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Chapter 12: Problem 62

Why is it dangerous to incinerate an aerosol can?

Short Answer

Expert verified
Incinerating an aerosol can is dangerous because the increased pressure and flammable propellant gases can cause the can to explode.

Step by step solution

01

Understanding Aerosol Can Composition

Aerosol cans contain a mixture of a product (such as paint or deodorant) and a propellant gas, which is necessary to expel the product out of the can when the nozzle is pressed.
02

Properties of the Propellant Gas

The propellant gas inside the aerosol can is often a volatile substance, such as butane, propane, or similar gases. These gases are highly flammable and can become dangerous when exposed to high temperatures.
03

Effect of High Temperature

When an aerosol can is exposed to high temperatures, such as those during incineration, the pressure inside the can increases rapidly due to the heating of both the product and the propellant gas. This significant pressure build-up can lead to an explosive rupture of the can.
04

Explosive Risk

The combination of increased internal pressure and the flammability of the propellant gas means that the can can explode violently. The explosion can cause injuries from flying metal shards and the high heat can ignite other flammable materials nearby.
05

Conclusion

Due to the presence of flammable propellant gases and the significant pressure increase when heated, incinerating an aerosol can poses a serious risk of explosion and injury.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

flammable gases
Aerosol cans are common household items that may contain flammable gases like butane or propane as propellants. These gases are used to pressurize the can, allowing the product—such as hairspray or deodorant—to be dispensed when you press the nozzle.

However, these propellant gases have a dangerous side. They're highly flammable, meaning they can easily catch fire and burn quickly when exposed to a spark or flame. Imagine using a lighter near an aerosol can; the gas can ignite almost instantly.

Because these gases are contained under pressure, even a slight exposure to high temperatures can have serious consequences.
high temperature effects
When an aerosol can is exposed to high temperatures, the contents inside, including the gas, start to heat up. High temperatures can come from several sources, such as direct sunlight or, even worse, fire.

Heating causes the gas molecules to move faster and spread out, increasing the pressure inside the can. This is a basic principle from physics: as temperature increases, so does pressure.

In extreme cases, like in the presence of fire, the temperature can rise rapidly. This can lead to a situation where the can becomes a ticking time bomb, waiting to explode under the increasing internal pressure.
pressure build-up
Pressure build-up is one of the main reasons why aerosol cans can become dangerous. When the internal temperature of the can increases, the gas inside expands and the pressure rises.

Think of it like blowing up a balloon: the more air you put in, the more it stretches, and the higher the internal pressure. At some point, if you keep adding air, the balloon will burst.

Aerosol cans work the same way. Extra pressure from the heating can make the can burst open, releasing the flammable gas and other contents suddenly, which can be very dangerous.
explosive risk
The explosive risk of an aerosol can is due to the combined effects of high internal pressure and flammable gas. When these cans are heated, the risks multiply.

If an aerosol can explodes, it doesn't just crack open quietly. It explodes violently, sending metal fragments flying in all directions. These flying bits can cause serious injuries or even fatalities.

The flammable gas released during the explosion can also ignite, leading to secondary fires. This can cause further damage to property and endanger lives.

For these reasons, it's crucial to handle aerosol cans with care and never subject them to high temperatures.

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Most popular questions from this chapter

A sample of \(\mathrm{CH}_{4}\) gas occupies a volume of \(575 \mathrm{~mL}\) at \(-25^{\circ} \mathrm{C}\). If pressure remains constant, what will be the new volume if temperature changes to: (a) \(298 \mathrm{~K}\) (b) \(32^{\circ} \mathrm{F}\) (c) \(45^{\circ} \mathrm{C}\)

When glucose is burned in a closed container, carbon dioxide gas and water are produced according to the following equation: $$ \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}(s)+6 \mathrm{O}_{2}(g) \longrightarrow 6 \mathrm{CO}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(l) $$ How many liters of \(\mathrm{CO}_{2}\) at STP can be produced when \(1.50 \mathrm{~kg}\) of glucose are burned?

A balloon will burst at a volume of \(2.00 \mathrm{~L}\). If it is partially filled at \(20.0^{\circ} \mathrm{C}\) and \(65 \mathrm{~cm}\) Hg to occupy \(1.75 \mathrm{~L}\), at what temperature will it burst if the pressure is exactly \(1 \mathrm{~atm}\) at the time that it bursts?

A chemist carried out a chemical reaction that produced a gas. It was found that the gas contained \(80.0 \%\) carbon and \(20.0 \%\) hydrogen. It was also noticed that \(1500 \mathrm{~mL}\) of the gas at STP had a mass of \(2.01 \mathrm{~g}\). (a) What is the empirical formula of the compound? (b) What is the molecular formula of the compound? (c) What Lewis structure fits this compound?

Sketch a graph to show each of the following relationships: (a) \(P\) vs. \(V\) at constant temperature and number of moles (b) \(T\) vs. \(V\) at constant pressure and number of moles (c) \(n\) vs. \(V\) at constant temperature and pressure
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