Statement I: At the same temperature, water has higher vapour pressure than acetic acid.

Statement II: Hydrogen bonding in water is weaker than in acetic acid.

Statement I is correct but Statement II is false

The correct answer is option 3. Statement I is correct but Statement II is false.

Let us analyze each statement about water and acetic acid:

Statement I: At the same temperature, water has higher vapor pressure than acetic acid.

Vapor pressure is the pressure exerted by a vapor in thermodynamic equilibrium with its condensed phases (solid or liquid) at a given temperature in a closed system. Water typically has a higher vapor pressure compared to acetic acid at the same temperature. This is because water molecules have stronger intermolecular forces (hydrogen bonding) compared to acetic acid, leading to easier escape of water molecules into the vapor phase.

Statement II: Hydrogen bonding in water is weaker than in acetic acid.

Hydrogen bonding occurs between hydrogen atoms attached to highly electronegative atoms (like oxygen or nitrogen) and other electronegative atoms. This statement is false. Hydrogen bonding in water is actually stronger than in acetic acid. Water molecules can form extensive networks of hydrogen bonds due to their ability to donate and accept hydrogen bonds from neighboring water molecules. Acetic acid also exhibits hydrogen bonding, but to a lesser exAnalysis of Statements:

Statement I is correct: Water does have a higher vapor pressure than acetic acid at the same temperature due to weaker intermolecular forces (hydrogen bonding) in acetic acid compared to water.

Statement II is false: Hydrogen bonding in water is stronger, not weaker, than in acetic acid.

Conclusion: Therefore, the correct assessment of the statements is: Statement I is correct but Statement II is false.