An aerosol can is "accidently" tossed into a bon-fire and the can explodes. The gas law applicable in this situation would be the Gay-Lussac Gas Law. How?
In Boyle's Law, Charles' Law, and The Combined Gas Law, V remains constant because the volume of the container doesn't change.
In the Gay-Lussac Gas Law, Pressure increases and temperature
increases. Before, the molecules were moving slowly. As heat is added, the molecules move faster and get farther away applying pressure inside the can, which expands it. This is exactly why aerosol cans warn you NOT to have it around ANY high temperatures.
So when the can is tossed into the bon-fire, The gas "expands" inside due to the heat, increasing the pressure until the can cannot handle the stress (pressure) and explodes! Sources Aerosol Cans and The Gas Laws http://answers.yahoo.com/question/index?qid=20100506133106AARtYT2
http://students.ed.uiuc.edu/mrayon/gllaw.html
http://wiki.answers.com/Q/Why_does_air_expand_and_what_happens_to_the_molecules_when_it_expands The Aerosol Can and a bon-fire conveniently
located right next to you... Equation: P1 / T1 = P2 / T2 Equation: P1 / T1 = P2 / T2 Explanation You before taking Chemistry: P1 / T1 = C
P1 \ 1200F
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Aerosol Can
Describes how the aerosol can and gas laws are related to one another.
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