Which of the following four statments are true for real gases and the corrections that must be made to the Ide

Which of the following four statments are true for real gases and the corrections that must be made to the Ideal Gas Law?


a) the constant a in van der waals equation corrects for attractions between particles





b) particles attract and repel each other





c) the volume of particles reduces observed pressure





d) the constant b in van der waals equation corrects for volume of real particles

Which of the following four statments are true for real gases and the corrections that must be made to the Ide
well im not 100% sure but my text book has some info...





observed pressure = nRT / (V-nb) - a(n/V)^2





the nb is a volume correction





and a(n/V)^2 is a pressure correction. the 'a' is correcting for the attractions between particles. (so A is true)





I 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.





my 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."


(that's too wordy for me to comprehend, so C and D are your call)