Labs / Chemistry
Partial Pressures
Pick a gas, then dial in how many moles of it to release into the shared container. The particles mix freely, and each gas pushes on the walls all by itself — the stacked bar shows every gas's partial pressure, and they add up to the total pressure through Dalton's law. Change the volume and temperature to see the whole stack respond.
n 1.0 molPN₂ 0.00 atmPtotal 0.00 atm
What to try
- If you double the moles of one gas, what happens to its partial pressure — and to the total?
- Add helium and nitrogen in equal moles. They move at very different speeds, so why are their partial pressures the same?
- Squeeze the volume down to 5 L. How does compressing every gas at once change the total?
- Heat the container from 150 K to 600 K. Does each gas's share of the pressure grow evenly?
- Can you build a mixture where one gas supplies exactly half of the total pressure? What has to be true of the moles?