Assume that you have 0.500 mol of N2 in a volume of 0.600 L at 300 K. Calculate the pressure in atmospheres using both the ideal gas law and the van der Waals equation. For N2, a = 1.351 L^2 atm/mol^2 and b = 0.0387 L/mol.

The Ideal Gas Law is a fundamental equation in chemistry that relates the pressure (P), volume (V), number of moles (n), and temperature (T) of an ideal gas through the equation PV = nRT. Here, R is the ideal gas constant. This law assumes that gas particles do not interact and occupy no volume, making it a good approximation under many conditions, particularly at high temperatures and low pressures.

The Van der Waals equation is an adjustment of the Ideal Gas Law that accounts for the volume occupied by gas molecules and the attractive forces between them. It is expressed as (P + a(n/V)^2)(V - nb) = nRT, where 'a' and 'b' are constants specific to each gas. This equation provides a more accurate description of real gas behavior, especially under high pressure and low temperature conditions.

Real gases deviate from ideal behavior due to intermolecular forces and the finite volume of gas particles. While the Ideal Gas Law assumes no interactions and negligible volume, real gases exhibit attractions and repulsions that can affect pressure and volume. Understanding these differences is crucial when applying the Ideal Gas Law and the Van der Waals equation to predict gas behavior accurately.