The Van der Waals Equation

The constant for the attraction between the molecules of a given gas

Johannes Diderik van der Waals

A real gas is a gas whose molecules have intermolecular forces and collide inelastically. They occupy an actual volume and do not obey the ideal gas law. In contrast, an ideal gas is a hypothetical gas whose molecules do not take up any space, have no intermolecular forces, and collide elastically.

<p>The main assumptions of the ideal gas theory are: 1) Gas molecules are in constant random motion, 2) Gas molecules have no intermolecular attraction among themselves, and 3) Collisions between gas molecules are elastic, meaning no energy is lost upon collision.</p> Signup and view all the answers

<p>Ideal gases are important because the application of the ideal gas law provides information about how gas molecules would behave under perfect conditions. This allows us to extrapolate and understand the behavior of real gases, which have intermolecular forces and occupy actual volume.</p> Signup and view all the answers

<p>The Van der Waals equation is used to describe the behavior of real gases, taking into consideration intermolecular forces and the volume of gas molecules.</p> Signup and view all the answers

<p>The coefficients a and b in the Van der Waals equation are correction factors that differ for each gas. Coefficient a accounts for the magnitude of intermolecular forces, while coefficient b accounts for the volume of 1 mole of gas.</p> Signup and view all the answers

<p>At low temperatures and high pressures, gas behavior deviates from ideal and becomes a real gas. Gas particles move slowly, become closer to one another, and exhibit more intermolecular forces.</p> Signup and view all the answers

<p>The ideal gas law assumes ideal gas behavior with no intermolecular forces and no volume for gas molecules. The Van der Waals equation incorporates correction factors for intermolecular forces and gas volume, providing a more accurate description of real gas behavior.</p> Signup and view all the answers

<p>The constant a represents the attraction between the molecules of a given gas, while the constant b represents the volume those molecules take up inside the container.</p> Signup and view all the answers

<p>The van der Waals equation takes into account the volume of the gas molecules and the attraction between those molecules, which are considered negligible under ideal conditions.</p> Signup and view all the answers

<p>The ideal gas law states that the pressure, volume, temperature, and number of moles of an ideal gas are related by the equation PV = nRT.</p> Signup and view all the answers

<p>The pressure calculated using the van der Waals equation is lower because the equation takes into account the attraction between gas molecules, which causes the molecules to stay closer together and occupy a smaller volume. This reduces the frequency of collisions with the container walls, resulting in a lower pressure.</p> Signup and view all the answers

<p>The van der Waals equation should be used instead of the ideal gas law when dealing with real gases, as it factors in the relative effects of the volume of the gas molecules and the attraction between those molecules. The ideal gas law can only be applied to ideal gases.</p> Signup and view all the answers