Electrolysis of molten magnesium chloride results in the formation of 0.4 g magnesium. Calculate the volume of chlorine liberated during the reaction at STP. When an electrolytic cell consisting of molten `AlCl_(3)` and molten `NaCl` are connected in series with the above cell, calculate the amount of aluminium and sodium deposited at cathode.

Explanation

`MgCl_(2) rarr Mg^(+2) + 2C^(-)`
For the deposition for 12 g of Mg (equivalent weight of magnesium) one faraday is required
`:.` 12 g requires 1 faraday
0.4 g requires ?
`= (0.14)/(12) = 0.03` Faraday
1 Faraday gives 11.2 L of `Cl_(2)` at STP, therefore, 0.03 faraday gives ?
`= 0.336 1 L " of " Cl_(2)` at STP
1 faraday required to deposit 9 g of Al
`:.` 0.03 faraday required to deposit ? = 0.27 g
1 faraday required to deposit 23 g of Na
`:.` 0.03 faraday required to deposit ?
`= 0.03 xx 23 = 0.69 g`