Question

Glycerol boils at a higher temperature than water. What does this indicate about the attractive forces of glycerol?

They are nonexistent.
They are the same as those in water.
They are stronger than those in water.
They are weaker than those in water.

Answer 1

The answer to your question is: They are stronger than those in water.

Step-by-step explanation:

When a substance is heated, heat is breaking forces among molecules like hydrogen bonds, london forces, van der waals forces, etc, if a substance has a lot of these forces, the boiling point will be higher because more forces must be broken.Then, glycerol must have stronger forces than those of water.

Answer 2

The correct answer is: "They are stronger than those in water."

Step-by-step explanation:

Intermolecular forces are those that hold the molecules together. Depending on the magnitude of these forces it will cost more or less to separate the molecules. That is what happens with the boiling point. The boiling point is the temperature at which a liquid leaves its state and enters the gaseous state (vapor). Then the intermolecular forces, which are greater in a liquid state with respect to the gaseous state, have to be broken so that the change of state can occur. The higher the intermolecular forces present in the liquid, the boiling point will be higher.

So, since glycerol has a boiling point higher than water, it indicates that the intermolecular forces will be greater, since it takes more temperature and energy to break the force that bonds the molecules.

So the correct answer is: "They are stronger than those in water."