All Labs

Gas Laws Lab

Explore how pressure, volume, temperature, and moles relate through the ideal gas law. Isolate individual gas laws, collect data across multiple trials, and discover the relationships experimentally with animated particle simulations.

Guided Experiment: Boyle's Law Investigation

If you increase the pressure on a gas at constant temperature, what do you predict will happen to the volume?

Write your hypothesis in the Lab Report panel, then click Next.

Controls

Pressure1.00 atm
Volume22.40 L
Temperature273.15 K
Moles1.00 mol

Results

PV=22.4000nRT=22.4147PV = 22.4000 \quad nRT = 22.4147
PV product
22.4000 L·atm
V/T ratio
0.0820 L/K
P/T ratio
0.00366 atm/K
Average Kinetic Energy (3/2 nRT)
33.6220 L·atm

Pressure vs Volume

Data Table

(0 rows)
#TrialPressure(atm)Volume(L)Temperature(K)Moles(mol)PV(L·atm)
0 / 500
0 / 500
0 / 500

Reference Guide

Ideal Gas Law

The ideal gas law relates the four state variables of a gas.

PV=nRTPV = nRT

Where P is pressure, V is volume, n is moles, R is the gas constant (0.08206 L·atm/mol·K), and T is temperature in Kelvin.

Boyle's Law

At constant temperature and moles, pressure and volume are inversely proportional.

P1V1=P2V2P_1 V_1 = P_2 V_2

Doubling pressure halves volume. The PV product remains constant.

Charles's Law

At constant pressure, volume is directly proportional to temperature.

V1T1=V2T2\frac{V_1}{T_1} = \frac{V_2}{T_2}

Heating a gas makes it expand. The V/T ratio stays constant.

Gay-Lussac's Law

At constant volume, pressure is directly proportional to temperature.

P1T1=P2T2\frac{P_1}{T_1} = \frac{P_2}{T_2}

Heating a sealed container increases pressure. The P/T ratio stays constant.