Which statement about real vs. ideal gases is not correct? Larger van der Waals constant b values indicate larger molecular sizes. Real gas molecules experience weak attractions toward each other whereas in the ideal gas model we assume there are no attractive forces between them. The greatest deviations from ideal behavior occur at low pressures and high temperatures. The most easily liquefied gases, such as water or methanol, have the largest values of the van der Waals constant a. Real gas molecules occupy some space, but in the ideal gas model we assume that they essentially have no volume