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Arrange the following compounds in order of increasing vapor pressure: CH3CH2OH, CH3OCH3, CH3CH2CH3.
CH3CH2CH3 < CH3OCH3 < CH3CH2OH
CH3CH2OH < CH3OCH3 < CH3CH2CH3
CH3OCH3 < CH3CH2CH3 < CH3CH2OH
CH3CH2CH3 < CH3CH2OH < CH3OCH3
Which of the following increases with an increase in temperature?
Viscosity
Surface tension
Vapor pressure
Density
At a given temperature, the vapour pressure of pure liquid A is 300 mmHg and that of pure liquid B is 500 mmHg. A solution of A and B shows a total vapour pressure of 400 mmHg. Assuming ideal behavior, what is the mole fraction of A in the liquid phase?
0.2
0.5
0.8
1.0
A solution containing a non-volatile solute exhibits a lower vapor pressure than the pure solvent. This phenomenon can be BEST explained by:
The solute particles increase the intermolecular forces between solvent molecules.
The solute particles decrease the kinetic energy of the solvent molecules.
The solute particles occupy some surface area, reducing the solvent's ability to evaporate.
The solute particles react with the solvent molecules, reducing the amount of solvent available.
A solution is prepared by dissolving 1.8 g of a non-volatile solute in 90 g of water. The vapor pressure of the solution is found to be 23.375 mm Hg at 25°C. If the vapor pressure of pure water at 25°C is 23.76 mm Hg, what is the molar mass of the solute? (Molar mass of water = 18 g/mol)
60 g/mol
180 g/mol
30 g/mol
120 g/mol
A mixture of two volatile liquids A and B follows Raoult's law. At a certain temperature, the partial pressures of A and B above the solution are 200 mmHg and 300 mmHg respectively. If the mole fraction of A in the liquid phase is 0.4, what is the vapor pressure of pure A at this temperature?
500 mmHg
600 mmHg
750 mmHg
1000 mmHg
A solution is prepared by dissolving 20g of a non-volatile solute in 180g of water. If the vapor pressure of pure water at this temperature is 23.76 mmHg and the solution exhibits a vapor pressure of 23.52 mmHg, what is the molar mass of the solute? (Molar mass of water = 18 g/mol)
99 g/mol
198 g/mol
297 g/mol
396 g/mol
Under conditions of high temperature and low humidity, which factor MOST directly exacerbates the transpiration and photosynthesis compromise?
Decreased CO2 concentration
Increased vapor pressure deficit
Reduced soil water potential
Elevated atmospheric pressure
Calculate the vapor pressure of a solution at containing benzene and octane in a molar ratio. The vapor pressures of pure benzene and octane at this temperature are 280 mm Hg and 420 mm Hg, respectively. Assume ideal behavior.
252 mm Hg
336 mm Hg
408 mm Hg
504 mm Hg
A solution is prepared by mixing benzene and toluene at in a molar ratio. If the vapor pressures of pure benzene and toluene at this temperature are 95 mm Hg and 28 mm Hg, respectively, what is the vapor pressure of the solution assuming ideal behavior?
50 mm Hg
72 mm Hg
40 mm Hg
60 mm Hg
