(a) Write van der Waals equation for one mole of a gas. (b) What are

1.	(a) Write van der Waals equation for one mole of a gas. (b) What are the conditions under which real gases show ideal behaviour? (c) Critical temperature for CO2, and CH4 are 31.1oC and - 81.9PoC respectively. Which of these has stronger intermolecular forces and why?
Answer» (a) \(\big(P+\frac{a}{V^2}\big)(V-a)\) = RT (b) At high temperature and low pressure, real gases show ideal behaviour. (c) Higher the critical temperature, stronger the intermolecular forces. Therefore, CO₂ has stronger intermolecular forces than CH₄.

(a) Write van der Waals equation for one mole of a gas. (b) What are the conditions under which real gases show ideal behaviour? (c) Critical temperature for CO2, and CH4 are 31.1oC and - 81.9PoC respectively. Which of these has stronger intermolecular forces and why?

Answer»

(a) \(\big(P+\frac{a}{V^2}\big)(V-a)\) = RT

(b) At high temperature and low pressure, real gases show ideal behaviour.

(c) Higher the critical temperature, stronger the intermolecular forces. Therefore, CO₂ has stronger intermolecular forces than CH₄.