The Van der Waals Equation

Which gas is considered to be hypothetical and does not take up any volume?

What equation is a modification of the original ideal gas law and takes into consideration the molecular size and intermolecular forces of the gas?

What type of gas is characterized by its individual molecules occupying an actual volume and exhibiting intermolecular forces?

Which equation is used to describe the behavior of real gases, taking into consideration the size of the gas molecule and the intermolecular forces?

What are the coefficients a and b used for in the Van der Waals equation?

Under what conditions does the behavior of a gas deviate from ideal and become a real gas?

What happens to the pressure of a gas when the volume of the container decreases?

Which equation describes the behavior of real gases, taking into account intermolecular forces and molecular size?

What changes are made to the ideal gas law in order to describe the behavior of real gases?

What conditions cause real gas behavior to deviate from ideal gas behavior?

Which scientist modified the ideal gas equation to consider intermolecular forces and molecular size?

Which equation is used to calculate the pressure, volume, temperature, or number of moles of an ideal gas?

Which equation takes into account the relative effects of the volume of gas molecules and the attraction between those molecules?

Why is the pressure obtained from the van der Waals equation lower than the pressure obtained from the ideal gas equation?

What does the 'a' constant represent in the van der Waals equation?

Which equation is used to account for the attractive forces between gas molecules and the volume of those molecules?

What is the value of the ideal gas constant (R)?

What is the difference between the ideal gas law and the van der Waals equation?

Under what conditions do real gases behave differently from ideal gases?