When water is electrolysed, hydrogen and oxygen gas are produced. If 1.008 g of `H_(2)` is liberated at the cathode. What mass of `O_(2)` is formed at the anode?

When water is electrolysed, hydrogen and oxgen gas are produced. If 1.008 g of H_(2) is liberated at cathode, calcualate the mass of O_(2) is formed at anode.

When hydrogen burns is oxygen, water is formed and when water is electrolysed, then hydrogen and oxygen are produced. What type of reaction takes place : (a) in the first case. (b) in the second case ?

If 0.024 L of H_(2) gas is formed at the cathode, the volume of O_(2) gas formed at the anode under identical conditions, is:

In the electrolysis of an aqueous solution of NaOH , 2.8 litres of O_(2)(g) is liberated at the anode at NTP . Volume of hydrogen gas liberated at the cathode at NTP will be

What mass of hydrogen and oxygen will be produced on complete electrolysis of 18 g of water

When molten magnesium oxide was electrolysed for a certain period , 150 mg of Mg was deposited on the cathode . The volume of oxygen gas in cm^3 at STP conditions liberated at the anode during the same period is (Atomic mass of Mg = 24 g mol^(-1) )

When the electrolytis of silver sulphate was carried out by Pt electrodes. 1-6 g oxygen was liberated at the anode, the amount of silver deposited at cathode will be

Copper sulphate solution is electrolysed between two platinum electrodes. A current is passed unit 1.6 g of oxygen is liberated at anode. The amount of copper deposited at the cathode during the same period is:

The electrolysis of hydrochloric acid results in the formation of 1 gm equivalent of H_2 gas at the cathode. The weight of Cl_2 liberated at anode is