Electrochemistr...

Three Faradays of electricity are passed through molten Al₂ O₃ , aqueous solution of CuSO₄  and molten NaCl taken in three different electrolytic cells. The amount of Al, Cu and Na deposited at the cathodes will be in the ratio of-

The quantity of electricity required to liberate 0.01g equivalent of an element at the electrode is-

The unit of electrochemical equivalent is-

One faraday of electricity will liberate one mole of metal from a solution of-

The number of faraday required to generate 1 mole of Mg from MgCl₂  is-

One gm metal M⁺²  was discharged by the passage of 1.81 ×10²²  electrons. What is the atomic weight of metal?

One mole of electron passes through each of the solution of AgNO₃ , CuSO₄  and AlCl₃  when Ag, Cu and Al are deposited at cathode. The molar ratio of Ag, Cu and Al deposited are

Salts of A (atomic weight = 7), B (atomic weight = 27) and C (atomic weight = 48) were electrolysed under identical conditions using the same quantity of electricity. It was found that when 2.1 g of A was deposited, the weights of B and C deposited were 2.7 and 7.2 g. The valencies of A, B and C respectively are

The density of Cu is 8.94 g cm^–3 . The quantity of electricity needed to plate an area 10 cm ×10cm to a thickness of 10^-2  cm using CuSO₄  solution would be

During electrolysis of an aqueous solution of sodium sulphate if 2.4 L of oxygen at STP was liberated at anode. The volume of hydrogen at STP, liberated at cathode would be :