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Faraday constant...

Faraday constant

A

depends on the amount of the electrolyte

B

depends on the current in the electrolyte

C

is a universal constant

D

depends on the amount of charge passed through the electrolyte

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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) .

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 .

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^(-) ?

Consider the following cell reaction Cd_(s)+Hg_(2)SO_(4)+9/5H_(2)O_(l) rarr CdSO_(4).9/5H_(2)O_(s)+2Hg_(l) The value of E_(cell)^(0) n is 4.315 V at 25^(@) C. If triangleH^(@) = - 825.2 kj "mol"^(-1) the standard entropy change triangleS^(@) in J K^(-1) is_________ (Nearest integer) [Given : Faraday constant = 96487 C "mol"^(-1) ]

A study potential difference of 1.62 V is maintained across two Pt electrodes placed in a solution of CuCl_(2) . At the end of 600s, the mass of copper deposited on the cathode is measured to be 5.92 g. The back emf of the voltameter is given to be 1.34 V. Estimate the resistance of voltameter. Faraday constant =96500 C mol^(-1) , relative atomic mass of copper =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).

Suppose that gold is being plated on to another metal in an electrolytic cell. The half - cell reaction producing the Au(s) is AuCl_(4)^(-)+3e^(-)+Au(s)+4Cl^(-) . If a 0.30 A current runs for 15.00 minute, what mass of Au(s) will be plated, assume all the electrons are used in the reduction of AuCl_(4)^(-) ? the Faraday constant is 96485 C/mol and molar mass of Au is 197.