Trap some air in a syringe, seal the end, and press. The further you push, the harder it resists. Halve the space and the pressure doubles. The same particles are simply crowded into less room, so they strike the walls twice as often.
For a fixed mass of gas at constant temperature, the pressure multiplied by the volume is constant: pV = constant, so p1V1 = p2V2. Halving the volume doubles the pressure.
Boyle’s law states that for a fixed mass of gas at constant temperature, the pressure multiplied by the volume is constant.
True only at constant temperature for a fixed mass of gas.
Change the volume of a trapped gas at constant temperature and watch the pressure respond.
Four quick checks. Each correct answer earns XP and lights this skill on your star map.
Boyle’s law applies to a fixed mass of gas at constant...
For a fixed mass of gas at constant temperature, the product pV is...
If the volume of a gas is halved at constant temperature, the pressure...
Compressing a gas at constant temperature makes the particles hit the walls...
Pressure and volume move in opposite directions so that their product stays fixed.
A gas at 100 kPa occupies 2.0 m³. It is compressed to 0.50 m³ at constant temperature. Find the new pressure.
At constant temperature the particles do not speed up when you compress the gas. The pressure rises only because the same particles are packed into a smaller space, so they strike the walls more often per second.
Unlocks once the four checks above are done. Worth more XP, written in the style of Paper 2.
A gas at 200 kPa occupies 3.0 m³. Compressed to 1.0 m³ at constant temperature, its pressure becomes...
A gas at 150 kPa and 4.0 L expands to 6.0 L at constant temperature. Its new pressure is...
The relationship p₁V₁ = p₂V₂ can be used only when the gas...
That completes the particle model. Keep the chain going.