Which of the following statements are correct?
(Select all correct answers.)
Breaking the bonds between the solute molecules is an endothermic process
Breaking the bonds between the solvent molecules is an endothermic process
Formation of the solvent-solute bond is exothermic
Overall the Gibbs free energy for the dissolution process is always endothermic
Overall the Gibbs free energy for the dissolution process is always exothermic
Larry, Nataly, Maria, et al. These look like pre-lab questions to an experiment. All of this is discussed in your notes, in your text, or in your lab manual. Posting here will not get them answered freebie style. If you pose specific questions, tell us what you think, and/or what you don't understand, perhaps we can put you on the right path.
To determine which statements are correct, let's break down each one and analyze the processes involved:
1. Breaking the bonds between the solute molecules is an endothermic process:
This statement is generally true. When the bonds between solute molecules are broken, it requires an input of energy (heat) to overcome the attractive forces between the molecules. Breaking bonds is typically an endothermic process.
2. Breaking the bonds between the solvent molecules is an endothermic process:
This statement is generally true as well. Similar to the previous statement, breaking the bonds between solvent molecules also requires an input of energy to overcome the attractive forces between them.
3. Formation of the solvent-solute bond is exothermic:
This statement is generally true. When the solute molecules interact with the solvent molecules and form new bonds, energy is released, resulting in an exothermic process. This energy release occurs due to the formation of favorable solute-solvent interactions.
4. Overall, the Gibbs free energy for the dissolution process is always endothermic:
This statement is incorrect. The Gibbs free energy (ΔG) for the dissolution process depends on various factors, including the temperature, pressure, and the nature of the solute and solvent. It can be both endothermic or exothermic, depending on the specific conditions. The sign of ΔG determines the spontaneity of the process, but it does not necessarily indicate whether the process is endothermic or exothermic.
5. Overall, the Gibbs free energy for the dissolution process is always exothermic:
This statement is also incorrect since the Gibbs free energy for the dissolution process can be either endothermic or exothermic, as explained in the previous statement.
In summary, the correct statements are:
- Breaking the bonds between the solute molecules is an endothermic process.
- Breaking the bonds between the solvent molecules is an endothermic process.
- Formation of the solvent-solute bond is exothermic.