Question

Question #708cb

Answer 1

Do you speak of a redox reaction?

Explanation:

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.