How do gases behave according to the laws of pressure and volume?

Gases behave according to the ideal gas laws, which outline the relationship between temperature, pressure, and volume. The correct answer indicates that gases expand and contract based on temperature changes. When the temperature of a gas increases, the kinetic energy of its particles increases, causing them to move more vigorously and thus occupy a larger volume—hence the expansion. Conversely, if the temperature decreases, the kinetic energy falls, leading the gas to contract.

This behavior can be described by Charles's Law, which states that at constant pressure, the volume of a gas is directly proportional to its absolute temperature. Therefore, temperature plays a crucial role in determining the volume and pressure of gases, validating the correctness of the first statement as it emphasizes the direct relationship between temperature and the behavior of gases.

The other options do not properly reflect the principles of gas behavior. For instance, stating that gases remain unaffected by temperature changes contradicts the fundamental gas laws, which clearly show the relationship between temperature changes and variations in volume and pressure. Similarly, eliminating thermal energy completely goes against the concept that energy affects gas behavior, and suggesting that gases have a constant volume regardless of temperature is true only for liquids and solids, not for gases, which are defined by their ability to fill the