Which gas law would help explain the varying concentration of gases in the atmosphere at different altitudes?

The correct choice is Dalton's Law, which is essential for understanding how gases behave in the atmosphere at different altitudes. Dalton's Law states that in a mixture of non-reacting gases, the total pressure is equal to the sum of the partial pressures of each individual gas. As altitude increases, atmospheric pressure decreases, resulting in a change in the concentration of gases, such as oxygen and nitrogen, leading to lower partial pressures at higher elevations.

This law is particularly relevant in aerospace physiology, where the availability of oxygen influences various physiological processes at high altitudes. Since each gas contributes separately to the total pressure, understanding how each gas's partial pressure changes with altitude helps explain issues like hypoxia (inadequate oxygen) that can occur during high-altitude flight.

The other laws mentioned, while important in various contexts, do not specifically address the behavior of gases in mixtures at varying altitudes in the same way that Dalton's Law does. For instance, Henry's Law relates to the solubility of gases in liquids, Charles' Law addresses the relationship between gas volume and temperature, and Boyle's Law focuses on the relationship between pressure and volume of a gas. Therefore, Dalton's Law is the most pertinent to the question regarding gas concentration variations with altitude