text: well im not 100% sure but my text book has some info...\n\nobserved pressure = nRT / (V-nb)  - a(n/V)^2\n\nthe nb is a volume correction\n\nand a(n/V)^2 is a pressure correction. the 'a' is correcting for the attractions between particles. (so A is true)\n\nI think B is false because van der waals forces involve gravitation pull between particles, not anything to do with charge. so particles only attract each other.\n\nmy book also says "a real gas consists of atoms or molecules that have finite volumes. therefor, the volume available to a given particle in a real gas is less then the volume of the container because the gas particles themselves take up some of the space. to account for the discrepency, van der waals represented the actual volumes as shown in the equation. n is the number of moles of gas and b is an empirical constant."\n(that's too wordy for me to comprehend, so C and D are your call)