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?

To determine which of the statements are true, we need to consider the concept of vapor pressure and the properties of the substances involved.

1. The vapor pressure of a substance is the pressure exerted by its vapor when it is in equilibrium with its liquid phase at a given temperature. Generally, substances with weaker intermolecular forces have higher vapor pressures.

2. Statement A: The vapor pressure of CO2 is lower than the vapor pressure of water. This statement is true. CO2 has weaker intermolecular forces compared to water, resulting in a lower vapor pressure.

3. Statement B: Sea water has a lower vapor pressure than distilled water. This statement is also true. Sea water contains dissolved salts, such as sodium chloride (NaCl), which increases the boiling point and decreases the vapor pressure compared to distilled water.

4. Statement C: The vapor pressure of 1 m NaCl is higher than the vapor pressure of 0.5 m KNO3, assuming the solvent in each case is water. This statement is false. Both NaCl and KNO3 are ionic compounds that dissociate in water. The higher the concentration of ions, the lower the vapor pressure. Therefore, 0.5 m KNO3 will have a higher vapor pressure than 1 m NaCl.

5. Statement D: The vapor pressure of 1 m sucrose (C12H22O11) is higher than the vapor pressure of 1 m NaCl where the solvent is water. This statement is false. Sucrose is a molecular compound that does not dissociate in water like NaCl. However, sucrose has stronger intermolecular forces compared to NaCl, resulting in a lower vapor pressure.

6. Statement 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. This statement is true. Both NaCl and MgCl2 are ionic compounds, and the vapor pressure depends on the concentration of ions. Since the concentration of ions is higher in 0.10 m NaCl compared to 0.05 m MgCl2, the vapor pressure will be higher for NaCl.

In summary:
- Statements A and B are true.
- Statements C, D, and E are false.