A fixed quantity of gas is compressed to a high density inside a rigid container held at a constant temperature \(T\). Under these conditions, the measured pressure \(P_{\text{measured}}\) is found to be lower than the pressure \(P_{\text{ideal}}\) predicted by the ideal gas law \(P = \dfrac{nRT}{V}\). Which of the following best explains why \(P_{\text{measured}}\) is less than \(P_{\text{ideal}}\) when attractive intermolecular forces are non-negligible?