According to Boyle's Law, what happens to the volume of a gas as pressure increases (holding temperature constant)?

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Multiple Choice

According to Boyle's Law, what happens to the volume of a gas as pressure increases (holding temperature constant)?

Explanation:
Boyle's Law shows that at constant temperature, pressure and volume have an inverse relationship: P × V remains constant. So when you increase pressure, the gas is squeezed into a smaller space, and the volume must decrease to keep the product P × V the same. A handy way to picture it is with a syringe or a bicycle pump: pushing harder (increasing pressure) reduces the space the gas can occupy. The math form P1V1 = P2V2 expresses this idea: with temperature and amount of gas fixed, raising pressure lowers volume. That’s why the volume decreases.

Boyle's Law shows that at constant temperature, pressure and volume have an inverse relationship: P × V remains constant. So when you increase pressure, the gas is squeezed into a smaller space, and the volume must decrease to keep the product P × V the same. A handy way to picture it is with a syringe or a bicycle pump: pushing harder (increasing pressure) reduces the space the gas can occupy. The math form P1V1 = P2V2 expresses this idea: with temperature and amount of gas fixed, raising pressure lowers volume. That’s why the volume decreases.

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