Critical temperature for carbon dioxide and methane

Critical temperature for carbon dioxide and methane are 31.1°C and - 81.9°C respectively. Which of these has stronger intermolecular forces and why?

Critical temperature is the temperature above which the gas cannot be liquefied, how so ever high pressure we may apply.

Higher the critical temperature, more easily the gas can be liquefied, i.e., stronger are the intermolecular forces. Hence, $CO_{ 2 }$ has stronger intermolecular forces than $CH_{ 4 }$.