ANS:C - Boyle's law & Charle's Law

The ideal gas laws are typically applicable to individual gases under certain conditions. However, when it comes to mixtures of gases, each gas in the mixture behaves independently according to its own properties, but their collective behavior may not always follow the ideal gas laws. Let's analyze the given options:

1. Amagat's law: Amagat's law states that the volume occupied by a mixture of non-reacting gases at constant temperature and pressure is equal to the sum of the volumes that each gas would occupy if it alone occupied the total volume under the same conditions. This law is specifically formulated for gas mixtures and is applicable to mixtures of ideal gases.
2. Dalton's law: Dalton's law states that the total pressure exerted by a mixture of non-reacting gases is equal to the sum of the partial pressures of the individual gases in the mixture. This law is also formulated for gas mixtures and is applicable to mixtures of ideal gases.
3. Boyle's law & Charles's law: These laws describe the behavior of individual gases, not mixtures. Boyle's law states that at constant temperature, the volume of a given amount of gas is inversely proportional to the pressure exerted on it. Charles's law states that at constant pressure, the volume of a given amount of gas is directly proportional to its temperature. While these laws apply to individual gases, they don't directly address gas mixtures.