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 of a gas, easier is its liquidification.

The maximum temperature at which a gas can be converted into a liquid by an increase in pressure is called its critical temperature(T_c). This means that the intermolecular forces of attraction between the molecules of a gas are directly proportional to its critical temperature. Hence, intermolecular forces of attraction are stronger in the case of $C{O}_2$. Hence, intermolecular forces of attraction are stronger in the case of $C{O}_2$.