posted by kendra
Which of the following statements is (are) true?
A. The vapor pressure of CO2 is lower than the vapor pressure of water.
B. Sea water has a lower vapor pressure than distilled water.
C. The vapor pressure of 1 m NaCl is higher than the vapor pressure of 0.5 m KNO3, assuming that the solvent in each case is water.
D. The vapor pressure of 1 m sucrose (C12H22O11) is higher than the vapor pressure of 1 m NaCl where the solvent is water.
E. The vapor pressure of 0.10 m NaCl is higher than the vapor pressure of 0.05 m MgCl2, assuming the solvent in each case is water.
What do you think about these. You know A can't be right because CO2 is a gas at room temperature and H2O is a liquid. B certainly is true since
P(soln) = X(solvent)*P(solvent) and sincd X(solvent) is lower for solutions than it is for pure liquid, the vapor pressure of the solution must be less.
why do the water vapor change back to a liuid
Rank these aqueous solutions in order of decreasing freezing point:
1 m Na2SO4
1 m LiF
1.5 m CaCl2
1.5 m glycerol
2 m NH4Cl
4.0 mole of an ideal gas at at temp of _33degree exerts a pressure of 5 atm.what will be its volume in dm at this temp?