Glycerol boils at a higher temperature than water. What does this indicate about the attractive forces of glycerol?
2 answers:
Answer: Glycerol has more attractive forces as compared to water.
Explanation:
Boiling point is the temperature at which vapor pressure of the liquid becomes equal to atmospheric pressure.
Boiling point depends on the strength of inter molecular forces.
The molecules of glycerol are more strongly bonded through hydrogen bonds as there are three OH groups.
But in water , only on e OH group is present and thus extent of hydrogen bonding is less.
Thus we can conclude that glycerol has more attractive forces as compared to water.
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Answer: Option (B) is the correct answer.
Explanation:
Degree of randomness of the molecules of a substance is known as entropy. More is the kinetic energy between the molecules of a substance more will be the degree of randomness.
Therefore, when a substance is present in a gaseous state then it has the maximum entropy. In liquid state, molecules are closer to each other so, there is less randomness between them.
On the other hand, in solid state molecules are much more closer to each other as they arr held by strong intermolecular forces of attraction. Therefore, they have very less entropy.
- When liquid water is formed from gaseous hydrogen and oxygen molecules then gas is changing into liquid. So, there is decrease in entropy.
- When
decomposes then the reaction will be as follows.
Since, 1 mole is producing 2 moles. This means that degree of randomness is increasing as both the molecules are present in gaseous form.
- In formation of a precipitate, aqueous solution is changing into solid state. Hence, degree of randomness is decreasing.
- Rusting of iron also leads to the formation of solid as it forms
.
Thus, we can conclude that decomposition of gas to
gas is the process that is expected to have an increase in entropy.