Redefining the Phase Space for Ideal Gas Systems Resolves the Gibbs Paradox

For an ideal gas consisting N molecules within a volume V, the volume accessible to each molecule at an instantaneous time is V/N. The rest of the volume, (N-1)(V/N), is occupied by other (N-1) molecules. The textbook assumption that a molecule can access any location inside the volume V at one instantaneous in time is wrong leading to the Gibbs paradox. By taking into account the correct physical space for individual molecules, the partition function for the N-molecule system is obtained without using any correction factor which gives rise to the correct entropy of the system. There is thus no need to argue about the distinguishability of molecules. Entropy of mixing two quantities of ideal gasses is zero no matter the gasses are the same type or different types. With the appropriate assignment of the phase space, the entropy of the system has the expected property of being extensive and the Gibbs paradox is removed.