Question

Critical temperature for carbon dioxide and methane are ${31.1}^{\circ }C$ and $-{81.9}^{\circ }C$ respectively. Which of these has stronger intermolecular forces and why?

Answer 1

Higher is the critical temperature, more easily the gas can be liquefied and greater are the intermolecular forces of attraction. Hence, $C{O}_2$ has stronger intermolecular forces than $H_{2}O$.