If the volume of a container of gas changes, the pressure of the gas will change in an inverse manner.

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The statement concerns how pressure responds to a change in volume for a gas, which is a classic form of Boyle's Law. 
Option 1: True. When temperature and the amount of gas (moles) are held constant, the pressure of a gas increases as volume decreases, and decreases as volume increases. This inverse relationship means P ∝ 1/V, so a change in volume results in a corresponding inverse change in pressure. The reasoning hinges on controlled conditions: constant T, constant n, and a purely gaseous system. 
Option 2: False. This would be the claim that pressure and volume are directly related or independent, which contradicts Boyle's law. If volume goes down but pressure stayed the same, or volume up with no pressure change, that would violate the observed inverse behavior under constant temperature and molar amount. In real scenarios, if temperature were not controlled and could change, the relationship could become more complex (since P also depends on T and n), but under the stated idealized condition of constant temperature and constant moles, the inverse relationship stands. 
Option 3: If we considered non-ideal gases or extreme conditions, deviations might occur, so the simple inverse proportionality is an approximation. However, the core statement presumes the standard gas-law context, where the inverse relation is the defining feature. 
Option 4: The statement does not specify temperature or amount of gas; without those qualifiers, the claim is incomplete, but in the typical gas-law framework where T and n are held constant, the inverse dependence is what Boyle's law predicts. Therefore, the nuance about conditions is essential for full accuracy, even though the inverse relationship is the core takeaway under standard assumptions.

BIO 112-Intro. Human Physiology-861, 862, 863 Quiz 12

If the volume of a container of gas changes, the pressure of the gas will change in an inverse manner.

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