An electric current is passed through two electrolytic cells connected in series. One cell contains `Cu^(2+)` and the other contains `Fe^(2+)` . Which of the following is the correct statement?

Options

A. Equal masses of iron and copper are deposited on the electrode
B. More moles of copper are depoosited on the electrode
C. Equal moles of iron and copper are deposited on the electrodes
D. One ampere current for a day would be required to deposit one mole of each metal.

Answer

C

Explanation

In electrolytic cells, reduction of each metal takes place on the respective electrodes `Fe^(2+) + 2e^(-) rarr Fe and Cu^(2+) + 2e^(-) rarr Cu`
Since both the cells are connected in series, equal amount of current passes through the cells. Each mole of iron and copper requires two moles of electrons or 2F current. So, in each cell, equal moles of metal will deposit at a particular time. Considering inert metal electrodes used for the electrolysis, the quantity of electricity passed, `Q = ixx t= 1 xx 24 xx 60 xx 60= 86400 C= (86400)/(96500)F= 0.9F`. Sincce one mole of metal requires 2F current, it will not deposit one mole of any metal