The ideal gas law is an equation that combines Avogadro’s law with the combined gas law. The ideal gas law holds true for ideal gases. Remember that an ideal gas is unlike a real gas because of the following assumptions.
- The particles of an ideal gas are considered to be small, hard spheres with no mass and no volume.
- The particles of an ideal gas are not attracted to each other.
- The particles of an ideal gas are moving very rapidly and randomly.
- The particles of an ideal gas are colliding with each other in perfectly elastic collisions.
The ideal gas law is shown by the following equation.
P is the pressure of the gas (in atm or kPa)
V is the volume of the gas (in L)
n is the number of moles of gas
R is the ideal gas constant ( 0.08206 L·atm·mol−1·K−1 or 8.3144 L·kPa·mol−1·K−1)
T is the temperature of the gas (in K)