A student measures the pressure exerted by separate \(1.00 \text{ mol}\) samples of \(\text{CH}_4\text{(g)}\) and \(\text{NH}_3\text{(g)}\) in identical \(1.00 \text{ L}\) rigid containers at \(200 \text{ K}\). Under these conditions, the measured pressure of each gas is lower than the pressure predicted by the ideal gas law (\(P_{\text{measured}} < P_{\text{ideal}}\)), but the deviation is significantly greater for \(\text{NH}_3\text{(g)}\) than for \(\text{CH}_4\text{(g)}\). Which of the following statements best explains why \(\text{NH}_3\text{(g)}\) shows a greater reduction from ideal pressure than \(\text{CH}_4\text{(g)}\)?