Completely analyze the following reaction from a redox perspective.
3CO(g) + Fe 2 O 3 (s) → 3CO 2 (g) + 2Fe(s)The change in the oxidation states of the elements is shown.Remember
The reducing agent is oxidized.
The oxidizing agent is reduced.Since the oxidation state of carbon is increasing from +2 to +4, it is being
oxidized, its responsibility for electrons is decreasing, and the compound of
which it is a part, carbon monoxide, is called the reducing agent. Carbon
monoxide is a common reducer because of its chemical desire to turn into carbon
dioxide when oxygen becomes available from other substances. On the other
hand, the oxidation state of iron is decreasing from +3 to 0, it is being reduced, its
responsibility for electrons is going up, and the compound of which it is a part,
iron(III) oxide, is called the oxidizing agent.
COMBUSTION REACTIONS
Combustion reactions are those chemical processes in which substances (called
fuels) are rapidly oxidized, accompanied by the release of heat and usually light.
Combustion is also referred to as burning. Typical, common, and historically
well-known combustion reactions involve using oxygen as the oxidizing agent—
hence, the name for the process of losing electrons has became known as
oxidation. When a combustion reaction is complete, the elements in the burning
fuel form compounds with the oxidizing agent and the responsibility for electrons
changes.
The reaction between magnesium and oxygen is a common example of
combustion. When the reaction occurs
2Mg(s) + O 2 (g) → 2MgO(s)the oxidation states of magnesium and oxygen change from 0 each to +2 and −2,
respectively. A blinding light and large quantity of heat is released by the system
as the reaction unfolds. The amount of heat released when 1 mole of a fuel burns
is referred to as its heat of combustion and is symbolized ΔHc. The ΔHc for Mg
is 602 kJ/mol. The change in enthalpy associated with the burning of 1 mole of