What is the effect of increasing the number of gas molecules in a fixed volume?

When the number of gas molecules in a fixed volume is increased, the pressure of the gas also increases. This relationship can be explained by the ideal gas law, which states that pressure (P) is directly proportional to the number of moles of gas (n) when the volume (V) and temperature (T) are held constant.

As more gas molecules are added to the container, they collide more frequently with the walls of the container. Each collision exerts a force, and the cumulative effect of these frequent collisions leads to an increase in pressure. Therefore, if the number of molecules rises while the volume remains unchanged, the pressure directly increases as a result of the increased number of collisions with the container walls.

The other choices indicate that pressure decreases or remains the same, or that the temperature changes, which does not apply in this context when focusing solely on the number of molecules while keeping the volume constant. The consistent increase in collisions with the walls of the container as more gas is added highlights why pressure increases in this scenario.