7. Based on your response to the previous question, why do you think the dissolution of urea is an endothermic process? Your response should include two parts:

i) How do the three sets of attractive forces (solvent-solvent, solute-solute, and solvent-solute) compare in magnitude for the dissolution process to be endothermic?

ii) Compare the intermolecular (IM) forces present in each set to predict why such a difference in the amount of attractive forces exists.

Question

01-07-2024
Chemistry

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7. Based on your response to the previous question, why do you think the dissolution of urea is an endothermic process? Your response should include two parts:

i) How do the three sets of attractive forces (solvent-solvent, solute-solute, and solvent-solute) compare in magnitude for the dissolution process to be endothermic?

ii) Compare the intermolecular (IM) forces present in each set to predict why such a difference in the amount of attractive forces exists.

Sagot :

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GinnyAnswer GinnyAnswer · Answer 1 · 2024-07-01T14:16:14-04:00

Final answer:

The dissolution of urea in water is an endothermic process due to the energy needed to overcome the attractive forces between solute-solute and solvent-solvent interactions before solute-solvent attractions are established.

Explanation:

In a solution, the dissolution process of urea is endothermic because energy is required to overcome the attractive forces between solute-solute and solvent-solvent interactions before solute-solvent attractions are established. The relative magnitudes of these energy changes determine whether the dissolution process will release or absorb energy. For urea dissolution in water, the energy consumed to break solute-solute and solvent-solvent attractions is greater than the energy released by solvation, resulting in an endothermic process.

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