The dissolution of water in octane (C8H18) is principally prevented by dipole-dipole attraction between octane molecules hydrogen bonding between water molecules repulsion between like-charged water and octane molecules ion-dipole attraction between water and octane molecules London dispersion forces between octane molecules

At 25.0°C, the Henry’s Law constant for helium (He) gas in water is 3.7×10^-4 M/atm. Calculate the mass in grams of He gas that can be dissolved in 1350. mL of water at 25.0°C and a He partial pressure of 2.14 atm. Round your answer to 2 significant digits.  

Which of the following would lower the freezing point of water the most?     AlCl3 Sugar NaOH NaCl

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?