Final answer:
A rigid container may burst when more gas is added at a constant temperature because the pressure increases due to more gas molecules hitting the walls of the container. The container can only withstand so much pressure before failing. This process is related to Avogadro's Law, where pressure increases as more gas is added to a container with a fixed volume.
Step-by-step explanation:
When gas is added to an enclosed, rigid container where the temperature does not change, the container may burst when the pressure inside becomes too great. The reason behind this is explained by Avogadro's Law, which states that under constant temperature and pressure conditions, the volume of a gas increases as more gas molecules are added. However, since the container in this scenario is rigid and cannot expand, the pressure will increase instead of the volume when more gas molecules are introduced.
The pressure inside the container increases as more gas molecules exert force on the walls of the container. If the pressure reaches beyond the container's ability to contain it, then it may result in a burst. This is a potential hazard that requires careful management, especially with gases that may leak or that are under high pressure.
Lastly, it is important to mention that even without temperature changes, just the action of adding more gas can result in dangerous levels of pressure. This explains why rigid containers often have air gaps to accommodate for minor changes, but if too much gas is added, these air gaps will not prevent the container from bursting.