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Question
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 and –81.9∘C respectively. Which of these has stronger intermolecular forces and why?
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Solution
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(Tc). 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 CO2. Hence, intermolecular forces of attraction are stronger in the case of CO2.
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(Tc). 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 CO2. Hence, intermolecular forces of attraction are stronger in the case of CO2.
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