4Fe(s) + 3O2(g) → 2Fe2O3(s)
Identify the type of chemical reaction represented by this equation.
is it redox?
Yes, the given equation represents a redox (reduction-oxidation) chemical reaction. In this reaction, iron (Fe) is being oxidized by oxygen (O2) to form iron(III) oxide (Fe2O3).
Yes, the chemical equation you provided represents a redox (reduction-oxidation) reaction. In a redox reaction, there is a transfer of electrons between the reactants.
To determine if a reaction is redox, you should first identify the oxidation states of the elements in the reactants and products. In this equation, the oxidation state of Fe changes from 0 on the left-hand side to +3 in Fe2O3 on the right-hand side. Similarly, the oxidation state of O changes from 0 on the left-hand side to -2 in Fe2O3 on the right-hand side.
The oxidation state of an element represents the hypothetical charge an atom would have if all the shared electrons were assigned to the more electronegative atom in a compound. In Fe(s), Fe has an oxidation state of 0 because it is in its elemental state, and in O2(g), O has an oxidation state of 0 because it is also in its elemental state. However, in Fe2O3(s), Fe has an oxidation state of +3 because it loses 3 electrons and O has an oxidation state of -2 because it gains 2 electrons.
Since the oxidation states of Fe and O change in this reaction, it is classified as a redox reaction. Furthermore, the equation represents a synthesis reaction because the reactants combine to form a single product.
yes
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yes