sep interpret data the table compares vapor pressure values for water, ethanol, and diethyl ether at six temperatures. determine the approximate normal boiling point for each substance. what do the data suggest about the relative strength of attraction between particles in each substance?

Question

Accepted Answer

# Brief Explanations:
- **Determining Boiling Points**:
    - The normal boiling point of a liquid is the temperature at which its vapor pressure equals $101.33\ kPa$ (atmospheric pressure).
    - For water, when the vapor pressure reaches $101.33\ kPa$, the temperature is $100^{\circ}C$. So, the boiling point of water is $100^{\circ}C$.
    - For ethanol,  when the vapor pressure reaches $101.33\ kPa$, looking at the table, the corresponding temperature is approximately $78^{\circ}C$ (by observing the trend as the vapor - pressure values approach $101.33\ kPa$).
    - For diethyl ether, since its vapor pressure exceeds $101.33\ kPa$ at relatively low temperatures (e.g., at $35^{\circ}C$ approximately, by interpolation as $24.70\ kPa$ at $0^{\circ}C$, $58.96\ kPa$ at $20^{\circ}C$, and it rises rapidly), its boiling point is around $35^{\circ}C$.
 - **Intermolecular Forces**:
    - Intermolecular forces (such as hydrogen bonding, dipole - dipole forces, and London dispersion forces) affect vapor pressure and boiling points.
    - Substances with stronger intermolecular forces have lower vapor pressures (because it is harder for molecules to escape from the liquid phase to the gas phase) and higher boiling points (more energy is required to overcome the intermolecular forces to convert the liquid to a gas).
    - Water has strong hydrogen bonding. Ethanol also has hydrogen bonding, but fewer hydrogen - bonding sites than water (water has two $O - H$ bonds per molecule for hydrogen bonding, while ethanol has one $O - H$ bond per molecule). Diethyl ether has only dipole - dipole and London dispersion forces (no hydrogen bonding as the $O$ is not directly bonded to $H$).
    - Since water has the highest boiling point ($100^{\circ}C$), it has the strongest intermolecular forces among the three. Ethanol ($bp\approx78^{\circ}C$) has weaker intermolecular forces than water but stronger than diethyl ether. Diethyl ether ($bp\approx35^{\circ}C$) has the weakest intermolecular forces as it has the lowest boiling point and highest vapor pressure at a given temperature (except at very high temperatures for water).

# Answer:
- **Boiling Points**:
    - Water: $100^{\circ}C$
    - Ethanol: Approximately $78^{\circ}C$
    - Diethyl ether: Approximately $35^{\circ}C$
 - **Intermolecular Forces**:
    - The strength of intermolecular forces (attraction between particles) follows the order: Water $>$ Ethanol $>$ Diethyl ether. Water has the strongest intermolecular forces (due to extensive hydrogen bonding), ethanol has moderate intermolecular forces (hydrogen bonding but less than water), and diethyl ether has the weakest intermolecular forces (dominated by weaker dipole - dipole and London dispersion forces).

Sovi.AI - AI Math Tutor

QUESTION IMAGE

Question

Explanation:

Answer: