Question at position 53 According to Boyle's Law, what happens to the pressure of a gas when the volume of its container is halved, assuming constant temperature?Pressure becomes zeroPressure remains the samePressure is halvedPressure doubles

Question

BlackTom AI · Accepted Answer

When evaluating how pressure changes with volume at constant temperature, Boyle's Law gives PV = constant for a fixed amount of gas.

Option 1: 'Pressure becomes zero' would require volume to become infinite or amount of gas to vanish; halving the volume does not drive pressure to zero under normal conditions, so this is incorrect.

Option 2: 'Pressure remains the same' would imply PV is unchanged with V changing, which contradicts Boyle's Law since reducing V must increase P if T and n are constant. Therefore this is incorrect.

Option 3: 'Pressure is halved' would require volume to double (P ∝ 1/V) for a fixed P, T, and n; halving V does not produce half the pressure, so this is not correct.

Option 4: 'Pressure doubles' directly follows from halving the volume while keeping temperature and the amount of gas constant: since P ∝ 1/V, reducing V by a factor of 2 doubles P to keep PV constant. This is the correct interpretation under Boyle's Law.

Question at position 53 According to Boyle's Law, what happens to the pressure of a gas when the volume of its container is halved, assuming constant temperature?Pressure becomes zeroPressure remains the samePressure is halvedPressure doubles

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