,\,g$$$$\therefore$$ Hence $$1.825\,g$$ of nickel will be deposited at the cathode.Chemistry

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