Podcast
Questions and Answers
What does the constant 'a' represent in the real gas equation?
What does the constant 'a' represent in the real gas equation?
The constant for the attraction between the molecules of a given gas
Who is the scientist credited with modifying the ideal gas equation to account for intermolecular forces and molecular size?
Who is the scientist credited with modifying the ideal gas equation to account for intermolecular forces and molecular size?
Johannes Diderik van der Waals
- What is a real gas and how does it differ from an ideal gas?
- What is a real gas and how does it differ from an ideal gas?
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.
- What are the main assumptions of the ideal gas theory?
- What are the main assumptions of the ideal gas theory?
- Why are ideal gases important, despite being hypothetical?
- Why are ideal gases important, despite being hypothetical?
What is the Van der Waals equation used for?
What is the Van der Waals equation used for?
What are the coefficients a and b in the Van der Waals equation?
What are the coefficients a and b in the Van der Waals equation?
What happens to gas behavior at low temperatures and high pressures?
What happens to gas behavior at low temperatures and high pressures?
What is the difference between the ideal gas law and the Van der Waals equation?
What is the difference between the ideal gas law and the Van der Waals equation?
What do the constants a and b represent in the van der Waals equation?
What do the constants a and b represent in the van der Waals equation?
How is the van der Waals equation different from the ideal gas law?
How is the van der Waals equation different from the ideal gas law?
According to the ideal gas law, what is the relationship between pressure, volume, temperature, and number of moles of an ideal gas?
According to the ideal gas law, what is the relationship between pressure, volume, temperature, and number of moles of an ideal gas?
Why is the pressure calculated using the van der Waals equation lower than the pressure calculated using the ideal gas law?
Why is the pressure calculated using the van der Waals equation lower than the pressure calculated using the ideal gas law?
When should the van der Waals equation be used instead of the ideal gas law?
When should the van der Waals equation be used instead of the ideal gas law?