The volume of a gas is doubled while the temperature is held constant. How does the gas pressure change?

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The question describes a gas undergoing a change where its volume doubles while the temperature remains constant. According to Boyle's law, for a fixed amount of gas at a constant temperature, pressure is inversely proportional to volume (P ∝ 1/V).
Option 1: 'It is reduced by one half.' This aligns with P1 = P2 × (V1/V2) = P × (V/(2V)) = P/2, so the pressure becomes half as large when the volume doubles. This reasoning is correct.
Option 2: 'It does not change.' If the volume increases while temperature is fixed, the pressure must drop to maintain the same PV product. Therefore, claiming no change is incorrect.
Option 3: 'It is doubled.' Doubling the volume would reduce, not increase, the pressure under constant temperature; stating that pressure doubles contradicts Boyle's law, making this option false.
Option 4: 'It varies depending on the type of gas.' For an ideal gas under these conditions, pressure depends on volume and temperature, not on the specific type of gas. Real gases may deviate at high pressures, but the standard relation given by Boyle's law assumes ideal behavior, so this option misstates the general principle in the typical context of this question.

Chemistry (H) - Varnold - Preparatory Academy - 2nd Semester - 2024/2025 Gases Practice Test for the Final

The volume of a gas is doubled while the temperature is held constant. How does the gas pressure change?

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