What are the oxidation and reduction equations for the following equations: Zn(s) + 2H2O(l) → Zn(OH)2(s) + H2(g) ?

1 Answer

Answer:

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

Explanation:

Zinc can be readily oxidized.........

#Zn(s) rarr Zn^(2+) + 2e^(-)# #(i)#

Hydrogen ion, as the #"acidium ion"# in water is commonly represented as #H_3O^+#, or even, more simply as #H^+#. Let's take the former..........

#H_3O^+ + e^(-) rarr1/2H_2(g) + H_2O(l)# #(ii)#

We add the individual redox equations in such a way that electrons do NOT appear.........i.e. #(i) + 2xx(ii)#

#Zn(s) +2H_3O^+ rarr Zn^(2+) + 2H_2O(l) + H_2(g)uarr#

Charge is balanced, and mass is balanced, as is required for any stoichiometric equation...........any representation of reality.