Question

One of the most recognizable corrosion reactions is the rusting of iron. rust is caused by iron reacting with oxygen gas in the presence of water to create an oxide layer. iron can form several different oxides, each having its own unique color. red rust is caused by the formation of iron(iii) oxide trihydrate. in the space provided, write the balanced reaction for the formation of fe2o3•3h2o(s). phases are optional.

Answer 1

Answer:  $Fe(s) + 6H_2O(l) + 3O_2(g)  -> 4Fe(OH)_3(s)$

Explanation:

The Chemical equation for the formation of rust is:

Iron + Water + Oxygen ----> Rust

4 Fe(s) + 6 H2O(l) + 3 O2(g) → 4 Fe(OH)3(s)

The Iron Hydroxide However dehydrates to produce Fe2O3 * nH2O

Answer 2

Answer : The balanced chemical reaction for rusting of irons is :

$4Fe(s)+3O_2(g)+6H_2O(l)\rightarrow 2[Fe_2O_3(s).3H_2O(s)]$

Explanation :

Iron rusting : It is a type of chemical process where an iron nail react with the water in the presence of moisture (oxygen) to give iron oxide as a product. Rusting of iron is an oxidation-reduction reaction in which iron losses electrons to oxygen atom.

Oxidation reaction : It is the reaction in which a substance looses its electrons. In this oxidation state increases.

Reduction reaction : It is the reaction in which a substance gains electrons. In this oxidation state decreases.

The balanced chemical reaction for rusting of irons is :

$4Fe(s)+3O_2(g)+6H_2O(l)\rightarrow 2[Fe_2O_3(s).3H_2O(s)]$

Half reactions of oxidation and reduction are :

Oxidation : $Fe(s)\rightarrow Fe^{3+}+3e^-$

Reduction : $\frac{1}{2}O_2+2e^-\rightarrow O^{2-}$