• # question_answer $A{{l}_{2}}{{O}_{3}}$is reduced by electrolysis at low potentials and high currents. If $4.0\times {{10}^{4}}$amperes of cur- rent is passed through molten $A{{l}_{2}}{{O}_{3}}$for 6 hours, what mass of aluminium is produced? (Assume 100% current efficiency. At mass of Al = 27g $mo{{l}^{-1}}$) A) $1.3\times {{10}^{4}}g$B) $1.3\times {{10}^{4}}g$C) $8.05\times {{10}^{4}}g$D) $2.4\times {{10}^{5}}\,g$

Eq. of Al formed $=\frac{m}{F}=\frac{it}{96500}$ $\therefore$ ${{m}_{Al}}=\frac{4\times {{10}^{4}}\times 6\times 60\times 60\times 27}{96500\times 3}\left( E=\frac{27}{3} \right)$ $\therefore$${{m}_{Al}}=8.05\times {{10}^{4}}g$