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Faraday constant ....

Faraday constant __________.

A

is a numerical constant

B

depends on equivalent

C

depends upon the current passed

D

depends on the number of electrons

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The correct Answer is:
A
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It is desired to deposit 0.254 kg of copper on the cathode of a copper voltameter . How long will it take to deposit this amount if a steady current of 100 A is maintained . Use the known value of Faraday constant . Relative atomic mass of copper is 63.5 .

A steady current of 10.0 A is passed through a water voltameter for 300 s . Estimate the volume of H_(2) evolved at standard temperature and pressure . Use the known value of Faraday constant . Relative molecular mass of H_(2) is 2.016 and molar volume = 22.4 litres (volume of 1 mol of an ideal gas at STP).

Faraday's law

A current of 1 A is passed through a dilute solution of sulphuric acid for some time to liberate 1 g of oxygen. How much hydrogen is liberated during this period ? How long the current was passed ? Faraday constant =96500 mol^(-1)

A current of 1 A is possed through a dilute solution of sulphuric acid for some time to liberate 1 g of oxygen. How much hydrogen is liberated during this period? How long was the current passed? Faraday constant = 96500 C mol^(-1) .

Some standard electrode potentials at 298K are given below: To a solution containing 0.001M of X^(2+) and 0.1M of Y^(2+) , the metal rods X and Y are inserted (at298K) and connected by a conducting wire. This resulted in dissolution of X. The correct combinations of X and Y, respectively is (are) (Given: Gas constant, R=8.314JK^(-1)mol^(-1) , Faraday constant,F= 96500C mol^(-1) )

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. How many faradays are required to reduce 1 mol BrO_(3)^(-) to Br^(-) ?

TARGET PUBLICATION-ELECTROCHEMISTRY-CRITICAL THINKING
  1. Faraday first law of electrolysis gives the relation between .

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  2. If the same quantity of electricity is passed through two electrolytes...

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  3. Faraday constant .

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  4. The charge ( in coulombs) on N(3)^(+) ions is ,.

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  5. One coulomb is equal to

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  6. The atomic mass of oxygen is 16, hence the electrochemical equivalent(...

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  7. The number of coulombs required to liberate 0.224 dm^(3) of chlorine a...

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  8. In the electrolysis of water, one faraday of electrical energy would e...

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  9. One Faraday of electricity will liberate half gram atom of the metal f...

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  10. If the atomic mass of M is x, the electrochemical equivalent of M in t...

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  11. When 48250 C of electricity is passed through an aqueous solution of ...

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  12. Mass of copper deposited by the passage of 2 A of current for 965 s th...

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  13. Passage of 96500 coulomb of electricity liberates …… litre of O2 at NT...

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  14. When a current of 3A is passed through an aqueous solution of a pallad...

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  15. The number of molecules of chlorine that would be deposited from molte...

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  16. A metal is know to form fluoride MF(2). When 10A of electricity is pas...

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  17. What will be the current required to deposited on the cathode 39.4 g g...

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  18. How many hour are required for a current of 3.0 ampere to decompose 18...

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  19. Cell-I containing a solution of mercuric percholarate Hg(ClO(4))(2), C...

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  20. When electricity is passed through H(2)SO(4) and CaCl(2) solution , th...

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