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We have three states of matter: solid, liquid, and gas.
These are best distinguished on the bases of the degree of attractive forces between the constituent particles.
For gases, the intermolecular forces of attraction is not strong enough to hold the neighboring atoms together. The free spaces between the molecules of gases are very large.
For liquids, intermolecular forces are strong enough to hold the neighboring atoms together but cannot keep them locked in fixed position. Liquid molecules are free to move or slide over one another. The spaces between liquid molecules are less than that of gases.
For this reason for a fixed mass, the volume of gaseous state is larger than that of the liquid state.
The density of liquid NH3 is 0.64 g/mL; the density of gaseous NH3 at STP is 0.0007 g/mL. Explain the difference between the densities of these two phases.
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