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

1 Answer
Jul 10, 2017

Answer:

#"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#