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)

Explanation

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