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 P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is temperature. The constants a and b are specific to each gas and represent the strength of intermolecular forces and the volume occupied by the gas molecules, respectively. This equation is particularly useful for real gases, which do not always behave ideally, especially under high pressure and low temperature conditions. By incorporating these factors, the Van der Waals Equation provides a more accurate description of gas behavior, helping scientists and engineers predict how gases will react in various situations.