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CHEMISTRY • GAS LAWS
Ideal Gas Law
Compress, heat and add gas while pressure responds through PV = nRT. Compare two volumes, inspect the pressure–volume isotherm and solve a target-pressure design problem.
● LIVE GAS STATEideal-gas state
Pressure—
Volume—
Reference P—
Target error—
PV—
Thermal index—
Separate the variables
This bench uses the ideal-gas equation as a macroscopic model. Hold two variables fixed while changing the third and use the reference state to distinguish inverse and direct relationships.
Fast investigations
- Double volume at fixed n and T and compare pressure.
- Double temperature at fixed n and V.
- Double moles at fixed T and V.
- Use the challenge to find the volume that produces approximately 1 atm.
LEARN WITH THE SIMULATION
Understand Ideal Gas Law by experimenting.
START HERE
The ideal gas law combines pressure, volume, temperature and amount of gas into one equation. It models gases best when particles are dilute and intermolecular interactions are relatively small.
BUILD THE IDEA
What you should understand first
- Use PV = nRT to solve for pressure.
- Predict how temperature or volume changes affect pressure.
- Keep Kelvin temperature distinct from Celsius.
TRY IT YOURSELF
What happens to pressure if absolute temperature doubles at fixed volume and moles?
- Record the initial pressure.
- Double the Kelvin temperature without changing n or V.
- Compare the pressure ratio.
Read the visual:
Pressure doubles because P is directly proportional to absolute temperature when n and V are fixed.
WHY IT WORKS 01
Use PV = nRT to solve for pressure.
The ideal gas law combines pressure, volume, temperature and amount of gas into one equation. It models gases best when particles are dilute and intermolecular interactions are relatively small. Focus on the relationship between the controlled variable and the measured response rather than treating the visual change as the explanation.
WHY IT WORKS 02
Predict how temperature or volume changes affect pressure.
Pressure doubles because P is directly proportional to absolute temperature when n and V are fixed. Use an extreme or boundary setting after the baseline trial to check whether the same reasoning still holds.
DO NOT MIX THESE UP
Common misconception
Temperature must be absolute Kelvin in the gas law. Real gases deviate most at high pressure and low temperature. Increasing container volume at fixed n and T lowers pressure rather than increasing it.
PRACTICE CHALLENGE
What happens to pressure if absolute temperature doubles at fixed volume and moles?
- Record the initial pressure.
- Double the Kelvin temperature without changing n or V.
- Compare the pressure ratio.
Reveal the reasoning
Pressure doubles because P is directly proportional to absolute temperature when n and V are fixed. Temperature must be absolute Kelvin in the gas law. Real gases deviate most at high pressure and low temperature. Increasing container volume at fixed n and T lowers pressure rather than increasing it.
MODEL BOUNDARIES
What this simulation assumes
Every simulation simplifies reality or a mathematical system. These are the assumptions and limits to keep in mind while interpreting the results.
Model assumptions
- Gas particles follow the ideal-gas equation PV = nRT.
- Particles have negligible molecular volume and no intermolecular forces.
- The gas is at equilibrium with uniform temperature and pressure.
Model limitations
- Real gases deviate from ideal behavior at high pressure and low temperature.
- Phase changes, molecular interactions and non-equilibrium gas dynamics are not represented.
CONNECT IT
Where this matters
- Gas storage
- Weather and atmospheric approximations
- Chemical-process calculations
WORDS THAT MATTER
Key vocabulary
- Pressure
- Force per unit area from molecular collisions.
- Mole
- Amount-of-substance unit.
- Ideal gas
- Model of point particles with negligible intermolecular forces.
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