Write a chemical equation of Dr. Jeff’s demonstration using a battery to light steel wool on fire. The battery is used to allow a current to travel through the steel wool, thus heating it up. Steel wool is made from iron (Fe).

The chemical equation for the combustion of steel wool is as follows:

4 Fe (s) + 3 O₂ (g) > 2 Fe₂O₃ (s)

Steel wool is an alloy of iron and carbon. It is composed mostly of iron though (about 98%) and only about 2% carbon.

The iron threads in steel wool creates a large surface area for reaction.

A battery is used to light the steel wool when the terminals of the battery touch the steel wool.

An electric circuit is set up around the thin wire which heats up to a high temperature of about 700°C (700 degrees C).

These high temperatures cause the iron to react with the oxygen present around the pockets of the wool and in the air resulting in the formation of diiron trioxide (Fe₂O₃).

The heat released initiates a chain reaction of the neighboring steel wool particles with oxygen.

The chemical equation for the combustion of steel wool is as follows:

4 Fe (s) + 3 O₂ (g) > 2 Fe₂O₃ (s)

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2Fe(s) + 3O2(g) > 2FeO3(s)

Explanation:

According to the question, a  battery was used  to light the steel wool by bringing the terminals very close together. When  the battery came into contact with the steel wool, current was sent out through the thin wire.  This caused the iron to heat up quite well.

Iron reacts with oxygen under these conditions as follows;

2Fe(s) + 3O2(g) > 2FeO3(s)

This is the chemical reaction that occurs when the steel wool is set on fire.