Electrochemistr...

The passage of current through a solution of certain electrolye results in the evolution of H₂ at cathode and Cl₂ at anode. The electrolytic solution is -

In an electrolytic cell current flows from -

When an aqueous solution of H₂SO₄ is electrolysed, the ion discharged at anode is-

1 mole of Al is deposited by X coulomb of electricity passing through aluminium nitrate solution. The number of moles of silver deposited by X coulomb of electricity from silver nitrate solution is-

A solution of Na₂SO₄ in water is electrolysed using Pt electrodes.The products at the cathode and anode are respectively -

In electrolysis of a fused salt, the weight deposited on an electrode will not depend on-

The electrolysis of a solution resulted in the formation of H₂ at the cathode and Cl₂ at the anode. The liquid is-

Which loses charge at cathode-

In the electrolysis of CuSO₄, the reaction :

Cu²⁺ + 2e¯ → Cu, takes place at :

If mercury is used as cathode in the electrolysis of aqueous NaCl solution, the ions discharged at cathode are-

The specific conductance of a solution is 0.3568 ohm^-1. When placed in a cell the conductance is 0.0268 ohm^-1. The cell constant is-

A conductance cell was filled with a 0.02 M KCl solution which has a specific conductance of 2.768 × 10^-3 ohm^-1 cm^-1. If its resistance is 82.4 ohm at 25ºC, the cell constant is-

The variation of equivalent conductance vs decrease in concentration of a strong electrolyte is correctly given in the plot -

Which of the following solutions has the highest equivalent conductance ?

The resistance of 0.01N solution of an electrolyte AB at 328K is 100 ohm. The specific conductance of solution is (cell constant = 1cm^-1) -

For an electrolytic solution of 0.05 mol L^-1, the conductivity has been found to be 0.0110 Scm^-1.The molar conductivity is-

Two electrodes are fitted in conductance cell 1.5 cm apart while the area of cross section of each electrode is 0.75 cm². The cell constant is-

The best conductor of electricity is in 1M solution of-

A certain current liberates 0.504 g of H₂ in 2 hours. How many grams of copper can be liberated by the same current flowing for the same time in CuSO₄ solution -

A currnet of 2.6 ampere is passed through CuSO₄ solution for 6 minutes 20 seconds. The amount of Cu deposited is (At. wt. of Cu = 63.5, Faraday = 96500 C)-

Three Faradays of electricity are passed through molten Al₂O₃, 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 :