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A solution of Ni(NO(3))(2) is electrolys...

A solution of `Ni(NO_(3))_(2)` is electrolysed between platinum electrodes using a current of 5A for 20 min. What mass of Ni is deposited at the cathode?

Text Solution

Verified by Experts

Here, current = 5A, time = 20 min
Quantity of electricity passed will be
`Q = i t = 5A xx 20 xx 60s = 6000 C`
Electrolysis of `Ni(NO_(3))_(2)` gives
`Ni^(2+) + 2e^(-) rarr Ni` ( Atomic mass of Ni = 58.7 )
Therefore, electricity required for 1 mole,
i.e. 58.7 g Ni is 2F` = 2xx 96500C`
`:. 2 xx 96500 C` deposit Ni = 58.7g
`:. ` 6000 C will deposit Ni `= ( 58.7 xx 6000)/( 2 xx 96500) g = 1.825g`
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