Which of the following gases would likely show a strong adherence to Boyle's Law?

The reason ideal gases show strong adherence to Boyle's Law lies in the foundational assumptions of the ideal gas model. Boyle's Law states that at constant temperature, the pressure of a gas is inversely proportional to its volume, meaning that as the volume decreases, the pressure increases, and vice versa.

Ideal gases are defined by conditions where gas molecules do not exhibit significant intermolecular forces and occupy negligible space compared to the total volume of the gas. These conditions allow for predictable behavior according to the mathematical equations that describe gas laws.

In real-world scenarios, non-ideal gases may deviate from this behavior due to interactions among gas particles or significant molecular volume, particularly at high pressures or low temperatures where these effects become pronounced. Therefore, while other gases may demonstrate some relation to Boyle's Law, ideal gases do so most accurately and consistently, affirming their status as the prime example of gases that adhere strongly to this law.