The quantitiy of electricity required to...

The quantitiy of electricity required to liberate 112 `cm^(3)` of hydrogen at STP from acidified water is

0.1 Faraday

1 faraday

965 coulomb

96500 coulomb

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The quantity of electricity required to release 112 cm^(3) of hydrogen at STP from acidified water is

Electrolysis is the process in which electrical energy is converted to chemical energy. In electrolytic cell, oxidation takes place at anode and reduction at cathode. Electrode process depends on the electrode taken for electrolysis. Amount of substance liberated at an electrode is directly propertional to the amount of charge passed through it. The mass of substance liberated at electrode is calculated using the following relation : m= ("ItE")/(96500) Here, E represents the equivalent mass and 96500 C is called the Faraday constant. Faraday (96500 C) is the charge of 1 mole electron, i.e., 6.023 xx 10^(23) electrons, it is used to liberate one gram equivalent of the substance. The quantity of electricity required to liberate 112 cc hydrogen at S.T.P. from acidified water is :

The quantigy of electricity required to liberate 1 gram equivalent of an element is at

How many moles of electrons are required to liberate 112 L of oxygen at STP when acidulated water is electrolysed ?

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