Which of the following will produce the lowest osmotic pressure in 0.2 L of water at 305 K?
1.0 g fructose (molar mass 180.2 g/mol)
1.0 g maltose (molar mass 342.3 g/mol)
1.0 g sorbitol (molar mass 182.2 g/mol)
1.0 g xylitol (molar mass 152.2 g/mol)
1.0 g threitol (molar mass 122.1 g/mol)

Which of the following compounds would you expect to be most soluble in H2O?
CH3F
CCl4
CH4
C2H6
CF4

Which of the following would be expected to deviate the most from the normal freezing point of water (0o C)?
1.00 m NaBr
0.50 m Al2(SO4)3
0.75 m NaCl
0.50 m NaF
1.00 m NaCl

The solubility of a gas in H2O at a temperature of 25 °C and a pressure of 1.2 atm is 0.042 M. What will the solubility of the same gas be in H2O at the same temperature at 3.4 atm?

What is the molality (m) of a solution containing 3.62 g of urea (MW 60.06 g/mol) in 513 g of water?
A student performs a kinetics experiment in which they measure the time it takes for a reaction to proceed using a color change for indication. They vary concentrations of one reactant to determine the order of the reaction relative to that reactant. If the student is consistently too slow in stopping their timer when performing their experiment, how will that affect the order they calculate for the reaction with respect to this reactant, and why? Choose from the following:

The reaction order will be too high because the measured rates will be too fas
The reaction order will be too high because the measured rates will be too slow
The reaction order will be too low because the measured rates will be too fast
The reaction order will be too low because the measured rates will be too slow
The reaction order will not be affected, as the errors in the measured rates will even out

A student carries out a kinetics experiment by determining initial rates of reaction at varying concentrations of one reactant (reactant A), while holding the concentration of the other reactant (reactant B) constant. The student later discovers that they had miscalculated their concentration of reactant B, although it was consistent throughout their experiments. How will this affect their calculations? Choose from

It will not affect either the reaction order with respect to A, or the calculated rate constant (k)
It will affect the reaction order with respect to A, but will not affect the calculated rate constant (k)
It will not affect the reaction order with respect to A, but it will affect the calculated rate constant (k)
It will affect both the reaction order with respect to A and the calculated rate constant (k)
It will affect the reaction order with respect to A; the rate constant (k) cannot be calculated with this method

What would be the effect of performing your kinetics experiments at a higher temperature than the one you used? Choose From:

The reaction rate would increase and the order of the reaction with respect to each reactant would increase
The reaction rate would increase and the order of the reaction with respect to each reactant would remain the same
The reaction rate would increase and the order of the reaction with respect to each reactant would decrease
The reaction rate would decrease and the order of the reaction with respect to each reactant would increase
Temperature will not affect the rate of reaction or reaction order

If using freezing point depression to determine the molar mass of an unknown ionic compound, which of the following factors must be known? Choose from:

The shape of each formula unit.
The size of each formula unit.
The number of particles in each formula unit.
The effect of ions on temperature determination.

No additional factors must be known, ionic compounds depress freezing points identically to molecular compounds.

When a student performs a freezing point depression experiment, the calculated molar mass of their unknown sample is lower than all of the possible identities for the sample. Which of the following is the most likely cause of the low molar mass? Choose from below

The volume of solvent used was too high.
The identity of the solvent was not accounted for.
The freezing point of the solute was not accounted for.
The mass of the sample used was too high.
Not all of the sample was dissolved in the solvent.

When determining the freezing point of an unknown compound, which of the following measurements does not need to be taken? Choose from below

The mass of solvent used for determining the freezing point of pure solvent.
The mass of solute used for determining the freezing point of the solvent/solute mixture.
The temperature at which the pure solvent freezes.
The temperature at which the solvent/solute mixture freezes.
The mass of solvent used for determining the freezing point of the solvent/solute mixture.