Aerosol cans carry clear warnings against incineration...

Aerosol cans carry clear warnings against incineration because of the high pressures that can develop upon heating. Suppose a can contains a residual amount of gas at a pressure of $755 \mathrm{mm} \mathrm{Hg}$ and $25^{\circ} \mathrm{C}$. What would the pressure be if the can were heated to $1155^{\circ} \mathrm{C} ?$

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Key Concepts

Ideal Gas Behavior in a Fixed Volume

When a gas is contained within a fixed volume, any change in its temperature directly affects its pressure according to the ideal gas law. This concept is fundamental in understanding how heating a confined gas can lead to significant pressure increases, as the number of gas molecules and the volume remain constant while the kinetic energy, and therefore the pressure, rises with temperature.

Temperature Conversion to Kelvin

In thermodynamics, temperatures must be expressed in an absolute scale such as Kelvin when used in gas law calculations. Converting from Celsius to Kelvin is necessary because the Kelvin scale starts at absolute zero, ensuring accurate proportional relationships in formulas like those derived from the ideal gas law.

Gay-Lussac's Law

This law states that for a fixed amount of gas at constant volume, the pressure is directly proportional to its absolute temperature. This relationship means that when the temperature increases, the pressure increases in a linear fashion provided the gas’s volume and mole number remain unchanged, which is critical for understanding pressure changes in confined gases.

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