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Answer 1 · 2016-10-09T09:45:03

Do you speak of a redox reaction?

When aluminum chloride is formed, we conceive that aluminum metal is oxidized:

$Al(s) rarr Al^(3+) + 3e^-$ $(i)$

And gaseous chlorine is reduced:

$1/2Cl_2(g) + e^(-) rarr Cl^-$ $(ii)$

As with any chemical reaction, both MASS and CHARGE are conserved.

TO represent the formation of $"aluminum chloride"$ , we simply add, $(i)+3xx(ii)$ :

$Al(s) + 3/2Cl_2(g) rarr AlCl_3(s)$

And of course mass and charge have been conserved, as required.