A student investigates the non-ideal behavior of gases at low temperature and moderately high pressure. Separate samples containing exactly \(1.00\text{ mol}\) of \(\text{CH}_4\text{(g)}\) and \(1.00\text{ mol}\) of \(\text{CF}_4\text{(g)}\) are placed into identical \(1.00\text{ L}\) rigid containers at \(250\text{ K}\). The student calculates the ideal pressure using \(PV = nRT\) and records the experimentally measured pressures in the table below.

Gas	Temperature (\(\text{K}\))	Volume (\(\text{L}\))	Calculated \(P_{\text{ideal}}\) (\(\text{atm}\))	Measured \(P\) (\(\text{atm}\))
\(\text{CH}_4\text{(g)}\)	\(250\)	\(1.00\)	\(20.5\)	\(19.2\)
\(\text{CF}_4\text{(g)}\)	\(250\)	\(1.00\)	\(20.5\)	\(17.9\)

Which of the following best explains why the measured pressure of \(\text{CF}_4\text{(g)}\) is lower than the measured pressure of \(\text{CH}_4\text{(g)}\) under these conditions?