Final answer:
The distance between pressure levels generally decreases when the temperature increases, as demonstrated by the laws of thermodynamics, especially Charles' law which states that volume increases with temperature at a constant pressure.
Step-by-step explanation:
When considering what happens to the distance between pressure levels at different temperatures, it is important to understand the behavior of gases under various thermal conditions. According to Charles' law (V vs. T), at constant pressure and a fixed amount of gas, the volume increases as the temperature increases. This is because the added energy causes the gas particles to move more swiftly, colliding with the walls of their container more frequently and with greater force, leading to an expansion of the gas.
Thus, when a large amount of energy is added, it can cause a decrease in the gas's volume if the pressure remains constant, or a decrease in pressure if the volume remains fixed. On the other hand, removing energy from the system could cause an increase in pressure or a decrease in volume. Considering these principles, the correct answer is that the distance between pressure levels increases with increased temperature, demonstrating expansion due to an increase in the energy of the system.
In summary, temperature directly affects the volume and pressure of a gas due to the kinetic molecular theory, which describes how particles move and interact. Therefore, the answer to what happens to the distance between pressure levels at different temperatures would be b) Decreases, assuming that the temperature change results in a volume change as the gas expands or compresses.