Question

The oxidation and reduction equations for when zinc is placed in water?

Answer 1

`"Oxidation:"` `Zn(s)rarrZn^(2+) + 2e^(-)` `(i)`

Explanation:

Water COULD be reduced.........

`H_2O + e^(-) rarr 1/2H_2(g)uarr +HO^-` `(ii)`

We add (i) and (ii) such that the electrons are eliminated from the reaction.......

`(i) + 2xx(ii)`

`Zn(s) + 2H_2O rarr Zn^(2+) + H_2(g)uarr +2HO^-`

We would need exceptionally clean and pure zinc metal for this reaction to occur, but in the presence of acid.......we could simply write.....

`Zn(s) +2HCl(aq) rarr ZnCl_2(aq) + H_2(g)uarr`