Ideal Gas Law Simulator
Classroom worksheet · Interactive simulation: https://lkforge.com/tools/physics/ideal-gas/
Name: Date:
Learning objectives
- Relate pressure, volume, temperature, and amount of gas.
- Connect macroscopic gas behavior to molecular motion.
- Apply the ideal gas law.
Variables to change
- Temperature
- Volume
- Number of particles
- Pressure
Procedure
- Hold temperature fixed and reduce the volume; watch the pressure (Boyle’s law).
- Hold volume fixed and raise the temperature; watch the pressure (Gay-Lussac’s law).
- Add more particles at fixed volume and temperature; watch the pressure.
Observations
Record how pressure responds to each change, keeping the other quantities fixed.
Questions
- At constant temperature, what happens to pressure when volume decreases?
- At constant volume, what happens to pressure when temperature rises?
- Write the ideal gas law.
- Microscopically, why does raising temperature raise pressure at fixed volume?
- Why must temperature be in kelvin for these relationships?
Answer key (instructors)
- 1. Pressure increases — P and V are inversely proportional (Boyle’s law).
- 2. Pressure increases in proportion to absolute temperature (Gay-Lussac’s law).
- 3. PV = nRT (or PV = NkT).
- 4. Molecules move faster and strike the walls harder and more often, increasing force per area.
- 5. The gas laws are proportional to absolute temperature; kelvin starts at absolute zero, where ideal-gas pressure would be zero.
The ideal gas law PV = nRT ties pressure, volume, temperature, and amount together. Microscopically, pressure comes from molecular collisions with the walls; hotter gas means faster molecules and more forceful, frequent collisions.