5. Explain by calculation that what masses of the products will be liberated at electrodes when
nickel nitrate solution is electrolysed using 5 ampere current for 3 hours.
(Atomic mass: Ni-58 g mol-1, O-16 g mol-1)
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ANSWER
Given
I=5A
Time=20×60=1200s
∴Charge=current×time
=5×1200
=6000C
According to the reaction.
Ni
2+
(aq.)+2e→Ni(s)
Nickeldepositeby(2×96487)C=58.7g
∴Nickeldepositeby 6000C=
2×96487
58.7×6000
=1.825g
∴ Hence 1.825g of nickel will be deposited at the cathode.
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