A solution of `CuSO_(4)` is electrolyzed for `10 ` min with a current of `1.5A`. What is the mass of `Cu` deposited at the cathode? `[` Atomic mass of `Cu=63g]`
A solution of CuSO_(4) is electrolsed for 10 minutes with a current of 1.5 amperes. What is the mass of copper deposited at the cathode ? (Molar mass of Cu=63.5 g//mol)
A solution of CuSO_(4) is electrolysed for 10 minutes with a current of 1.7 amperes. What is the mass of copper deposited at the cathode? (Molar mass of Cu= 63.5g/mol).
A solution of Ni(NO_(3))_(2) is electrolyzed between platium electrodes using a current of 5A for 20 mi n . What mass of Ni is deposited at the cathode ?
A solution of Ni (NO_(3))_(2) was electrolysed between platinum electrodes using current of 5 amp for 30 min . What is the mass of Ni deposited at the cathode ?
A solution of Ni(NO_(3))_(2) is electrolyzed between platinum electrodes using a current of 5 amperes for 20 min. What mass of Ni is deposited at the cathode? (Atomic mass of Ni = 58.7) [Report your answer by rounding it upto nearset whole number]
Two Faraday of electricity is passed through solution of CuSO_(4) . The mass of copper deposited at the cathode is : (Atomic mass of Cu = 63.5 amu)
