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You know from previous classes, the volume V of a gas is inversely proportional to the pressure P, temperature being held constant. Separately, volume V and pressure P are directly proportional to temperature.
In a nut shell,
Boyle's law: V ∝ 1/P at constant T
Charles' law: V ∝ T at constant P
Gay-Lussac's law: P ∝ T at constant V
All the three laws apply to fixed mass m of an enclosed gas. Combining the three laws into a single relation for a fixed mass of gas yields ideal gas equation.
PV ∝ T
Alternatively, PV = NkBT where kB is the Boltzmann constant.
The laws of Boyle, Charles, and Gay-Lussac are strictly valid for real gases, only if the pressure of the gas is not too high and the temperature is not close to the liquefaction temperature of the gas. A gas obeying the equation of state PV = nRT at all pressures, and temperatures is an ideal gas.
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