1. Osmotic pressure = imRT where m = molality of solute, R = molar gas constant, T = temperature and i = van\'t Hoff factor. i is a measure of how many particles each particle of solute dissociates into. ethylene glycol which is a non-electrolyte, i = 1 acetic acid (weak electrolyte with partial dissociation int H+ and acetate), 1 < i < 2 and NaCl (strong electrolyte with complete dissociation intp Na+ and Cl-), i = 2 So the osmotic pressure of ethylene glycol < acetic acid < NaCl for the same molality of solute 2. Vapor pressure depends on the strength of the intermolecular bonding between molecules. The weaker the intermolecular bonds, the more easily the molecules escape into the gas phase and the higher the vapor pressure. For BrF3. PF5 and CF4 are all molecular compounds held together by intermolecular van del Waal\'s (dispersion) forces, which increase with molecular weight. So in terms of intermolecular bond strength, BrF3 > PF5 > CF4, and the vapor pressures are BrF3 < PF5 Solution 1. Osmotic pressure = imRT where m = molality of solute, R = molar gas constant, T = temperature and i = van\'t Hoff factor. i is a measure of how many particles each particle of solute dissociates into. ethylene glycol which is a non-electrolyte, i = 1 acetic acid (weak electrolyte with partial dissociation int H+ and acetate), 1 < i < 2 and NaCl (strong electrolyte with complete dissociation intp Na+ and Cl-), i = 2 So the osmotic pressure of ethylene glycol < acetic acid < NaCl for the same molality of solute 2. Vapor pressure depends on the strength of the intermolecular bonding between molecules. The weaker the intermolecular bonds, the more easily the molecules escape into the gas phase and the higher the vapor pressure. For BrF3. PF5 and CF4 are all molecular compounds held together by intermolecular van del Waal\'s (dispersion) forces, which increase with molecular weight. So in terms of intermolecular bond strength, BrF3 > PF5 > CF4, and the vapor pressures are BrF3 < PF5.

1. 1. Osmotic pressure = imRT
where m = molality of solute, R = molar gas constant, T = temperature and i = van't Hoff factor.
i is a measure of how many particles each particle of solute dissociates into.
ethylene glycol which is a non-electrolyte, i = 1
acetic acid (weak electrolyte with partial dissociation int H+ and acetate), 1 < i < 2
and NaCl (strong electrolyte with complete dissociation intp Na+ and Cl-), i = 2
So the osmotic pressure of ethylene glycol < acetic acid < NaCl for the same molality of solute
2. Vapor pressure depends on the strength of the intermolecular bonding between molecules. The
weaker the intermolecular bonds, the more easily the molecules escape into the gas phase and the
higher the vapor pressure.
For BrF3. PF5 and CF4 are all molecular compounds held together by intermolecular van del
Waal's (dispersion) forces, which increase with molecular weight.
So in terms of intermolecular bond strength, BrF3 > PF5 > CF4, and the vapor pressures are
BrF3 < PF5
Solution
1. Osmotic pressure = imRT
where m = molality of solute, R = molar gas constant, T = temperature and i = van't Hoff factor.
i is a measure of how many particles each particle of solute dissociates into.
ethylene glycol which is a non-electrolyte, i = 1
acetic acid (weak electrolyte with partial dissociation int H+ and acetate), 1 < i < 2
and NaCl (strong electrolyte with complete dissociation intp Na+ and Cl-), i = 2
So the osmotic pressure of ethylene glycol < acetic acid < NaCl for the same molality of solute
2. Vapor pressure depends on the strength of the intermolecular bonding between molecules. The
weaker the intermolecular bonds, the more easily the molecules escape into the gas phase and the
higher the vapor pressure.
For BrF3. PF5 and CF4 are all molecular compounds held together by intermolecular van del
Waal's (dispersion) forces, which increase with molecular weight.
So in terms of intermolecular bond strength, BrF3 > PF5 > CF4, and the vapor pressures are
BrF3 < PF5