Gas-law nomenclature at constant pressure The statement “All perfect gases change in volume by 1/273 of their original volume at 0°C for every 1°C change in temperature at constant pressure” refers to which named law?

Introduction / Context:
Classical gas laws describe limiting behaviors of ideal gases when one state variable is held fixed. Recognizing the correct eponym ensures you apply the right proportionality for experiments and calculations involving constant-pressure heating or cooling.

Given Data / Assumptions:

• Perfect (ideal) gas behavior.
• Pressure held constant.
• Reference condition at 0°C (273.15 K).

Concept / Approach:

Charles’ law states that, at constant pressure, the volume of a given mass of gas is directly proportional to its absolute temperature. Expressed differentially near 0°C, the fractional change in volume per 1°C is approximately 1/273 of the volume at 0°C, reflecting linear expansion on the Kelvin scale. Boyle’s law pertains to P–V inverse proportionality at constant temperature; Gay-Lussac’s commonly names P–T proportionality at constant volume (terminology conventions vary regionally), while Joule’s law relates internal energy of an ideal gas to temperature only.

Step-by-Step Solution:

Verification / Alternative check:

From the ideal-gas equation P * V = n * R * T, with P and n fixed, V/T is constant. This yields the linear relation underlying the 1/273 figure at 0°C.

Why Other Options Are Wrong:

Boyle: constant T, not constant P.Gay-Lussac: commonly P–T at constant V, not V–T at constant P.Joule: internal energy independence from volume for ideal gases.Avogadro: equal volumes at the same T and P contain equal numbers of molecules.

Common Pitfalls:

Memorizing names without the associated constraints (which variable is held constant). Always tie the eponym to the controlled variable.

Final Answer:

Charles' law