Critical temperature carbon dioxide and methane are 31-1-C and -81-9-C respectively- Which of these has stronger intermolecular forces and why-

Question

Toppr Admin · Accepted Answer

Higher is the critical temperature- more easily the gas can be liquefied and greater are the intermolecular forces of attraction- Hence- CO2 has stronger intermolecular forces than H2O-

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?

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 $H_{2} O$ .

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?

Higher is the critical temperature, more easily the gas can be liquefied and greater are the intermolecular forces of attraction. Hence, CO2 has stronger intermolecular forces than H2O.

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?

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 $H_{2} O$ .