Calculate the mass of aluminium produced when a 6.80 A current is applied to AlCl3 (l) for 1.50 hours.,?

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1 Answer
Michael
Apr 9, 2018

3.4 g

Explanation:

Aluminium is discharged:

#sf(Al^(3+)+3erarrAl)#

This means that 1 mole of Al requires 3 moles of electrons to be discharged.

#sf(Q=It)#

So the charge passed #sf(=6.80xx1.5xx60 xx60=36,720color(white)(x)C)#

The charge on a mole of electrons is referred to the Faraday and = #sf(9.65xx10^(4)color(white)(x)"C/"mol)#

#:.##sf(3Frarr27gcolor(white)(g)Al)#

#sf(3xx9.65xx10^(4)Crarr27g)#

#sf(28.95xx10^(4)Crarr27g)#

#:.##sf(1Crarr(27)/(28.94xx10^(4))color(white)(x)g)#

#sf(36,720Crarr(27xx36,720)/(28.94xx10^(4))color(white)(x)g)#

#sf(=3.4color(white)(x)g)#

This is not a good question as solid aluminium chloride sublimes on heating so the electrolyte cannot be molten as described. A better choice would be a solution of aluminium nitrate or similar.

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