An aqueous solution of ferrous sulphate is taken and subjected to electrolysis. Calculate the number of electrons flowing through the circuit when 0,7 g of iron is deposited at cathode (atomic mass of Fe = 56)

An aqueous solution of ferrous sulphate is taken and subjected to elec

1.	An aqueous solution of ferrous sulphate is taken and subjected to electrolysis. Calculate the number of electrons flowing through the circuit when 0,7 g of iron is deposited at cathode (atomic mass of Fe = 56)
Answer» Solution :EQUIVALENT mass of IROM `= (56)/(2) = 28` `(FE^(+2) + 2e^(-) rarr Fe)` 1 faraday of electricity is required to deposit 28 g of iron. 1 faraday charge is required to deposit `6.023 xx 10^(23)` ELECTRONS. `:.` 28 g of Fe required to deposit `6.023 xx 10^(23)` electrons. 0.7 g of Fe required to deposit `= (6.023 xx 10^(23) xx 0.7)/(28) = 1.5 xx 10^(23)` electrons