Which condition would most likely prevent gas expansion?

Low temperature is the condition that most likely prevents gas expansion due to its direct impact on the kinetic energy of gas molecules. When the temperature of a gas decreases, the average kinetic energy of its particles also decreases. This reduction in kinetic energy means that the particles move more slowly and collide with each other and the walls of the container with less force. As a result, the gas does not have sufficient energy to overcome intermolecular forces or to expand significantly within its container.

In contrast, high temperature generally increases kinetic energy, encouraging gas expansion, while low pressure allows gas molecules to spread out and occupy a larger volume. High pressure compresses gas by forcing particles closer together but does not inherently prevent expansion in the same way that low temperature does. Therefore, low temperature is the most effective condition for limiting gas expansion.