Why is naphthalene (C10H8) more soluble than CsF in benzene?

1.) Are there any intermolecular forces (IMF’s) between water molecules and cyclohexane molecules? What kind(s)? Given this, what would the magnitude and sign of DHMIXING be for cyclohexane dissolving in water?   a) Are there any IMF’s between water molecules and other water molecules? What kind(s)? Given this, what would the magnitude and sign of DHSOLVENT be for cyclohexane dissolving in water?   c) Are there any IMF’s between cyclohexane molecules and other cyclohexane molecules? What kind(s)? Given this, what would the magnitude and sign of DHSOLUTE  be for cyclohexane dissolving in water?   d) Why do you think cyclohexane does not dissolve in water? Analyze this the way it was done in class, thinking about the three contributions to DHSOLUTION. What do you think the magnitude and sign of DHSOLUTION would be for dissolving cyclohexane in water?  (Explain.)  Would you expect these substances to dissolve in each other? Why?

(Q53) For what reason is the solubility of gaseous ammonia (NH3) significantly higher than that of hydrogen gas (H2) at the same temperature and pressure? O Because they are both polar molecules, the solute-solvent interactions are higher between ammonia and water than they are between water and hydrogen gas O Ammonia reacts with water primarily through dispersion forces O Ammonia has a relatively high boiling point O Ammonia has a larger molar mass than does hydrogen gas O Ammonia is an inorganic (carbon-free) molecule

Which compound would you expect to be more soluble in carbon tetrachloride, CH4 or NH3? Explain.