`30 mL` of `0.13 M NiSO_(4)` is electrolysed using a current of `360` milliamperes for `35.3` minutes. The mass of the metal that would have been plated out if current efficiency is only `60%` (`Ni = 58.7 u`) is

State and explain Faradays laws of electrolysis ? A solution of Ni (NO_3)_2 is electrolysed between platinum electrodes using a current of 5,0 ampere for 30 minutes . Calculate the mass of nickel produced at the cathode at mass of Ni = 58.7 )

A solution of Ni(NO_3)_2 is electrolysed between platinum electrodes using a current of 5 amperes for 20 minutes. What mass of nickel is deposited at the cathode?[molar mass of Ni = 58.7gma " mol"^(-1) ]

A solution of Ni(NO3)_2 is electrolyzed between platinum electrodes using a current of 5.0 amperes for 20 minutes. What weight of Ni will be produced at cathode ? The atomic mass of Ni = 58.7 a.m.u ?

500 ml CuSO_(4) solution was electrolysed using a current of 2 amp (efficiency =75%) for 60 min calculate the pH of solution at the end of electrolysis (Assume initial pH=7)

500 ml CuSO_(4) solution was electrolysed using a current of 2 amp (efficiency =75%) for 60 min calculate the pH of solution at the end of electrolysis (Assume initial pH=7)