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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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