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 for carbon dioxide and methane are 31.1 ""^(@)C a

1.	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 ?
Answer» Solution :Intermolecular forces is more STRONG in CARBON DIOXIDE. Critical temperature of carbon dioxide is `31.1 ""^(@)C`. Which is more than methane liquification of carbon dioxide occurs easily at high temperature. Intermolecular attraction forces are strong in methane and LESS strong (weak) than `CO_(2)`. Molecular mass of `CO_(2)` is 44 gm/mol. and methane is 16 gm/mol. So attraction force of Van der waal are more in `CO_(2)` than `CH_(4)`.