A sealed cylinder holds argon gas under a movable piston. Change the temperature, volume or amount and the lab recomputes the pressure from PV = nRT, while the particles bounce off the walls and their RMS speed follows the temperature.
• A transparent cylinder, a movable sealed piston, argon particle samples, a controlled thermal reservoir and an absolute-pressure gauge. • Sliders for gas temperature (200 to 600 K), chamber volume (5 to 30 L) and gas amount (0.1 to 1 mol), with toggles for an animated isothermal compression and explanatory particles. • Readouts: absolute pressure in kPa, volume, temperature, argon RMS speed and monatomic internal energy. • Experiments: doubling the temperature from 300 to 600 K at fixed volume and amount doubles the pressure; a compression cycle raises pressure as the piston descends.
PV = nRT with R = 8.3144626 kPa·L/(mol·K). The RMS speed is v_RMS = √(3RT/M) with M_Ar = 0.039948 kg/mol, and the internal energy of a monatomic ideal gas is U = 3nRT/2. The isothermal sweep shows Boyle's law, P inversely proportional to V.
The gas is ideal monatomic argon at a controlled uniform temperature. Displayed particles are representative samples, not an Avogadro-scale simulation, and wall paths do not solve intermolecular collisions. The isothermal volume sweep excludes work and heat transient dynamics.
At constant temperature and amount it doubles, which is Boyle's law. The compression cycle demonstrates this with the gauge reading.
At fixed volume and amount, PV = nRT makes P proportional to T. Hotter particles hit the walls harder and more often.
A monatomic noble gas is well approximated as an ideal gas, and its internal energy is simply 3nRT/2 with a known molar mass for the RMS speed.
No. It assumes an ideal gas, with no intermolecular forces or finite particle size, and it does not simulate Avogadro-scale collisions.