Explanation:
When the volume of a fixed amount of gas at constant temperature decreases, its pressure increases. This relationship is described by Boyle's Law, which states that the pressure of a gas is inversely proportional to its volume, when the temperature and amount of gas remain constant.
Here is a detailed explanation of why this occurs:
- Boyle's Law: According to Boyle's Law, the pressure of a gas is inversely proportional to its volume, when the temperature and amount of gas remain constant. This can be represented by the equation: P1V1 = P2V2, where P1 and V1 are the initial pressure and volume, and P2 and V2 are the final pressure and volume.
- Decreasing Volume: When the volume of a gas decreases, the same amount of gas is now confined to a smaller space. This means that the gas particles are more crowded together, resulting in more frequent collisions between the particles and the container walls.
- Increased Collisions: With more frequent collisions, there is an increase in the force exerted by the gas particles on the container walls. This increase in force leads to an increase in pressure.
- Pressure-Volume Relationship: The pressure of a gas is directly related to the force exerted by the gas particles on the container walls. As the force increases, the pressure also increases. Therefore, when the volume decreases, the pressure increases.
In conclusion, as the volume of a fixed amount of gas at constant temperature decreases, its pressure increases. This relationship is explained by Boyle's Law, which states that the pressure of a gas is inversely proportional to its volume, when the temperature and amount of gas remain constant.