Final answer:
The given scenario possibly illustrates Gay-Lussac's Law, which states that the pressure of an enclosed gas is directly proportional to its temperature, if volume is constant. Without knowing the original pressure, it cannot be definitively said if this law fully applies.
Step-by-step explanation:
This question relates to the Gas Laws, a set of physical principles regarding gases in chemistry and physics. A vital concept here is Gay-Lussac's Law, which states that the pressure of an enclosed gas is directly proportional to its temperature, when the volume is held constant.
When the pressure changes from an unspecified value to 456 torr, and the temperature changes from 150°C to 75°C, this is an illustration of Gay-Lussac's Law. If the original pressure were higher than 456 torr, then it decreasing as the temperature decreases would align with Gay-Lussac's Law. Conversely, if the original pressure were less than 456 torr, and it increased with the decreasing temperature, this would contradict Gay-Lussac's Law, implying there might be another factor at play, such as a change in volume.
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