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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. |
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Answer» `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` |
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