What happens to pressure when the amount of gas in a closed container is increased?

When the amount of gas in a closed container is increased, the pressure within the container rises. This relationship is described by the Ideal Gas Law, which is expressed as PV = nRT. In this equation, P represents pressure, V is volume, n is the number of moles of gas, R is the universal gas constant, and T is temperature.

If the volume of the container and the temperature remain constant, increasing the amount of gas (n) directly leads to an increase in pressure (P). This occurs because more gas molecules are present, resulting in more frequent collisions with the walls of the container. Each collision exerts a force on the walls, thereby increasing the overall pressure.

In contrast, pressure does not remain constant, since that would imply no additional gas is being added or removed. Fluctuations in pressure may occur due to various factors, but a direct increase in the amount of gas in a constant volume scenario will lead to a consistent and predictable increase in pressure based on the gas laws. Thus, the correct choice indicates a straightforward application of the principles governing the behavior of gases.